How will the rate of reaction, `2NO_((g)) +O_(2(g)) + 2NO_(2(g))` get affected if the volume of the reacting system is doubled? (Given that the reaction is second order with respect to NO and first order with respect to `O_2`).

Options

A. Diminishes to one-fourth of its initial value
B. Diminishes to one-eighth of its initial value
C. Increases four times
D. Increases eight times

Answer

B

Explanation

Initially rate law can be written as `r_1=k[NO]^2[O_2]` On doubling the volume, concentration becomes half then , `r_2=k[1/2NO]^2[1/2O_2]=1/4xx1/2k[NO]^2[O_2]-1/8r_1`
Thus, rate diminishes to one-eighth of the its initial volume.