Question

The experimental data for the reaction $2A+B_2⟶2AB$, is:

Expt. No.	$\left[A\right]$	$\left[B_2\right]$	Rate $\left(mol{L}^{-1}{s}^{-1}\right)$
$1.$	$0.50$	$0.50$	$1.6\times {10}^{-4}$
$2.$	$0.50$	$1.00$	$3.2\times {10}^{-4}$
$3.$	$1.0$	$1.00$	$3.2\times {10}^{-4}$

The rate equation for the above data is:

• A. Rate $=k{\left[B_2\right]}^2$
• B. Rate $=k\left[B_2\right]$
• C. Rate $=k{\left[A\right]}^2{\left[B\right]}^2$
• D. Rate $=k{\left[A\right]}^2\left[B\right]$

Answer 1

The correct option is B Rate $=k\left[B_2\right]$

On dividing equation (iii) by (ii), we get ,

$2^x=2^0$

$x$ = 0

now divide eq(ii) by eq(i)

we get ,

y= 1

Thus rate eq is

$\therefore Rate=k\left[A{]}^0\right[B_2]=k[B_2]$