Question

Write the rate law for the reaction $A+B\to C$, from the following data:
What is the value of k?

Initial [A]/M	Initial [B]/M	Initial rate/$M{s}^{-1}$
0.4	0.2	$4.0\times {10}^{-5}$
0.6	0.2	$6.0\times {10}^{-5}$
0.8	0.4	$3.2\times {10}^{-4}$

Answer 1

$\left[A\right]$	$\left[B\right]$	Rate
$0.4$	$0.2$	$4.0\times {10}^{-5}$
$0.6$	$0.2$	$6.0\times {10}^{-5}$
$0.8$	$0.4$	$3.2\times {10}^{-4}$

A) $\therefore Rate=K{\left[A\right]}^1{\left[B\right]}^2$

B) value of $K=\frac{Rate}{\left[A\right]{\left[B\right]}^2}=\frac{4\times {10}^{-5}\times {10}^3}{0.4\times 0.04}$

$=\frac{{10}^{-2}}{4}=0.25\times {10}^{-2}$

$=2.5\times {10}^{-3}$