The equilibrium constant for the following reaction is 1.29×10-2 at 600K. COCl2(g) <---> CO(g) + Cl2(g) If an equilibrium mixture of the three gases at 600K contains 2.28×10-2 M COCl2(g) and 1.87×10-2 M CO, what is the equilibrium concentration of Cl2? M
The equilibrium constant for the following reaction is 1.29×10-2 at 600K. COCl2(g) <---> CO(g) + Cl2(g) If an equilibrium mixture of the three gases at 600K contains 2.28×10-2 M COCl2(g) and 1.87×10-2 M CO, what is the equilibrium concentration of Cl2? M
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 40GQ: Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample...
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The equilibrium constant for the following reaction is 1.29×10-2 at 600K.
COCl2(g) <---> CO(g) + Cl2(g)
If an equilibrium mixture of the three gases at 600K contains 2.28×10-2 M COCl2(g) and 1.87×10-2 M CO, what is the equilibrium concentration of Cl2? M
Consider the following equilibrium system at 786 K.
2NH3(g) <---> N2(g) + 3H2(g)
If an equilibrium mixture of the three gases at 786 K contains 7.71*10^M NH3 , 2.68*10^-2 M , and 1.73*10^-2M H2, what is the value of the equilibrium constant K?
K =
Consider the following system at equilibrium at 800 K:
2H2(g) + S2(g) 2H2S(g) + 69.3 kcal
2H2(g) + S2(g) 2H2S(g) + 69.3 kcal
Indicate whether each individual change would favor the production of H2S(g). Evaluate each change separately, assuming that all other conditions remain constant.
Increasing the temperature. | |
Decreasing the pressure. | |
Increasing the volume. | |
Adding H2S. | |
Removing S2. |
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