Question

Select the rate law that corresponds to the data shown for the following reaction: $A+B\to C$

Exp.	$\left[A\right]$	$\left[B\right]$	Initial rate
$1$.	$0.012$	$0.035$	$0.10$
$2$.	$0.024$	$0.070$	$1.6$
$3$.	$0.024$	$0.035$	$0.20$
$4$.	$0.012$	$0.070$	$0.80$

• 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

Answer: (C)

Rate $=K\left[A\right][B{]}^3$

Exp	[A]	[B]	Initial rate
1.	0.012	0.035	0.10
2.	0.024	0.070	1.6
3.	0.024	0.035	0.20
4.	0.012	0.070	0.80

From $\left(1\right)\&\left(4\right)$

On doubling $\left[B\right],$ initial rate become ${\left(2\right)}^3$ times.

order wrt $B=3$

From $\left(1\right)\&\left(3\right)$ On doubling $\left[A\right],$ initial rate becomes ${\left(2\right)}^1$ times

Order wrt $A=1$

$\therefore$ rate $=k\left[A\right]{\left[B\right]}^3$