Consider the reaction: Which of the following statements are true and which are
ID: 483248 • Letter: C
Question
Consider the reaction:
Which of the following statements are true and which are false.
At equilibrium, the overall composition of the reaction mixture is not changing.
At equilibrium, individual molecules may be subject to rapid chemical transformations.
The rate at which equilibrium is established cannot be inferred from the magnitude of the equilibrium constant.
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.
In general, at a given temperature, the reaction quotient (Q) is a 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 may be found in both CO and CO2 molecules.
Explanation / Answer
1. True. AT equilibrium, the reactants and products achieve a state where their concentrations do not change.
2. True. AT equilibrium, rate if forward reaction equalize rate of backward reaction. However, both these reactions takes place simulatneously.
3. False. Equilibrium constant can tell about qualitatively , but not quantitatively.
4. False, as the rate will be same for both reactions. So, they will be equivalent.
5. False, Q keeps on changing with change in concentrations.
6. True, as both forward and backward reactions takes place, both will have 14C.
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