Which one is not correct, and explain why. Thanks. Consider the reaction: H_2O(g

Question

Which one is not correct, and explain why. Thanks.

Consider the reaction: H_2O(g) + CO(g) H_2(g) + CO_2(g) Which of the following statements are true and which are false. At equilibrium, individual molecules cannot undergo any chemical reactions. In general, at a given temperature, the reaction quotient (Q) is a constant. l mol of H_2O(g) and l mol of CO(g) are placed in a vessel and l mol of H_2(g) and l mol of CO_2(g) are placed In another of equal volume. At equilibrium, at 350 degree C. the amounts of CO_2(g). In the two vessels are not equivalent. 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 CO_2. At equilibrium, the overall composition of the reaction mixture is changing rapidly. The equilibrium constant does not reveal the rate of that reaction.

Explanation / Answer

1. False. Equilibria are dynamic. The forward and reverse reactions are constantly reacting, but at the same rates, so that the relative concentrations are constant.

2. false. there could be an infinite number of values of Q depending upon the number of concentration. Keq is a constant at a given temperature, in fact T is the only variable for which Keq changes, but Q is not a constant.

3. true

4. false, the radioactive carbon is distributed through out. so its found in co2 also

5. False. At equilibrium the concentrations does not change they are constant .even though the reactions are running in both directions.

6.True. All you know is the the rate of the forward reaction is equal to the rate of the reverse reaction. The value of Keq is the ratio of the rate constants, but you know only the ratio not the actual values of the rate constants, and hence the rates.

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