Question

The half-life of decomposition of $N_2{O}_5$ is a first order reaction represented by
$N_2{O}_5\to N_2{O}_4+1/2O_2$
After $15$ minutes the volume of $O_2$ produced is $9mL$ and at the end of the reaction $35mL.$ The rate constant is equal to:

• A. $\frac{1}{15}lo{g}_e\frac{35}{26}$
• B. $\frac{1}{15}lo{g}_e\frac{44}{26}$
• C. $\frac{1}{15}lo{g}_e\frac{35}{36}$
• D. None of the foregoing

Answer 1

Answer: (A)

$K\times 15=ln\left(\frac{35-0}{35-9}\right)$