0 liter container. H2 (g) + I2 (g) ↔ 2 HI (g). Assumptions 1 The equilibrium composition consists of CO2, CO, O2, and N2. 3 " 10#3 K ! = 160 6. 2CO2 (g) 2CO (g) + O2 (g) DHe = -514 kJ. The reaction CO(g)+H2O(g)-->CO2(g)+H2(g) has the equilibrium constant kp of 23. NH3(g) <-> 3/2 H2(g) + 1/2 N2(g) 5. If two or more reactions are added to give another, the equilibrium constant for the reaction is the product of the equilibrium constants of the equations added. Once you know how many of each type of. The reaction was started with 0. 2CO (g) + O2 (g) ⇄ 2CO2 (g) + energy. Initially, two moles of CO and one mole of H2O were mixed in a 1. Calculate the equilibrium constant for the reaction given the equation below : (4 marks) 2 NH3 (g)  N2 (g) + 3 H2 (g) 3. However, above pH 11, the hydration reaction is relatively rapid as carbon dioxide reacts directly with. 50 moles of N 2 gas is mixed with 0. Write the expression for K for the reaction below. The model solutions describe that, at standard physiological conditions, the hemoglobin is about 97. Carbon monoxide reaches equilibrium with water vapour as they react to form hydrogen gas and carbon dioxide gas. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 0 L, to get the equilibrium concentration of CO2. !!equilibrium. Equilibrium Reaction Calculator. Aqueous carbon dioxide reacts to form carbonic acid via the following reaction: 2 0. Replace immutable groups in compounds to avoid ambiguity. May 04,2020 - The equilibrium constant for the reaction co+H2O=co2+H2 at a certain temperature is 2. Reaction Information. 2 "The Equilibrium Constant" that the equilibrium constant for the decomposition of CaCO 3 (s) to CaO(s) and CO 2 (g) is K = [CO 2]. Concentrations or gas pressures of reactants and products at equilibrium can be calculated from the initial concentrations or gas pressures of reactants and products and equilibrium constants. 35  10-5 and 8. 80 moles of H2 and 0. Based on the molarities of reactants and products at equilibrium. Not only Henry constant but also dissociation constants have to be used. 94 x 10^54)^1/2 = 1. 000355 Atmosphere. Carbon Monoxide Poisoning. equilibrium constant tells you that at equilibrium the concentrations of products will be much larger than the concentrations of reactants. 00mol each of carbon monoxide and water in a 50. 2(aq)][ CO. The equilibrium constant for is K' = [HCO3-]2/PCO2[CO32-] = KHK1/K2. aA(g) + bB(g) ⇄ cC(g) + dD(g) the pressure-based equilibrium constant, K P, is defined as follows: where P A is the partial pressure of substance A at equilibrium in atmospheres, and so. A third reaction 2 CO <=> C + CO2 (carbon dusting) also occurs if you operate in a range where it is favored by equilibrium. Chapter 13 Fundamental Equilibrium Concepts Figure 13. 72 T (J) or (-135194 + 41. Consider the reaction 2 CO2 ⇔ 2 CO + O2 obtained after heating 1 kmol CO2 to 3000 K. CH40S Chemical Equilibrium Unit Review Part A: Multiple Choice 1. 5xFrom Table A-28, ln K p = −17. 18 a-d) Write equilibrium constants. Justify your prediction. 0908 moles of H 2, 0. reacting species at equilibrium are found to be [NO] = 0. CO+O2=O+CO2. Department of Commerce National Bureau of Standards RESEARCH PAPER RP1634 Part of Journal of Research of the Rational Bureau of Standards, Volume 34 February 1945 HEATS, FREE ENERGIES, AND EQUILIBRIUM CONSTANTS OF SOME REACTIONS INVOLVING 2 , H 2. The equilibrium constant for is K' = [HCO3-]2/PCO2[CO32-] = KHK1/K2. 1M each of CO and H2O at 800K. Not only Henry constant but also dissociation constants have to be used. 88 atm) 2 = 15. 1Chemical Equilibria 13. Chemists usually simply say that "the equilibrium shifts to the left". There are many variations of this procedure, but because our goal is only to introduce you to this category. RefractiveIndex. The system will subsequently experience a net reaction in the direction of. The bottom arrow points to the left. 22 mol of water vapour are combined in a 1. iv) Raising the temperature would shift the equilibrium to the right. If the constant is grater than one there are more. 5 O2 X 1 CO X1 CO2 = 1 K1 (8) Using equations (6, 7 and 8), it is now possible to derive a simple. 45 mol of carbon monoxide and 2. (ii) State how increasing the pressure of the reaction mixture at constant temperature will affect the position of equilibrium and the value of K c. This value is 0. the carbon dioxide gas dissolved in it fizzes out rapidly. CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g) Calculate the value of the equilibrium constant. Carbon monoxide is toxic because it bonds much more strongly to the iron in hemoglobin (Hgb) than does O2. 1%) of CO 2 (aq) as H 2 CO 3. low temperature carbon dioxide does not react with carbon to produce carbon monoxide. 2CO2(g)+2H2O(l)⇌CH3COOH(l)+2O2(g), K1 = 5. K p = P water(g) x P carbon dioxide(g) = (3. At this temperature, Kc equals 1. On a mass fraction basis, the inhibiting effect on the carbon dioxide hydrate. 0 M and the concentration of O2 is 9. 2 Equilibrium Constants At the end of the lesson, students should be able to: (a) Define homogeneous and heterogeneous equilibria. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. When ammonium carbamate crystals, NH4CONH, are placed into a container. At equilibrium, Q = K, and δ G = 0. 47) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. This means that the ratio of oxygen to ozone in given by: If we know the equilibrium concentration of oxygen, we can solve for the equilibrium constant of ozone. In the table below are data that show the percent of CO in the equilibrium mixture at two different temperatures. Carbon monoxide (CO) reacts with haemoglobin in the same way as oxygen: Hb(aq) + CO(aq) ⇋ HbCO(aq) OR Hb 4 (aq) + 4CO(aq) ⇋ Hb 4 (CO) 4 (aq). 2CO (g) + O2 (g) ⇄ 2CO2 (g) + energy. 30 M before they are mixed and when equilibrium is reached, the equilibrium concentration of A2D is 0. ZnO(s) + CO(g) ⇌ Zn(s) +CO2(g) Find the value of the equilibrium constant: H2 (g) + CO2 (g) ↔ CO(g) + H2O (g) The equilibrium concentrations are found to be [H2] = 0. org are unblocked. 500 mole of carbon monoxide and 0. 000 moles, [O2]eq = 4. May 04,2020 - The equilibrium constant for the reaction co+H2O=co2+H2 at a certain temperature is 2. View Test Prep - quiz. This value is 0. NH3(g) <-> 3/2 H2(g) + 1/2 N2(g) 5. At 2000°C, the Keq for the decomposition of carbon dioxide gas to carbon monoxide and oxygen gases is 6. A solution of Co2+ ions in water containing hydrochloric acid is a system that involves the following equilibrium: Co(H2O)62+(aq) + 4 Cl-(aq) CoCl42-(aq) + 6H2O(l) The Co(H2O)62+ ion is pink, whereas the CoCl42- ion is blue (for your information, a solid-phase version of this reaction is commonly used as a visual indicator of humidity levels in. At 250oC the equilibrium constant for the following gaseous reaction is 0. In one experiment, the following equilibrium concentrations were measured. Calculate [CO2] at equilibrium when [CO] = for Teachers for Schools for Working Scholars. 3 × 10-3 atm, P (CO2)eq = 0. The initial moles of CO, H2O, CO2 and H 2 are 2, 5, 0 and 2 moles respectively. Removing $\ce{CO2}$ produce that $\ce{CO}$ react with $\ce{O2}$ to produce more $\ce{CO2}$. If you're behind a web filter, please make sure that the domains *. 00 L container and allowed to come to equilibrium. Calculate the equilibrium constant (KC) of the reaction at this temperature. It is the reaction of Coke (carbon) with CO2 giving CO (carbon monoxide). 00 x 10^5 x 2. Carbon dioxide does dissolve in water, however the system is somewhat complex[1]. the concentration of all dissolved CO2 by [H2CO3]. 21 mol/mol, and argon (Ar) with CAr = 0. The equilibrium constant for the following reaction is 600(C is 4. 352 moles of H2O is heated to 700°C in a 10. Question: Consider the reaction, NH4CO2NH2(s)<---. 19 mol of CO remaining. If an equilibrium system is subjected to a change in conditions that affects these reaction rates differently (a stress), then the rates are no longer equal and the system is not at equilibrium. 8 KJ/mol Estimate The Value Of The Equilibrium Constant At 625 K For The Following Reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g)2 CO(g) + O2(g) ⇌ 2 CO2(g). 8 KJ/mol -25. At this temperature, K c equals 1. Use uppercase for the first character in the element and lowercase for the second character. 0020 M Solved If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture conta. Assuming that the exhaust gas (total pressure 1 atm) by volume contains 0. Calculate the equilibrium [O2] in this mixture. 2 mol is for CO, not for CO2. 12 atm H2O, 0. Consider the following equilibrium system: O 2(g) + 2HF (g) ⇌ OF. asked by josh on February 26, 2010; Physical Chemistry. 1 Since CO 2 is an acid (i. If the equations of reactions are added, the equilibrium constant of the resulting reaction is obtained by multiplying the equilibrium constants of the reactions added. In both cases just as much CO 2 or O 2 is added or removed from the water until the preset pCO2 or pe value is reached. Equilibrium Constant. Write an expression for the equilibrium constant for this reaction. Results are recorded in the table below. For a reaction made up of two or more steps, the equilibrium constant for the net. 55% CO by mass. A solution of Co2+ ions in water containing hydrochloric acid is a system that involves the following equilibrium: Co(H2O)62+(aq) + 4 Cl-(aq) CoCl42-(aq) + 6H2O(l) The Co(H2O)62+ ion is pink, whereas the CoCl42- ion is blue (for your information, a solid-phase version of this reaction is commonly used as a visual indicator of humidity levels in. Introduction. First, be sure to count all of C and O atoms on each side of the chemical equation. The overall equation would be multiplied by 1/c. The equilibrium constant at 25°C is K h = 1. 12 atm H2O, 0. 2Equilibrium Constants 13. Find the equilibrium constant for this reaction at 850 C. 7 × 10-2 M, and CO2 was measured to be 1. The equilibrium constant is the value of the reaction quotient that is calculated from the expression for chemical equilibrium. Calculating an Equilibrium Constant from Equilibrium Concentrations. 2 "The Equilibrium Constant" that the equilibrium constant for the decomposition of CaCO 3 (s) to CaO(s) and CO 2 (g) is K = [CO 2]. 27) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Calculate the equilibrium partial pressures of CO2, H2 and CO. 50 moles of N 2 gas is mixed with 0. 0010 M CO2 and 0. 86 moles of O 2 gas in a 2. 13) + 1(-393. The amount that dissolves at a particular temperature depends on the pressure, or partial pressure, of the gas. What is the equilibrium constant, K, for the following reaction, if the concentration of CO was measured to be 3. 22 mol of CO remaining. The system was prepared with [NH3] = [O2] = 3. Calculate the equilibrium partial pressure of CO2. 2 CO(g) + O2(g) = 2 CO2(g) b. rate is kept low enough that equilibrium will be attained, and analysis of the effluent gas gives the data necessary for calculation of the equilibrium constant. Reversible Reactions and Chemical Equilibrium At high temperatures, carbon dioxide gas decomposes into carbon monoxide and oxygen gas. We also use published experimental data to find similar thermodynamic properties of CO 2 (g) and of CH 4 (g) adsorbed on activated carbon. 8 KJ/mol Estimate The Value Of The Equilibrium Constant At 625 K For The Following Reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g)2 CO(g) + O2(g) ⇌ 2 CO2(g). RefractiveIndex. The CO placed in the vessel is labelled with 14C. 21 x 1020 C) 3. CO-L container and the system was allowed to come to equilibrium. Analysis The stoichiometric and actual reactions in this case are. A mixture of 0. 2748 P_H2 = 2. 0 x 10-2 M [H2] = 3. The equilibrium constant for reaction (1) below is K. But the equilibrium constant is too small for you to see any measurable change in pH of the water. 00 x 10^5 x 2. 0010 M CO2 and 0. At equilibrium, Q = K, and δ G = 0. 1% saturated by CO2. In an open system, the partial pressure of CO 2 (g) is relatively constant at P(CO 2) = 0. An acid dissociation constant, K a, is the equilibrium constant for the dissociation of an acid in aqueous solution. K 1 , K 2 , etc. 35 mol of CO and 0. 1k points) equilibrium. The number of moles of H2, S2, and H2S present at the equilibrium for the reaction are 2. 1) For the reaction CO(g) + 3H 2(g) CH 4(g) + H 2O(g) ΔHo = -206. Carbon dioxide does dissolve in water, however the system is somewhat complex[1]. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. 0010 M CO2 and 0. It would not change because the amount of solid present at equilibrium is not important as long as there is some solid present. Consider the following reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kp=0. 2no 2 ( g ). 0908 moles of H 2, 0. 0 x 10-2 M [H2] = 3. The effect of temperature on the extent of the Boudouard reaction is indicated better by the value of the equilibrium constant than by the standard free energy of reaction. Introduction. CHEMICAL EQUILIBRIUM. WRITING THE EQUILIBRIUM EXPRESSION. What is the correct equilibrium constant expression for this equation? 2C0F,(g) CO2(g) + CF_(g) Get the answers you need, now!. Generally omit the. We know that at equilibrium, the value of the reaction quotient of any reaction is equal to its equilibrium constant. Calculating an Equilibrium Constant from Equilibrium Concentrations. Briefly account for. Given [Ca21]o 5 1 mM, [Ca21 ]i 5 100 nM, find ECa21 b. increasing the volume D. d) decrease the value of the equilibrium constant. It is due to the property of pressure being disrupted in this system that causes a sudden decrease of oxygen that cannot be reimbursed. The following equilibrium is established at 500K: CO2(g) + H2(g) CO(g) + H2O (g) a) calculate the initial partial pressures of CO2, H2 and H2O. A mixture of 0. 5, calculate Kc for Reaction 2 CO2(g)␣CO(g) + 1/2O2(g) how do i calculate kc?. Hi! Can somebody please help me? At 1200 K, the approximate temperature of vehicle exhaust gases, Kp for the reaction 2CO2(g) -> <- 2CO(g) + O2(g) is about 1 E-13. Section 5- Carbonate Chemistry CASE 1 CO 2 - H 2 O open system Aqueous carbon dioxide reacts to form carbonic acid via the following reaction: 2 0. 97 H2(g) + CO2(g) <–> H20(g) + CO(g) Kp2 = 0. 5 mole of CO2 and 0. 35  10-5 and 8. The overall reaction is: CO2 (g) + 2 NH3 (g) ⇔ NH4CO2NH2 (s) (5) In this experiment the thermodynamic properties of the reve rse reaction, the d ecomposition of ammoni um carbamate, will. Equilibrium Constant • If the reaction involves a pure solid or pure liquid, these species do not appear in the equilibrium constant expression: Example: CH 4(g) + H 2O(l) CO(g) + 3 H 2(g) KC = [CO(g)] [H2(g)] 3 [CH4 (g)] Note that H 2O(l) does not appear in the denominator. 300 mol Br2, and 0. 0 liter container. Question: Consider the reaction, NH4CO2NH2(s)<---. 2 CO(g) + O2(g) = 2 CO2(g) b. 7 x 10-2 M [NH3] = 1. At 750°C, the Kp for the reaction 2 CO + O2 2 CO2 is 2. The moles of CO, H2O , CO2 and H2 present at equilibrium are 2-x, 5-x, ,x and 2+x moles respectively. For example, at the same temperature, the above reaction may have a different set of concentrations and another equilibrium position, such as, [SO2] = 0. Equilibrium 8 Pressure Equilibrium Constants K is the general symbol for equilibrium constant K c is the equilibrium constant defined by concentrations K p is the equilibrium constant defined by partial pressures Below shows how K c and K p are defined for same reaction For reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) K c = [NH 3] 2 / [N 2] [H 2] 3 K. PHYSICAL CHEMISTRY By: Shailendra Kumar 1. A)increase the partial pressure of O2(g) B)decrease the value of the equilibrium constant C)increase the partial pressure of CO D)decrease the partial pressure of CO2(g) E)increase the value of the equilibrium constant 16) Consider the following reaction at equilibrium. CO-L container and the system was allowed to come to equilibrium. Justify your prediction. 4 atm and CO2 p = 0. Consider the reaction: S (s) + O2 (g) CO2 (g) Ka b. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. Reactions don't stop when they come to equilibrium. The equilibrium constant {eq}\left( {{K_{\rm{p}}}} \right) {/eq} is a value determined by taking the ratio of partial pressures of all the gaseous products to the partial. The equilibrium composition is to be determined. 7 × 10-2 M, and CO2 was measured to be 1. RefractiveIndex. 23) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. K' = K 1 x K 2. 003 5 atm of chlorine at 600°C. CO/CO2 Ratio Grid Lines Oxygen partial pressure in a system can also be controlled using the CO-CO2-O2 equilibrium. h 2 o ( g ). CO+OH=H+CO2. Predict the sign for the change in entropy, (S, for the reaction. Keq = (H2O) (CO) / (H2) (CO2) Pretty sure it's called it's Boiling Point. 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). Link to: Dissociation of CO2 to CO and O2 Applet Link to: Dissociation of N2 and O2 to NO Applet. equilibrium is a state in which. 0 L reaction vessel. Subtracting 3/2 from 2 gives us 1/2 O2, which matches with the final equation. 2 mol/L, [CO (g)] = 0. For a reaction made up of two or more steps, the equilibrium constant for the net. 0010 M CO2 and 0. When equilibrium was reached, there was still some C(s) remaining in the container. Use data from Appendix IIB to calculate the equilibrium constants at 25°C for each reaction. 2 CO(g) + O2(g) = 2 CO2(g) b. This equilibrium competition method is the first report of direct measurement of equilibrium constants for O 2 and CO binding to Hbs with dissociation equilibrium constants in the nM range. Determine the value of the equilibrium constant, Kgoal, for the reaction N2(g)+O2(g)+H2(g)⇌12N2H4(g)+NO2(g), Kgoal=? by making use of the following information: 1. At 1000 K, a sample of pure NO2 gas decomposes. 00 L flask, equilibrium is established. CO(g) + 1/2 O2(g) CO(g)Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a. 00-L reaction vessel. So basically you can say those are a constant, so that would mean that then the solids and the liquids are not included in the equilibrium expression. The equilibrium constant for reaction (1) below is K. Some reactions convert reactants to products with near 100% efficiency but others do not. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. Consider the reaction: C(s) + O2(g)---> CO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a. 6 Heterogeneous Equilibria • 14. In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H 2 O (g) ↔ CO 2 (g) + H 2 (g) In an experiment, 0. Problems - Chapter 15 (with solutions) 1) What is the significance of the equilibrium constant? What does a large equilibrium constant tell us about a reaction? A small one? The equilibrium constant tells you the relationship between product and reactant CO) (p O2) [CO 2] 2 (p CO2) b) K C 2= [O 3]2 K p = (p O3) [O 2]3 (p O2)3 c) K C = [COCl. Increase in concentration => increase in rate Decrease in concentration => decrease in rate If you increase the concentration of the reactants, the forward reaction rate increases and the equillibrium shifts to the right. (1) The equilibrium constant, K, is much stronger in haemoglobin-carbon monoxide reaction compared to the haemoglobin-oxygen reaction which means that the haemoglobin puts priority on carbon monoxide bonds, therefore the haemoglobin that has bonded with carbon monoxide is no longer available for oxygen. The initial moles of CO, H2O, CO2 and H 2 are 2, 5, 0 and 2 moles respectively. 000355 Atmosphere. equilibrium constant tells you that at equilibrium the concentrations of products will be much larger than the concentrations of reactants. 352 moles of H2O is heated to 700°C in a 10. Consider the following reactions and approximate free energy changes: Hgb + O2 —> HgbO2 ∆G⁰ = -70 kJ Hgb + CO —> HgbCO ∆G⁰ = -80 kJ Using these data, estimate the equilibrium constant value at …. The first acid constant accounts for the relatively small fraction (~0. 3 M), CO2 in liquid is practically zero and so is partial CO2 gas pressure at equilibrium. Also, the pressure of CO2 is given, and therefore, first we solve for Kp and then solve for Kc. ) C(s) + O2(g) Get more help from Chegg. If one has a mixture that is initially composed of 0. 4 kPa, amine concentration of 2 mol·L −1 and the second-order reaction constant was determined at 298 K , , , ,. Carbon Dioxide (CO 2) CO2 Carbonic Acid Gas Dry Ice [CO2. 0010 M CO2 and 0. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following 11) reaction:CO (g) + H2O (g) CO2 (g) + H2 (g)In an experiment, 0. 0200 mol COBr2 is sealed in a 5. CO2(g) + C(graphite) ⇌ 2 CO(g)-The equilibrium constant will increase. 00-L reaction vessel. 0908 moles of H 2, 0. This equation says that CO 2 can be converted to a mixture of CO and O2, while CO plus O2 can convert to CO 2. The equilibrium constant for an. Purchase CO2 in Seawater: Equilibrium, Kinetics, Isotopes, Volume 65 - 1st Edition. 37 (a) Write the expression for the equilibrium constant, K p, for the reaction. Initially, two moles of CO and one mole of H2O were mixed in a 1. [ch3oh]^1/2[co]^1/2 / [c)[h2][o2]1/2 = (2. Equilibrium Constant. Acetic acid is a weak electrolyte because ; The free energy for a reversible reaction at equilibrium is ; In any chemical reaction, equilibrium is supposed to be established when. reacting species at equilibrium are found to be [NO] = 0. Use uppercase for the first character in the element and lowercase for the second character. The Le Châtelier principle states that the net reaction will be in a direction that tends to reduce the effect of the added H 2. (a) Calculate the partial pressure of phosgene that is in equilibrium with a mixture of 0. 00 moles each of H2(g) and CO2(g) are placed in a 1. 50 mol of H2O 7. 00mol each of carbon monoxide and water in a 50. 40 x 10^2 x 1. 12 atm CO, 0. If we raise the temperature we add more heat to this equilibrium reaction. Suppose that an air mixture becomes polluted with carbon monoxide at a level of 0. 45 mol of carbon monoxide and 2. 27) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 1 kJ and ΔSo = -214. 00-L reaction vessel. Hence, the majority of the carbon dioxide is not converted into carbonic acid, remaining as CO 2 molecules. N2 and O2. -The equilibrium constant will decrease. Heterogeneous equilibria implies that not all species are in the same state, that is there might be some species in gaseous state, others in aqueous and others in solid. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Find ΔHorxn For The Reaction. Equilibrium 8 Pressure Equilibrium Constants K is the general symbol for equilibrium constant K c is the equilibrium constant defined by concentrations K p is the equilibrium constant defined by partial pressures Below shows how K c and K p are defined for same reaction For reaction: N 2 (g) + 3H 2 (g) 2NH 3 (g) K c = [NH 3] 2 / [N 2] [H 2] 3 K. So now cancel the H2Os as they are on opposite sides and. N2(g)+O2(g)⇌2NO(g), K1 = 4. A chemical engineering view of a fullscale carbon dioxide absorber. -The reaction will shift to the right in the direction of products. 2CO(g) + O2(g) <----> 2CO2(g) K = (1 / 2. 0908 moles of H 2, 0. Chemical Equilibrium. 28 x 10-21 The equilibrium constant is related to the change in the standard Gibbs Free Energy for a reaction: Go rxn = H o rxn - T S o rxn = - RT ln Keq. CARBON C + O2 = CO2 Mass ratio 12 + 32 = 44 Hence 1kg of C needs 32/12kg of O2 and makes 44/12kg of CO2 HYDROGEN 2H2 + O2 = 2H2O Mass ratio 4 + 32 = 36 Hence 1kg of H2 needs 8kg of O2 and makes 9 kg of H2O SULPHUR S + O2= SO2 32+32 = 64 Hence 1 kg of S needs 1kg of O2 and makes 2kg of SO2. The initial moles of CO, H2O, CO2 and H 2 are 2, 5, 0 and 2 moles respectively. 6 x 10-2 M, calculate the equilibrium constant, Kc Kc = 1. Calculate Δ*G*° for each of the following reactions from the equilibrium constant at the temperature given. a)i) Calculate the amounts, in moles, of methane, steam and hydrogen in the equilibrium mixture. 8 KJ/mol -48. 0010 M CO2 and 0. The equilibrium constant K p = 2. low temperature carbon dioxide does not react with carbon to produce carbon monoxide. 0 L, to get the equilibrium concentration of CO2. , CO 2 (gas) ⇌CO 2(in solution) This equilibrium is governed by. -No effect will be observed since C is not included in the equilibrium expression. At equilibrium, there were 0. 2CH 4(g) C 2H 2(g) + 3H 2(g) While studying this reaction mixture, a chemist analysed a 4. 12 atm CO, 0. Equilibrium Constant. 640, the equilibrium constant for the reaction under these conditions. Keq = (H2O) (CO) / (H2) (CO2) Pretty sure it's called it's Boiling Point. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. CHEMICAL EQUILIBRIUM Chapter 16 a A + b B 'c C + d D K = [C]c [D]d [A]a [B]b conc. Keq at the temperature of the experiment is _____. 6 Heterogeneous Equilibria • 14. CO(g) + H2O(g) ( CO2 (g) + H2 (g) Initial 2. Write the equilibrium equation for each of the following reactions: a) 2 SO2(g) + O2(g) 2 SO3(g) b) 2 SO3(g) 2 SO2(g) + O2(g) The following equilibrium concentrations were measured at 800 K: [SO2] = 3. At 100°C the equilibrium constant for the reaction COCl 2 (g) CO(g) + Cl 2 (g) has the value of K eq = 2. 7 L container. The number of moles of H2, S2, and H2S present at the equilibrium for the reaction are 2. If, at equilibrium, the concentration of CO2 is 3. 19 mol of CO remaining. Similar Questions. For atmospheric pressure of CO. Multiple Choice 48. ) C(s) + O2(g) Get more help from Chegg. 14) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. 2(aq)][ CO. Consider the following equilibrium system: O 2(g) + 2HF (g) ⇌ OF 2(g) H = +318 kJ/mol If the temperature of the system is increased, A. In an open system, the partial pressure of CO 2 (g) is relatively constant at P (CO 2) = 0. 00-L reaction vessel. Mahual Kothi, Alpana Market, Patna Page No. Balance Chemical Equations with this Calculator and view a list of previously balanced equations beginning with F 2Fe + O2 = 2FeO: Fe2O3 + CO = Fe + CO2: Fe2O3. rate is kept low enough that equilibrium will be attained, and analysis of the effluent gas gives the data necessary for calculation of the equilibrium constant. Write the expression for K for the reaction below. At a constant temperature the ratio of : CO 2 dissolved in water / CO 2 in the air is constant at a constant temperature - the so-called equilibrium constant. Note that we could have solved for the amount of NO produced rather than. 9), including one proportionality. equilibrium constant tells you that at equilibrium the concentrations of products will be much larger than the concentrations of reactants. equilibrium constant? 1. Find the equilibrium constant for this reaction at 850 C. Calculating an Equilibrium Constant from Equilibrium Concentrations. We will learn more about this later in our combustion studies. 90 moles of H2 and. ) NaHCO3 (s)--> NaOH (s) + CO2 (g) I have already found out that Keq=Pco2,but i need help finding the values. 0 x 10^11/bar for the given reaction at equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g) What is Kc at this temperature? asked Feb 11 in Chemistry by Nishu03 ( 64. Look at everything else it balances. 17th Oct, 2019. 00-L reaction vessel. At equilibrium, the pressure of CO = 2. 2 2 2 CO H CO H O n n n n K = The equilibrium constant K is actually a function of temperature. We show, using published molecular simulation data, how this procedure gives the thermodynamic equilibrium constant and enthalpies of adsorption for CO 2 (g) on graphite. CO2 (g) 3H2(g) CH:ОН (g) + HәО(g). 40 mol of H 2 O were placed in a 1. The equilibrium constant for the formation of CO2 by the reaction 2CO (g) + O2 (g) ↔ 2 CO2 (g) is 1. 00 L container and allowed to come to equilibrium. The reaction CO (g) + H 2O(g) ↔ CO 2(g) + H 2(g) is used to increase the ratio of hydrogen in synthesis gas (mixtures of CO and H 2). Consider the reaction 2 CO2 ⇔ 2 CO + O2 obtained after heating 1 kmol CO2 to 3000 K. At 100°C the equilibrium constant for the reaction COCl 2 (g) CO(g) + Cl 2 (g) has the value of K c = 2. Carbon monoxide reaches equilibrium with water vapour as they react to form hydrogen gas and carbon dioxide gas. CO (g) + H2O (g) ⇄ CO2 (g) + H2 (g) Calculate the value of the equilibrium constant. At this temperature, Kc equals 1. An acid dissociation constant, K a, is the equilibrium constant for the dissociation of an acid in aqueous solution. 5, calculate Kc for Reaction 2 CO2(g)␣CO(g) + 1/2O2(g) how do i calculate kc?. C(s) + H2O(g) <-> H2(g) + CO(g) 4. If at equilibrium [H2] = 0. Identify the equilibrium expression for the following reaction: boy + girl couple 20. ) 2 S (s) + 3 O2 (g)CO2 (g) Kb K =_________ 2. T= Absolute temperature, value of. Analysis Assuming N2 to remain as an inert gas, the stoichiometric and actual reactions can be written asStoichiometric: CO + 1 O 2 ⇔ CO 2 (thus ν. However the Engine Parameters Performance Applets showed that the reaction temperature does in fact go beyond 1000 K. (i) Deduce the equilibrium constant expression, K c, for this reaction. 2NO (g) (N2 (g) + O2 (g) + heat. Consider the following reaction and its equilibrium constant: SO2( g ) + NO2( g ) ⇌ SO3( g ) + NO( g ) Kc = 0. If you're behind a web filter, please make sure that the domains *. 00 atm, and that of the O2 is 1. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. The 3 equations are now: 1. So the O2s are now balanced as well. 0 mol of steam were placed in a flask and heated with a catalyst until equilibrium was established. 100 mol of H2O in a 1. 0611 at 2000 K A reaction mixture initially contains a CO partial pressure of 1326torr and a H2O partial pressure of 1772torr at 2000 K. org are unblocked. a) increase the partial pressure of CO2 (g) at equilibrium. : 3 14) For the reaction PCl 3 (g) + Cl 2 (g) PCl 5 (g) K c = 96. 8 torr) ÷ (760 torr / atm) = 0. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. Determine the normal boiling point (in kelvin) of dichloroethane, CH 2 Cl 2. (b) Oxygen gas oxidizes gaseous ammonia to gaseous nitrogen monoxide; water vapor is the other product. 2NO(g)+O2(g)⇌2NO2(g), K3 = 6. The percent of carbon dioxide gas present in retort smelting as taken from several sources is Iwhile that present in electric furnace smelting is very likely to he more than I %, Study of the Equilibrium of the Reaction. 00-Liter container and allowed to come to equilibrium, determine the equilibrium concentrations of the four chemicals. The equilibrium constant (Kc) for the following reaction is 6. I am going to consider that 0. At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. We know that at equilibrium, the value of the reaction quotient of any reaction is equal to its equilibrium constant. Ionic charges are not yet supported and will be ignored. C(graphite) + O2-->CO2 3. The fourth O2 equilibrium binding constant, K4, measured by kinetic techniques, could be used to ana- lyze equilibrium curves for either native or cross- linked hemoglobin. Write the chemical equation for the equilibrium. The equilibrium constant for this reaction is very large, about 200 times greater than that for the oxygen reaction, so that there is very little haemoglobin left to react with oxygen. 47) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Where, ΔG ° is the standard free change of a reaction, value of ΔG ° is -35000 (calculated in part(a)) R = gas constant, value of R is 8. 39 M SO2, 0. But the forward and reverse reactions are in balance at equilibrium, so there is no net change in the concentrations of the reactants or products, and the reaction appears to stop on the macroscopic scale. The initial moles of CO, H2O, CO2 and H 2 are 2, 5, 0 and 2 moles respectively. Carbon monoxide reaches equilibrium with water vapour as they react to form hydrogen gas and carbon dioxide gas. CO2, H2O, O2, and N2 For rich mixtures CO also exists in the products and at high temperatures the molecules dissociate to form H, O, OH, NO via the following reactions: The opposite direction reactions are also possible At equilibrium the rate of the forward reaction equals the rate of the backward reaction. After an indefinite period of time 14C would still be found only in the CO molecules and not in CO2. 0 liter container. Find the equilibrium constant from the shift in Gibbs function and verify its value with the entry in Table A. At a particular temperature, K = 2. ZnO(s) + CO(g) ⇌ Zn(s) +CO2(g) Find the value of the equilibrium constant: H2 (g) + CO2 (g) ↔ CO(g) + H2O (g) The equilibrium concentrations are found to be [H2] = 0. Change -x -x +x +x. Therefore: H2O(g) increases (formed in the reverse) CO increases (formed in the reverse) Reaction absorbs energy. 45 mol of carbon monoxide and 2. Schematic: 0:24 System Equation: 1:03 Equilibrium Equation: 2:14 Tables: 5:11 Compute the equilibrium composition of CO2 CO and O2 at 3000 K and 3 atm, given that 2 kmol of C and 6 kmol of 02 are. 0010 M CO2 and 0. Carbon (graphite), carbon dioxide, and carbon monoxide form an equilibrium mixture, as represented by the equation. The total pressure of gases at equilibrium when 1. the carbon dioxide gas dissolved in it fizzes out rapidly. 1 × 10-2 M, the concentration of O2 was measured to be 1. If you mean CO2(g) + H2O(l) <==> H2CO3(aq). In chemical reactions involving solids, however, the concentration of the solid—because it is considered to be invariant—does not appear in the equilibrium constant. The top arrow points to the right. The mixture of gases that results is an important industrial fuel called water gas (a) At 800 ºC, the equilibrium constant for this reaction is Kc = 0. What are the concentrations of all the substances when the reaction reaches the equilibrium? | EduRev Class 11 Question is disucussed on EduRev Study Group by 251 Class 11 Students. So now cancel the H2Os as they are on opposite sides and. PHYSICAL CHEMISTRY By: Shailendra Kumar 1. 352 moles of CO and 0. Answer to: For the reaction 2CO(g)+O2(g)<-->2CO2(g), the value of K at a certain temperature is 1300. which is the equilibrium constant. CO+O2=O+CO2. But, we're not finished there. Principles of Chemistry II © Vanden Bout Let’s look at a new condition A AB AB A B B AB A A! A. Definition of equilibrium constant Kp for gas phase reactions, and how to calculate Kp from Kc. We can compare the equilibrium. Keq = 798 for the reaction 2 SO2 (g) + O2 (g)  2 SO3 (g) In a particular mixture at equilibrium, [SO2] = 4. Equilibrium Constant • If the reaction involves a pure solid or pure liquid, these species do not appear in the equilibrium constant expression: Example: CH 4(g) + H 2O(l) CO(g) + 3 H 2(g) KC = [CO(g)] [H2(g)] 3 [CH4 (g)] Note that H 2O(l) does not appear in the denominator. Write the equilibrium constant expression and calculate the value of the equilibrium constant for each of the following reactions at 298 K - Hint: calculate the values of standard Gibb's Free Energy changes first, then use the formula to find the corresponding equilibrium constants. K p = 2 2 CO CO ()P P. 37 (a) Write the expression for the equilibrium constant, K p, for the reaction. 57 mol H2O, 0. ★★★ Correct answer to the question: Please help thank you and the last question says4. This statement is known as Henry's law and the equilibrium constant is quite often referred to as the Henry's law constant. The coefficients a , b , c , and d in the chemical equation become exponents in the expression for K eq. The equilibrium constant {eq}\left( {{K_{\rm{p}}}} \right) {/eq} is a value determined by taking the ratio of partial pressures of all the gaseous products to the partial. First the CO2 dissolves according to: CO2 (g) ( CO2 (l) At room temperature, the solubility of carbon dioxide is about 90 cm3 of CO2 per 100 ml water (cl/cg = 0. At 2000°C, the Keq for the decomposition of carbon dioxide gas to carbon monoxide and oxygen gases is 6. Once you know how many of each type of. 18) Write equilibrium constants for. (a) Cl2(g)+Br2(g) 2BrCl(g)T=25°CKp=4. 00 atm, and that of the O2 is 1. So basically you can say those are a constant, so that would mean that then the solids and the liquids are not included in the equilibrium expression. Chemical equilibrium. At equilibrium, the gases have the following concentrations: [CO 2(g)] = 1. Find ΔHorxn For The Reaction. Use uppercase for the first character in the element and lowercase for the second character. Carbon dioxide (CO2) at 1978C, 2 bar enters a chamber at steady state with a molar flow rate of 2 kmol/s and mixes with nitrogen (N2) entering at 278C, 2 bar with a molar flow rate of 1 kmol/s. 2, the reaction is not at. 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. For a reaction made up of two or more steps, the equilibrium constant for the net. !!equilibrium. 88) An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. Calculate the equilibrium partial pressure of CO2. of reactants equilibrium constant CONSTANT (at a given T) Properties of an Equilibrium Equilibrium systems are • DYNAMIC (in constant motion) • REVERSIBLE • can be approached from either direction Pink to blue Co(H 2O) 6Cl ---> Co(H O) 4Cl. Now the pressure is doubled. () 3 9 2 3 6 T 0. NH3(g) <-> 3/2 H2(g) + 1/2 N2(g) 5. 2CO2 (g) 2CO (g) + O2 (g) DHe = -514 kJ. 0 mol H2S, 4. (d) The equilibrium constant for the reverse reaction, K′, is the reciprocal of K. 2480479034e+069 This process is favorable at. However, the oceans are no longer able to absorb the increased concentration of CO 2 in the atmosphere without changes to the acidity levels. For a chemical equilibrium, the equilibrium constant is defined as the ratio between the product of the equilibrium concentrations of the products and the product of the equilibrium concentrations of the reactants, all raised to the power of their respective stoichiometric coefficients. We also use published experimental data to find similar thermodynamic properties of CO 2 (g) and of CH 4 (g) adsorbed on activated carbon. N2O5 2NO2 + O2 II. depend on dissolved oxygen for respiration. Chemical equilibrium. Chemical Equilibrium -. Change -x -x +x +x. We know that at equilibrium, the value of the reaction quotient of any reaction is equal to its equilibrium constant. 56 - 2 R ln ) T (cal) Since, R T ln is the ordinate of the Ellingham diagram, constant CO/CO2 ratios fall on straight lines on Ellingham diagram. 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). The equilibrium constant for the reaction: N2(g) + 3H2(g) ⇄ 2NH3(g), is Kc = 3. Use uppercase for the first character in the element and lowercase for the second character. 00-L reaction vessel. When you put these numbers into the equation, K is found to be: K = 0. 0 liter container. For any reaction. h 2 o ( l ). At constant temperature, for Le Chatêlier purposes, Adding $\ce{CO}$ produces that it react with $\ce{O2}$ to produce more $\ce{CO2}$ to counteract the effect of the applied change and a new equilibrium is established. If a reaction can be expressed as sum of two or more reactions, the equilibrium constant for the overall reaction is given by the product of the equilibrium constants of the individual reactions K c = K’ c K” c Example The equilibrium constants for carbonic acid (H 2 CO 3) dissociation at 25 C H 2 CO 3 (aq) D H+(aq) + HCO 3-(aq) K c. 2CO(g) + O2(g) <----> 2CO2(g) K = (1 / 2. 39 M SO2, 0. NH3(g) <-> 3/2 H2(g) + 1/2 N2(g) 5. 3H2(g) + N2(g) ( 2NH3(g) 2H2O(g) ( 2H2(g) + O2(g) The units for Keq. As the reaction proceeds toward equilibrium, the reaction shifts left (the amount of products drops while the amount of reactants increases): Q < 1, and δG298 becomes less positive as it approaches zero. 1 Movement of carbon dioxide through tissues and blood cells involves several equilibrium reactions. 1 Equilibrium Chem 36 Spring 2002 2 The Equilibrium Condition ØRecall: a system is at equilibrium when ∆G = 0 • No net driving force for process in either direction ØEquilibrium is a dynamic condition. The following equilibrium is established at 500K: CO2(g) + H2(g) CO(g) + H2O (g) a) calculate the initial partial pressures of CO2, H2 and H2O. 5 × 10 −3 M. The bottom arrow points to the left. If, at equilibrium, the concentration of CO2 is 3. aA + bB ( cC + dD. 00-L reaction vessel. org are unblocked. Which of the following will change the value of the equilibrium constant: A. 55% CO by massC (s) + CO2 (g) ⇌ 2CO (g)Calculate Kc for this reaction at the above temperature. 00 L flask, equilibrium is established. What is the equilibrium constant for the following reaction, NH3(g) ⇄ ½ N2(g) + 3/2 H2(g) 2. 2CH 4(g) C 2H 2(g) + 3H 2(g) While studying this reaction mixture, a chemist analysed a 4. 00 L reaction vessel were present at equilibrium. 16-29E A mixture of CO, O2, and N2 is heated to a high temperature at a constant pressure. Principles of Chemistry II © Vanden Bout Let's look at a new condition A AB AB A B B AB A A! A. So let's go ahead and kind of look at that really quickly. 40 mol of H2O were placed in a 1. We will learn more about this later in our combustion studies. 452 × 10-1 M? 2 CO(g) + O2(g) ⇌ 2 CO2(g). 4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g). At 100°C the equilibrium constant for the reaction COCl 2 (g) CO(g) + Cl 2 (g) has the value of K eq = 2. 56 T (cal)) R T ln = -135194 + (41. The equilibrium equation for the formation of ammonia is: N 2(g) + 3H 2(g) 2NH 3(g) In an equilibrium mixture at 200 °C, the concentrations were found to be as follows: [N 2] = 2. But the forward and reverse reactions are in balance at equilibrium, so there is no net change in the concentrations of the reactants or products, and the reaction appears to stop on the macroscopic scale. Schematic: 0:24 System Equation: 1:03 Equilibrium Equation: 2:14 Tables: 5:11 Compute the equilibrium composition of CO2 CO and O2 at 3000 K and 3 atm, given that 2 kmol of C and 6 kmol of 02 are. Determine the equilibrium constant KP at this temperature. Reaction : Its value. N2O5 2NO2 + O2 II. Are the following mixtures of COCl 2, CO, and Cl 2 at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. 28x10^23)^2 x (1. NaHCO3(s)⇌NaOH(s)+CO2(g) 2HBr(g)+Cl2(g)⇌2HCl(g)+Br2(g) 2SO2(g)+O2(g)⇌2SO3(g). If we raise the temperature we add more heat to this equilibrium reaction. 72 atm CO2, and 0. Consider the reaction: C(s) + O2(g)---> CO2(g) Write the equilibrium constant for this reaction in terms of the equilibrium constants, Ka and Kb, for reactions a and b below: a. Hence: $\left[CO\right]=\frac{0. The expression for the equilibrium constant is Kc = [CO2][H2] / [CO][H2O] Substitute values in the above expression. 303 RT log K c. 1 kJ and ΔSo = -214. Please explain the steps to get the answer! Thanks!!. Section 5- Carbonate Chemistry CASE 1 CO 2 - H 2 O open system Aqueous carbon dioxide reacts to form carbonic acid via the following reaction: 2 0. Carbon dioxide (CO2) at 1978C, 2 bar enters a chamber at steady state with a molar flow rate of 2 kmol/s and mixes with nitrogen (N2) entering at 278C, 2 bar with a molar flow rate of 1 kmol/s. 025 atm of carbon monoxide and 0. 1Chemical Equilibria 13. rate is kept low enough that equilibrium will be attained, and analysis of the effluent gas gives the data necessary for calculation of the equilibrium constant. (b) Oxygen gas oxidizes gaseous ammonia to gaseous nitrogen monoxide; water vapor is the other product. 0015 M Solved If the value for the equilibrium constant is much greater than 1, then the equilibrium mixture conta. T= Absolute temperature, value of. 1 kJ and ΔSo = -214. Justify your prediction. 937 * 10³ As K > 1 the equilibrium favours the products. 00-2x 2x x Therefore the [O2] = 5. Calculate the equilibrium [O2] in this mixture. 7 x 10-2 M [NH3] = 1. Sample Exercise 15. At 855 K, The Equilibrium Constant Is 0. What is the equilibrium concentration of the lightest gas? 0. 0010 M CO2 and 0. varying the initial concentration of a reactant C. 00-L vessel?. On analysis, an equilibrium mixture for the reaction 2H2S(g) ↔ 2H2(g) + S2(g) was found to contain 1. C (s graphite) + 1 O2 (g) → CO2 (g) Back to reactions list. 352 moles of CO and 0. 40 10-33 18. For the reaction given below at 700°C, Kc = 0. Compared to the original system, the rates of the forward and reverse reactions of the new equilibrium. So let's go ahead and kind of look at that really quickly. 1908 moles of CO 2, 0. CO2(g) + C(graphite) ⇌ 2 CO(g)-The equilibrium constant will increase. An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0. There is always some CO present in the TOX flue gas because CO 2 and CO exist in a "chemical equilibrium", which can be described by the equation: CO + ½ O 2 <--> CO 2. Previously, the products of combustion were determined assuming that the reaction temperature did not reach greater than 1000 K.
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