Consider the reaction: H2O(g) + CO(g) = H2(g) + CO2(g) Which of the following st
ID: 690911 • 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.
1) The equilibrium position depends on the initialconcentrations.
2) Amounts of all reactants and products corresponding to an exactequilibrium composition for this reaction are sealed in a vessel.The CO placed in the vessel is labelled with 14C. After anindefinite period of time 14C may be found in both CO and CO2molecules.
3) At equilibrium, the overall composition of the reaction mixtureis constant.
4) In general, at a given temperature, the reaction quotient (Q) isa constant.
5) 1 mol of H2O(g) and 1 mol of CO(g) are placed in a vessel and 1mol of H2(g) and 1 mol of CO2(g) are placed in another of equalvolume. At equilibrium, at 350°C, the amounts of H2O(g) in thetwo vessels are equivalent.
6) At equilibrium, individual molecules may be subject to rapidchemical transformations.
I've tried: T T T F F F T T T T T T F T T F F F F T T F F T F T T T F T F T T T T T F T T F T T All of them are wrong. I have no idea as to which ones areright/wrong.
I've tried: T T T F F F T T T T T T F T T F F F F T T F F T F T T T F T F T T T T T F T T F T T All of them are wrong. I have no idea as to which ones areright/wrong.
Explanation / Answer
1) F 2) T 3) ? 4) F 5) T 6) T
However 3) I'm only guessing:
3) I know that saying the equilibrium composition is changingslowly is incorrect so therefore constant seems right. Assumingnothing is being added or removed the forward and reverse reactionsshould be the same.