In a reaction between A and B- the initial rate of reaction r 0- was measured for different initial concentrations of A and B as given below-A - mol L -1 0-20 0-20 0-40 B - mol L -1 0-30 0-10 0-05 r 0 - mol L -1 s -1 5-07 - 10-5 5-07 - 10-5 1-43 - 10-4 What is the order of the reaction with respect to A and B-

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Standard XII

Chemistry

Molecularity of Reaction

In a reaction...

Question

In a reaction between A and B, the initial rate of reaction (r₀) was measured for different initial concentrations of A and B as given below:

A/ mol L⁻¹

0.20

0.20

0.40

B/ mol L⁻¹

0.30

0.10

0.05

r₀/ mol L⁻¹ s⁻¹

5.07 × 10⁻⁵

5.07 × 10⁻⁵

1.43 × 10⁻⁴

What is the order of the reaction with respect to A and B?

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Solution

Let the order of the reaction with respect to A be x and with respect to B be y.

Therefore,

Dividing equation (i) by (ii), we obtain

Dividing equation (iii) by (ii), we obtain

= 1.496

= 1.5 (approximately)

Hence, the order of the reaction with respect to A is 1.5 and with respect to B is zero.

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Similar questions

Q. In a reaction between

A

and

B

, the initial rate of reaction

(r_{0})

was measured for different initial concentrations of

A

and

B

as given below:

$A / m o l L^{- 1}$	$0.20$	$0.20$	$0.40$
$B / m o l L^{- 1}$	$0.30$	$0.10$	$0.05$
$r_{0} / m o l L^{- 1} s^{- 1}$	$5.07 \times 10^{- 5}$	$5.07 \times 10^{- 5}$	$1.43 \times 10^{- 4}$

What is the order of the reaction with respect to

A

and

B

In a reaction between A and B the initial rate of reaction $(r_{0})$ was measured for different initial concentrations of A and B as given below.
$\begin{matrix} A / m o l L^{- 1} & 0.20 & 0.20 & 0.40 B / m o l L^{- 1} & 0.30 & 0.10 & 0.05 x_{0} / m o l L^{- 1} s^{- 1} & 5.07 \times 10^{- 5} & 5.07 \times 10^{- 5} & 1.43 \times 10^{- 4} \end{matrix}$
What is the order to the reaction with respect to A and B?

Q. In a reaction between

A

and

B

, initial rate of reaction was measured for different initial concentration

A

and

B

given as:

$[A]$ in mol $L^{- 1}$	$[B]$ in mol $L^{- 1}$	Initial rate in mole $L^{- 1} s^{- 1}$
0.2	0.3	$5.07 \times 10^{- 5}$
0.2	0.1	$5.07 \times 10^{- 5}$
0.4	0.05	$1.47 \times 10^{- 4}$

Order of reaction with respect to

A

and

B

is:

The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:

Experiment	A/ mol L⁻¹	B/ mol L⁻¹	Initial rate/mol L⁻¹ min⁻¹
I	0.1	0.1	2.0 × 10⁻²
II	--	0.2	4.0 × 10⁻²
III	0.4	0.4	--
IV	--	0.2	2.0 × 10⁻²

Q. What is the rate law expression for the reaction,

A + B \to C

?
The following data were collected from the experiments:

Expt. No.	Initial $[A]$ $(m o l L^{- 1})$	Initial $[B]$ $(m o l L^{- 1})$	Rate of formation of $C$
$1.$	$0.10$	$0.10$	$4.0 \times 10^{- 4}$
$2.$	$0.20$	$0.20$	$3.2 \times 10^{- 3}$
$3.$	$0.10$	$0.20$	$1.6 \times 10^{- 3}$

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A/ mol L⁻¹	0.20	0.20	0.40
B/ mol L⁻¹	0.30	0.10	0.05
r₀/ mol L⁻¹ s⁻¹	5.07 × 10⁻⁵	5.07 × 10⁻⁵	1.43 × 10⁻⁴

Let the order of the reaction with respect to A be x and with respect to B be y. Therefore, Dividing equation (i) by (ii), we obtain Dividing equation (iii) by (ii), we obtain = 1.496 = 1.5 (approximately) Hence, the order of the reaction with respect to A is 1.5 and with respect to B is zero.