At room temperature, the reaction between ${\rm{NO}}$ and ${{\rm{O}}_2}$ to give ${\rm{N}}{{\rm{O}}_2}$ is fast, while that between ${\rm{CO}}$ and ${{\rm{O}}_2}$ is slow. It is due to:

The activation energy for the reaction, $2{\rm{NO}} + {{\rm{O}}_2} \to 2{\rm{N}}{{\rm{O}}_2}$ is less than $2{\rm{CO}} + {{\rm{O}}_2} \to 2{\rm{C}}{{\rm{O}}_2}$

${\rm{CO}}$ is smaller in size than that of ${\rm{NO}}$

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NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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Understanding +4 | -1

At room temperature, the reaction between

\mathrm{NO}

and

{\mathrm{O}_2}

to give

\mathrm{N}{\mathrm{O}_2}

is fast, while that between

\mathrm{CO}

and

{\mathrm{O}_2}

is slow. It is due to:

View answer and explanation

Correct option: C

The activation energy for the reaction,

2\mathrm{NO} + {\mathrm{O}_2} \to 2\mathrm{N}{\mathrm{O}_2}

is less than

2\mathrm{CO} + {\mathrm{O}_2} \to 2\mathrm{C}{\mathrm{O}_2}

Option C (The activation energy for the reaction,

2\mathrm{NO} + {\mathrm{O}_2} \to 2\mathrm{N}{\mathrm{O}_2}

is less than

2\mathrm{CO} + {\mathrm{O}_2} \to 2\mathrm{C}{\mathrm{O}_2}

) is correct because reactions with lower activation energies proceed faster.

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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