When are more products of a reaction available initially than at equilibrium?

A. K = 0
B. Q < K
C. Q = K
D. Q > K

To determine when more products of a reaction are available initially than at equilibrium, we need to compare the reaction quotient, Q, with the equilibrium constant, K.

Here's a breakdown of the possible answer choices:

A. K = 0: This answer choice is incorrect. If the equilibrium constant, K, is equal to zero, it means that there are no products formed at equilibrium. It does not indicate whether more products are available initially.

B. Q < K: This answer choice is correct. When the reaction quotient, Q, is less than the equilibrium constant, K, it signifies that the reaction has not yet reached equilibrium and there are more products available initially. This suggests that the reaction will proceed in the forward direction to reach equilibrium.

C. Q = K: This answer choice is incorrect. If the reaction quotient, Q, is equal to the equilibrium constant, K, it means that the reaction is already at equilibrium. It doesn't indicate whether there are more products available initially.

D. Q > K: This answer choice is incorrect. When the reaction quotient, Q, is greater than the equilibrium constant, K, it suggests that the reaction has gone past equilibrium and has more products consumed than initially available. It does not indicate that there are more products available initially.

In conclusion, the correct answer is B. Q < K.