For the overall reaction NO2 + CO -> NO + CO2 the proposed mechanism is: step 1, 2NO2 -> NO3 + NO (slow); step 2, NO3 + CO -> NO2 + CO2 (fast). Select the correct statements.

The rate law is rate = k[NO2]^2.

NO3 is a reaction intermediate.

The rate-determining step is bimolecular.

The rate law is rate = k[NO2]^2.

NO3 is a reaction intermediate.

Doubling [CO] doubles the rate.

The rate-determining step is bimolecular.

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3ck030

For the overall reaction $NO X_{2} + CO NO + CO X_{2}$ the proposed mechanism is: step 1, $2 NO X_{2} NO X_{3} + NO$ (slow); step 2, $NO X_{3} + CO NO X_{2} + CO X_{2}$ (fast). Select the correct statements.

The slow step 1 is elementary, so rate

= k [NO X_{2}]^{2}

, and CO appears only after the slow step so doubling

[CO]

does not change the rate.

NO X_{3}

is formed in step 1 and consumed in step 2, so it is an intermediate. Step 1 involves two

NO X_{2}

molecules, so it is bimolecular.