Question

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	$\left[A\right]/M$	$\left[B\right]/M$	Initial rate/ $Mmin$
I	$0.1$	$0.1$	$2.0\times {10}^{-2}$
II	....	$0.2$	$4.0\times {10}^{-2}$
III	$0.4$	$0.4$	....
IV	....	$0.2$	$2.0\times {10}^{-2}$

Answer 1

By the question given we get rate of equation as

$rate=k\left[A{]}^{\prime }\right[B{]}^0$

$[B{]}^{\prime }$ that is there no dependence on the concentration of B.

$\left(I\right)$ $2.0\times {10}^{-2}=K\times 0.1$

Rate Constant (K)$=\frac{2.0\times {10}^{-2}}{1\times {10}^{-1}}=2\times {10}^{-1}=0.2$

$\left(II\right)4\times {10}^{-2}=0.2\times \left[A\right]$

$\left[A\right]=\frac{4}{2}\times {10}^{-1}\times {10}^{-2}$

$\left[A\right]=2\times {10}^{-1}=0.2$

$\left(III\right)R=0.2\times 0.4$

$R=8\times {10}^{-2}$

$\left(IV\right)$ Rate $=0.2\times \left[A\right]$

$2.0\times {10}^{-2}=0.2\times \left[A\right]$

$\left[A\right]=\frac{2.0\times {10}^{-2}}{2\times {10}^{-1}}$

$\left[A\right]=0.1$