Question

If the decomposition of nitrogen oxides as ${2N}_2{O}_5\to {4NO}_2+O_2$.
Calculate the rate constant for a $0.05M$ solution if the instantaneous rate is $1.5\times {10}^{-6}mol/l/s.$

• A. $3\times {10}^{-5}$
• B. $3\times {10}^{-4}$
• C. $3\times {10}^{-2}$
• D. $2\times {10}^{-4}$

Answer 1

The correct option is A $3\times {10}^{-5}$

Solution:- (A) $3\times {10}^{-5}$

Given that:-

$\left[N_2{O}_5\right]=0.05M$

$Rate=1.5\times {10}^{-6}mol/l/s$

For the reaction, $2N_2{O}_5⟶4N{O}_2+O_2$,

Rate constant, $\left(K\right)=\frac{Rate}{\left[N_2{O}_5\right]}=\frac{1.5\times {10}^{-6}}{0.05}=3\times {10}^{-5}{s}^{-1}$