For the following reaction :
\(2 \mathrm{~A}_2(\mathrm{~g})+\frac{1}{4} \mathrm{X}(\mathrm{~g}) \rightarrow 2 \mathrm{~A}_2 \mathrm{X}(\mathrm{~g})\)
volume is increased to double its value by decreasing the pressure on it. If the reaction is first order with respect to X and second order with respect to A2, the rate of reaction will:
1
Decrease by eight times of its initial value
2
Increase by eight times of its initial value
3
Increase by four times of its initial value
4
Remain unchanged