In the reaction, $2{N_2}{O_5} \to 4N{O_2} + {O_2}$ initial pressure is $500\;atm$ and rate constant $k$ is $3.38 \times {10^{ - 5}}\;{s^{ - 1}}$ after 10 min the final pressure of ${N_2}{O_5}$ is

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

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Application +4 | -1

In the reaction,

2{N_2}{O_5} \to 4N{O_2} + {O_2}

initial pressure is

500\;atm

and rate constant

k

3.38 \times {10^{ - 5}}\;{s^{ - 1}}

after 10 min the final pressure of

{N_2}{O_5}

View answer and explanation

Correct option: A

490 atm

Option A (490 atm) is correct because it is calculated using the first-order kinetics equation and the given rate constant to determine the pressure change of N2O5 after 10 minutes.

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