Question

Consider the reaction:
2N2O (g) 2N2 (g) + O2 (g)

The values of Kc at different temperatures are:
Temperature: 838, Kc= 1.10 x 10^-3
Temperature: 1001, Kc= 3.80 x 10^-1
Temperature: 1030, Kc= 8.71 x 10^-1
Temperature: 1053, Kc= 1.67

Which statement is correct at a higher temperature?
A. The forward reaction is favoured.
B. The reverse reaction is favoured.
C. The rate of the reverse reaction is greater than the rate of the forward reaction.
D. The concentration of both reactants and products increase.

Answer 1

Note that as T increases the Kc value increases which means the products are increasing at the expense of the reactants; therefore, A is the only statement that is true.