Consider the reaction: H2O(g) + CO(g) = H2(g) + CO2(g) Which of the following st
ID: 476297 • Letter: C
Question
Consider the reaction: H2O(g) + CO(g) = H2(g) + CO2(g) Which of the following statements are true and which are false.
At equilibrium, the overall composition of the reaction mixture is constant.
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 would still be found only in the CO molecules and not in CO2.
In general, at a given temperature, the reaction quotient (Q) is a constant.
The equilibrium constant depends on the initial concentrations.
At equilibrium, individual molecules may be subject to rapid chemical transformations.
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 CO(g) in the two vessels are equivalent.
Explanation / Answer
At equilibrium, the overall composition of the reaction mixture is constant. - true
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 would still be found only in the CO molecules and not in CO2. - false
In general, at a given temperature, the reaction quotient (Q) is a constant. true
The equilibrium constant depends on the initial concentrations. - false
The equilibrium constant depends on the initial concentrations. - false
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 CO(g) in the two vessels are equivalent. - false