When are more products of a reaction available initially than at equilibrium?
A. K = 0
B. Q < K
C. Q = K
D. Q > K
Q>K
Go away bob
Thanks Drbob
To determine when there are more products of a reaction available initially than at equilibrium, we need to consider the reaction quotient (Q) compared to the equilibrium constant (K).
The reaction quotient (Q) is calculated in the same way as the equilibrium constant (K), but it is calculated using the concentrations or pressures of the reactants and products at any given point during the reaction, rather than at equilibrium.
In this case, we are looking for the condition when there are more products initially compared to equilibrium. This means that the quotient Q must be greater than the equilibrium constant K.
So, the correct answer is:
D. Q > K
When the reaction quotient (Q) is greater than the equilibrium constant (K), it indicates that there are relatively higher concentrations of products compared to the equilibrium state.
Q = (products)/(reactants)
K = (products)/(reactants)
reactants ==> products
You want products to be higher so is it B or D