Question

Which of the following statement is incorrect about the reaction?

• A. The degree of decomposition is $N_2{O}_5,\alpha =1-e^{-K_1\cdot t}$
• B. The forward reaction is endothermic
• C. The forward reaction is exothermic
• D. The half-life of reaction is $\frac{ln2}{K_1}$

Answer 1

The correct option is C The forward reaction is exothermic

For 1s, order reaction $K_{1}t=ln\frac{N_0}{N}$
$\frac{N_0}{N}=e^{K_1\cdot t}$ or $\frac{N}{N_0}=e^{-K_1\cdot t}$
$1-\frac{N}{N_0}=1-e^{-K_1\cdot t}$
or $\frac{N_0-N}{N_0}=\alpha =1-e^{-K_1\cdot t}$
Also, for Ist order $K_1\cdot t_{1/2}=ln2$; the decomposition is always endothermic.