Consider this reaction in a closed container. 2NO(g) + O2(g) 2NO2(g) An equilibrium mixture is prepared at 298 K with these values: [NO] = 0.0542 M, [0,] = 0.127 M, and [NO,] = 15.5 M. Suddenly, the NO, partial pressure is increased by a factor of 6.61 In which direction do you predict the reaction will go to return to equilibrium? Calculate AG for this non-equilibrium mixture before any further reaction occurs.

Consider this reaction in a closed container. 2NO(g) + O2(g) 2NO2(g) An equilibrium mixture is prepared at 298 K with these values: [NO] = 0.0542 M, [0,] = 0.127 M, and [NO,] = 15.5 M. Suddenly, the NO, partial pressure is increased by a factor of 6.61 In which direction do you predict the reaction will go to return to equilibrium? Calculate AG for this non-equilibrium mixture before any further reaction occurs.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.220 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At equilibrium, [NOCl] = 1.60 M and [NO] = 0.80 M. The [Cl2] is
At a given temperature, an equilibrium mixture associated with the reaction A(g) + 2 B(g) = 2 C(g) contains: [A] = 0.0250 M [B] = 0.150 M [C] = 0.550 M What is the value of K, for this reaction at the same temperature?
The equilibrium constant, Kp, for the following reaction is 5.40 at 346 K:COBr2(g) CO(g) + Br2(g)Calculate the equilibrium partial pressures of all species when COBr2(g) is introduced into an evacuated flask at a pressure of 0.767 atm at 346 K. PCOBr2 = atm PCO = atm PBr2 = atm
The reaction H2(g) + I2(g) 2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.01 atm and H2 at a pressure of 2.62 atm. Calculate the equilibrium pressure of I2(g) in this mixture.
At 500K, the methanol decomposes according to the following reaction, CH3OH(g) = CO(g) + 2 H2(g) K= 9.60×10-2 Some methanol, CH3OH (molar mass: 32 g/mol), is placed into a rigid 2.00-L vessel, and the temperature is raised to 500K. If the concentration of H2 in the equilibrium mixture is 0.246M, what is the initial concentration of methanol? O A, 0.231 M Ов. 0.866 М OC 0.200 M OD. 1.109 M O E. 0.012 M
The equilibrium constant Kp for the reaction PC15(g) = PC13(g) + Cl₂(g) is 1.05 at 250°C. The reaction starts with a mixture of PC15, PC13, and Cl₂ at pressures 0.177 atm, 0.233 atm, and 0.161 atm, respectively, at 250°C. When the mixture comes to equilibrium at that temperature, which pressure(s) will have decreased? Cl₂ PC13 PC15
The equilibrium constant, K., for the following reaction is 77.5 at 600 K. CO(g) + Cl(g) COCI,(g) Calculate the equilibrium concentrations of reactant and products when 0.451 moles of CO and 0.451 moles of Cl, are introduced into a 1.00 L vessel at 600 K. [CO] [Cl] [COCL,] = MMM
12) For the reaction: Br,(g) + Cl₂(g) = 2 BrCl(g), Kc = 7.20 at 200°C. If a reaction vessel is filled with these gases, such that [Br₂] = 5.0 M, [CL] = 5.0 M and [BrC1] = 5.0 M a) We do not know if this system has reached at equilibrium or not. Please find out whether this reaction is at equilibrium or not? You should show your work to determine this. b) If it is not at equilibrium, which direction the reaction will proceed? S yred site to induty inatambolt (o 9815011 (6
Consider the following equilibrium process at 686 degrees celsius. CO2 (g) + H2 (g) ---> CO (g) + H2O (g) The equilibrium concentrations of the reaction species are [CO]= 0.0510 M, [H2]= 0.0410 M, [CO2]= 0.0840 M, and [H2O]= 0.0390 M. a) alculate Kc for the reaction at 686 degrees celcius. Round your answer to 3 significant figures. b) If we add CO2 to increase its concentration to 0.420 M, what will the concentration of all the gases be when equilibrium is reestablished? [CO2]= M. Round your answer to 3 significant figures. c) [H2] = M. Round your answer to 2 significant figures. d) [CO]= M. Round your answer to 2 significant figures. e) [H2O]= M. Round your answer to 2 significatnt figures
CS 2( g) + 3Cl 2( g) <=> CCl 4( g) + S 2Cl 2( g) At a given temperature, the reaction above is at equilibrium when [CS2] = 0.075 M, [Cl2] = 0.35 M, [CCl4] = 0.25 M, and [S2Cl2] = 0.45 M. What will be the direction of the reaction when the reactants and products have the following concentrations: CS2 = 0.15 M, Cl2 = 0.15 M, CCl4 = 0.45M, and S2Cl2 = 0.31 M? I would like help with this problem I am solving for Kc and then Qc I believe. for Kc I set up the following equation using the molarity values in the brackets as (.25)(.45)/(.075)(.035)^3 and the Qc as (.45)(.31)/(.15)(.15)^3