Question

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

In general, at a given temperature, the reaction quotient (Q) is a 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 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 CO₂.

At equilibrium, individual molecules cannot undergo any chemical reactions.

At equilibrium, the overall composition of the reaction mixture is changing rapidly.

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

Answer 1

Statement I	True	The reaction quotient (denoted by Q) is a measure of the relative amounts of products and reactants present in a reaction at a given time. In general at at a given temperature the reaction quotient is a constant.
Statement II	False	The amounts of CO in the two vessels ( at equilibrium) will only be the same if the equation states that the amount of reactants and products are same, which would be K =1. Unless K is 1, this statement is false.
Statement III	True	This statement is true because the forward and reverse reactions continue to occur at the equilibrium.
Statement IV	False	Equilibrium never means "no reaction". The forward and reverse reactions continue to occur at the equilibrium.
Statement V	False	At equilibrium the composition of mixture does not change.
Statement VI	True	Value of Kc (Equilibrium Constant) is used to predict the direction of the given reaction.