Question

For the reaction
$2N_2{O}_5\left(g\right)\to 4N{O}_2\left(g\right)+O_2\left(g\right)$
$-\frac{\Delta \left[N_2{O}_5\right]}{\Delta t}=k_1\left[N_2{O}_5\right],+\frac{\left[N{O}_2\right]}{\Delta t}=k_2\left[N_2{O}_5\right],+\frac{\Delta \left[O_2\right]}{\Delta t}=k_3\left[N_2{O}_5\right]$ Thus,

• A. $2k_1=4k_2=k_3$
• B. $2k_1=k_2=4k_3$
• C. $k_1=k_2=k_3$
• D. None of these

Answer 1

The correct option is B $2k_1=k_2=4k_3$

For the reaction
$2N_2{O}_5\left(g\right)\to 4N{O}_2\left(g\right)+O_2\left(g\right)$
Rate of the reaction:
$-\frac{1}{2}\frac{d\left[N_2{O}_5\right]}{dt}=\frac{k_1}{2}{N}_2{O}_5\left]\right(i)$
$\frac{1}{4}\frac{d\left[N{O}_2\right]}{dt}=\frac{k_2}{4}\left[N_2{O}_5\right]\left(ii\right)$
$\frac{d\left[O_2\right]}{dt}=k_3\left[N_2{O}_5\right]\left(iii\right)$
all are rate of reaction thus
$i=ii=iii$
$2k_1=k_2=4k_3$