Question

The rate equation of a gaseous reaction is given by, $r=K\left[A\right]\left[B\right]$.

If the volume of the reaction vessel is suddenly reduced to $\frac{1}{2}$ of the initial volume, the reaction rate relating to the original rate will be:

• A. $\frac{1}{4}$
• B. $4$
• C. $\frac{1}{2}$
• D. $2$

Answer 1

Answer: (B)

$4$

$r=K\left[A\right]\left[B\right]$

when the volume of the vessel is reduced to one half of the initial volume,

$r^{\prime \prime }=k\left[2A\right]\left[2B\right]$

$r^{\prime \prime }=4r$

The reaction rate becomes 4 times the original rate.

Hence, option B is correct.