Question

The reaction $N_2{O}_5$ (in $C{Cl}_4$)$\to 2{NO}_2+1/2O_2\left(g\right)$ is first order in $N_2{O}_5$ with rate constant $6.2\times {10}^{-4}$. What is the value of rate of reaction when $\left[N_2{O}_5\right]=1.25mole$ $L^{-1}$

• A. $7.75\times {10}^{4}mol$ $L^{-1}{S}^{-1}$
• B. $6.35\times {10}^{3}mol$ $L^{-1}{S}^{-1}$
• C. $5.15\times {10}^{5}mol$ $L^{-1}{S}^{-1}$
• D. $3.85\times {10}^{4}mol$ $L^{-1}{S}^{-1}$

Answer 1

The correct option is A $7.75\times {10}^{4}mol$ $L^{-1}{S}^{-1}$

Its a 1st Order Reaction

$Rate=k\left[A\right]$

So, Rate of reaction would be

$Rate=6.2\times {10}^{-4}\times 1.25$

$Rate=7.75\times {10}^{4}mol{L}^{-1}{S}^{-1}$