Question

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

Expt No.	$[A{]}_{0}mole{L}^{-1}$	$[B{]}_{0}mole{L}^{-1}$	Initital rate
1.	0.012	0.035	0.10
2.	0.024	0.070	0.80
3.	0.024	0.035	0.10
4.	0.012	0.070	0.80

• A. The rate law expression for the given reaction is Rate $=k[B{]}^3$
• B. The order with respect to [A] is zero.
• C. The order with respect to [A] is one.
• D. The rate law expression for the given reaction is Rate $=k\left[A\right][B{]}^3$

Answer 1

Answer: (A), (B)

The correct options are
A The rate law expression for the given reaction is Rate $=k[B{]}^3$
B The order with respect to [A] is zero.

$rate=k\left[A{]}^m\right[B{]}^n$

$0.10=k\left[0.012{]}^m\right[0.035{]}^n$ ------ 1

$0.8=k\left[0.024{]}^m\right[0.07{]}^n$ --------- 2

$0.10=k\left[0.024{]}^m\right[0.035{]}^n$ ------- 3

$0.8=k\left[0.012{]}^m\right[0.07{]}^n$ ------- 4

On solving, we get

$m=0;n=3$

So, order with respect to A is zero and with respect to B the order is 3.