Question

For the reaction $A+B\to$ Products, it is found that the order of the reactions A and B are 1 and 2, respectively. When the concentration of A is halved and that of B is doubled, the rate increases by a factor of:

Answer 1

According to given reaction, $A+B\to Products$
$rate,r=\frac{dx}{dt}=k\left[A\right][B{]}^2$
$r^{\prime }=k\left[\frac{A}{2}\right][2B{]}^2$$=\frac{1}{2}k\left[A\right]4[B{]}^2=2k[A\left]\right[B{]}^2$
$\frac{r^{\prime }}{r}=\frac{2k\left[A\right][B{]}^2}{k\left[A\right][B{]}^2}=2$