H2O(g) + CO(g) = H2(g) + CO2(g)

Question

Which of the following statements are true and which are false.

a) 1 mol of H2O(g) and 1 mol of CO(g) are placed in a vessel and 1 mol of H2(g) and 1 mol of CO2(g) are placed in another of equal volume. At equilibrium, at 350°C, the amounts of H2O(g) in the two vessels are not equivalent.

b) At equilibrium, the overall composition of the reaction mixture is not changing.

c) Q = K when the system is at equilibrium.

d) At equilibrium, individual molecules may be subject to rapid chemical transformations.

e) Amounts of all reactants and products corresponding to an exact equilibrium composition for this reaction are sealed in a vessel. The CO placed in the vessel is labelled with 14C. After an indefinite period of time 14C may be found in both CO and CO2 molecules.

f) The equilibrium constant does not reveal the rate of that reaction.

Answer 1

f is true.
e is true.
I am unsure how to interpret part d but by my interpretation it is true. Equilibrium is not a static set because even at equilibrium the equation is a dynamic one and the concentrations are changing rapidly. Also see part b and understand that although the system is still dynamic at equilibrium the K for the reaction does not change rapidly and the overall concentrations do not change.
c is true.
a is false. They will be the same.