Question

Select the law that corresponds to data shown for the following reaction;
$A+B\to Products$

Exp.	$\left[A\right]$	$\left[B\right]$	Initial rate
$1$	$0.012$	$0.035$	$0.1$
$2$	$0.024$	$0.070$	$0.8$
$3$	$0.024$	$0.035$	$0.1$
$4$	$0.012$	$0.070$	$0.8$

• A. $rate=k[B{]}^3$
• B. $rate=k[B{]}^4$
• C. $rate=k\left[A\right][B{]}^3$
• D. $rate=k\left[A{]}^2\right[B{]}^2$

Answer 1

The correct option is A $rate=k[B{]}^3$

$\begin{array}{c}Rate=k{\left(A\right)}^x{\left(B\right)}^y\\ \\ \frac{r_2}{r_1}=\frac{0.8}{0.1}=\frac{k{\left(0.024\right)}^x{\left(0.070\right)}^y}{k{\left(0.012\right)}^x{\left(0.035\right)}^y}\Rightarrow {\left(2\right)}^{x+y}=8,x+y=3\\ \\ \frac{r_1}{r_3}=1={\left(\frac{1}{2}\right)}^x\\ \\ So,x=0\&y=3\\ \\ Thus,Rate=k{\left[B\right]}^3\end{array}$

Option A is correct.