Question

For the reaction system:
$2NO\left(g\right)+O_2\left(g\right)\to 2N{O}_2\left(g\right)$, volume is suddenly reduced to half its value by increasing the pressure on it. If the reaction is of first order with respect to $O_2$ and second order with respect to $NO$, the rate of reaction will:

• A. diminish to one-eighth of its initial value
• B. increase to eight times of its initial value
• C. increase to four times of its initial value
• D. diminish to one-fourth of its initial value

Answer 1

The correct option is B increase to eight times of its initial value

Order of reaction with respect to $O_2:first$

Order of reaction with respect to $NO:second$

$Rate=k\left[NO{]}^2\right[O]$

Volume is decreased to half, then concentration of each reactants gets doubled.

$RateNew=k\left[2NO{]}^2\right[2O]$

$\therefore$ Rate of reaction will increase to eight times of it’s initial value.