Question

For the gaseous reaction $2A+B\to C+D$, the rate is given by $k\left[A\right]\left[B\right]$. The volume of the container containing the reaction mixture is suddenly reduced to one-fourth of its original volume. with respect to the original rate, now the rate would be:

• A. $\frac{1}{16}$ times the original rate
• B. $\frac{1}{8}$ times the original rate
• C. $16$ times the original rate
• D. $8$ times the original rate

Answer 1

Answer: (A)

$\frac{1}{16}$ times the original rate

$rate=k\left[A\right]\left[B\right]$

The volume of the container containing the reaction mixture is reduced to one-fourth of its original volume w.r.t. original rate.

So, the rate would become $\left[\frac{1}{4}\right]\times \left[\frac{1}{4}\right]$ = $\frac{1}{16}$ times the original rate

Hence, the correct option is $A$