The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:

Experiment	$[A] / mol \, L^{-1}$	$[B] / mol \, L^{-1}$	Initial rate / $mol \, L^{-1} \, min^{-1}$
$I$	$0.1$	$0.1$	$2.0 \times 10^{-2}$
$II$	$-$	$0.2$	$4.0 \times 10^{-2}$
$III$	$0.4$	$0.4$	$-$
$IV$	$-$	$0.2$	$2.0 \times 10^{-2}$

(A) The given reaction is of the first order with respect to $A$ and of zero order with respect to $B$.
Therefore,the rate of the reaction is given by,
Rate $= k[A]^1[B]^0 = k[A]$
From experiment $I$:
$2.0 \times 10^{-2} \, mol \, L^{-1} \, min^{-1} = k(0.1 \, mol \, L^{-1})$
$\Rightarrow k = 0.2 \, min^{-1}$
From experiment $II$:
$4.0 \times 10^{-2} \, mol \, L^{-1} \, min^{-1} = 0.2 \, min^{-1} \times [A]$
$\Rightarrow [A] = 0.2 \, mol \, L^{-1}$
From experiment $III$:
Rate $= 0.2 \, min^{-1} \times 0.4 \, mol \, L^{-1} = 0.08 \, mol \, L^{-1} \, min^{-1}$
From experiment $IV$:
$2.0 \times 10^{-2} \, mol \, L^{-1} \, min^{-1} = 0.2 \, min^{-1} \times [A]$
$\Rightarrow [A] = 0.1 \, mol \, L^{-1}$