The experimental data for the reaction $2A+B_2\to 2AB$ is given below. Based on the data, write the rate equation

$\left[A\right],mol{L}^{-1}$	$\left[{\text{B}}_{\text{2}}\right]{\text{ mol L}}^{-1}$	Rate $mol{L}^{-1},S^{-1}$
0.5	0.5	$1.6\times {10}^{-4}$
0.5	1.0	$3.2\times {10}^{-4}$
1.0	1.0	$3.2\times {10}^{-4}$

keeping [A] constant doubling $\left[B_2\right],$ the rate is doubled. hence, order with reject to $B_2$ is 1

Keeping $\left[B_2\right]$ constant, doubling[A] there is no change in the rate. hence order with respect to ‘A’ is zero

$\therefore$the rate equation is $= K{\left[A\right]}^0\left[B_2\right]$