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 repeat to NO, the rate of reaction will:

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

Answer 1

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

The rate law expression is $R=k\left[O_2\right][NO{]}^2$

When volume is suddenly reduced to half its value ,
The rate law expression becomes $R^{\prime }=k\left[2O_2\right][2NO{]}^2=8k[O_2\left]\right[NO{]}^2=8R$