For the reaction, ${{\rm{N}}_2}{{\rm{O}}_5} \to 2{\rm{N}}{{\rm{O}}_2} + \frac{1}{2}{{\rm{O}}_2}$ Given, $ - \frac{{d\left[ {{{\rm{N}}_2}{{\rm{O}}_5}} \right]}}{{dt}} = {K_1}\left[ {{{\rm{N}}_2}{{\rm{O}}_5}} \right]$ $\frac{{d\left[ {{\rm{N}}{{\rm{O}}_2}} \right]}}{{dt}} = {K_2}\left[ {{{\rm{N}}_2}{{\rm{O}}_5}} \right]$ ${\rm{and}}\;\;\frac{{d\left[ {{{\rm{O}}_2}} \right]}}{{dt}} = {K_3}\left[ {{{\rm{N}}_2}{{\rm{O}}_5}} \right]$ The relation in between ${K_1},{K_2}\;and\;{K_3}$ is:

JEE CHEMISTRY MCQ: CHEMICAL KINETICS

1 Easy

1 of 1

Analyzing +4 | -1

For the reaction,

{\mathrm{N}_2}{\mathrm{O}_5} \to 2\mathrm{N}{\mathrm{O}_2} + \frac{1}{2}{\mathrm{O}_2}

Given,

- \frac{{d\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]}}{{dt}} = {K_1}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]

\frac{{d\left[ {\mathrm{N}{\mathrm{O}_2}} \right]}}{{dt}} = {K_2}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]

\mathrm{and}\;\;\frac{{d\left[ {{\mathrm{O}_2}} \right]}}{{dt}} = {K_3}\left[ {{\mathrm{N}_2}{\mathrm{O}_5}} \right]

The relation in between

{K_1},{K_2}\;and\;{K_3}

is:

View answer and explanation

Correct option: A

2{K_1} = {K_2} = 4{K_3}

Option A (

2{K_1} = {K_2} = 4{K_3}

) is correct because it correctly relates the rate constants based on the stoichiometry of the reaction.