Write the equilibrium expression for the following reaction.
CO2(g) + H2(g)↔ CO(g) + H2O(g)
Select one:
a. Keq = [CO2] + [H2]/[ CO]+ [H2O]
b. Keq = [ CO][H2O] / [CO2] [H2]
c. Keq = [ CO] +[H2O] / [CO2] + [H2]
d. Keq = [CO2] [H2]/[ CO][H2O]
Write the equilibrium expression for the following reaction. CO2(g) + H2(g)↔ CO(g) + H2O(g) Select one: a. Keq = [CO2] + [H2]/[ CO]+ [H2O] b. Keq = [ CO][H2O] / [CO2] [H2] c. Keq = [ CO] +[H2O] / [CO2...
The equilibrium constant Kc for the following reaction is 8.30. H2(g) + CO2(g) ↔ H2O(g) + CO(g) Initially, 0.40 moles each of H2 and CO2 are injected into a 9.00 L flask. Calculate the concentration of the CO(g) at equilibrium.
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0580 M, [H2] = 0.0430 M, [CO2] = 0.0830 M, and [H2O] = 0.0370 M. (a) Calculate Kc for the reaction at 686°C. (b) If we add CO2 to increase its concentration to 0.460 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M H2: M CO: M...
Consider the following equilibrium process at 686 ° C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0480 M, [H2] = 0.0400 M, [CO2] = 0.0880 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686 ° C. (b) If we add CO2 to increase its concentration to 0.510 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? CO2: M...
4. Consider the following reaction at equilibrium CO(g) + H2O(g) + CO2(g) + H2(g) 2.50 mole of CO(g) and 2.50 mole of H2O(g) gas at 588 K are mixed in a 10.00 L container. (Kc = 31.4 at 588 K) Calculate the concentration of CO(g), H2O(g), CO (g), and H.(g) at equilibrium. 5. Consider the following reaction: CO(g) + H2O(g) + CO2(g) + H2(g) (a) If a 10.00L container has 2.50 mole of CO(g), 2.50 mole of H2O(g), 5.00 mole...
Practice: In the reaction: CO2(g) + H2(g) + CO(g) + H2O(g) Kc = 0.11 The equilibrium concentrations are [CO2] = 0.25M, [H2] = 0.80M, (H2O) = 0.50M. What is the concentration of CO at equilibrium?
(a) Calculate ∆G for the reaction: C(s, graphite) + H2O (g) ↔ CO (g) + H2 (g) where temperature is 700 K, ∆G⁰ = 92 kJ and the initial pressure of each gas is P H2O = 0.67 atm, P CO = 0.23 atm, P H2 = 0.51 atm. (b) What direction would this reaction proceed?
An industrial chemist puts 1.25 mol each of H2(g) and CO2(g) in a 1.00-L container at a certain temperature. When equilibrium is reached, 0.56 mol of CO(g) is in the container. Find Keq at this temperature for the following reaction: H2(g) + CO2(g)↔H2O(g) + CO(g)
Which of the following is the equilibrium expression (Kc) for the following equilibrium H2O (l) + CO (g) <--> H2 (g) + CO2 (g) Select the correct answer [H2O] [CO] / [H2] [CO2] [H2] [CO2] / [H2O] [CO] [H2] [CO2] / [CO] [H2] [CO2] / [H2O]
The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.71 mol H2 and 0.71 mol CO2 are injected into a 5.0−L flask. Calculate the concentration of each species at equilibrium.
Chemical Equilibrium Characteristics Consider the reaction: H2O(g) + CO(g) H2(g) + CO2(g) Which of the following statements are true and which are false. true false At equilibrium, the overall composition of the reaction mixture is not changing. true false At equilibrium, individual molecules may be subject to rapid chemical transformations. true false The rate at which equilibrium is established can be inferred from the magnitude of the equilibrium constant. true false When Q < K the system will spontaneously shift to the right. true...