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Byju's Answer

Standard XII

Chemistry

Zero Order Reaction

For a reactio...

Question

For a reaction between $A$ and $B$ , the initial rate of reaction is measured for various initial concentrations of $A$ and $B$ . The data provided are:
Expt. No. $[A]$ $[B]$ Initial reaction rate $(m o l L^{- 1} s^{- 1})$
$1.$ $0.2 M$ $0.3 M$ $5 \times 10^{- 5}$
$2.$ $0.2 M$ $0.1 M$ $5 \times 10^{- 5}$
$3.$ $0.4 M$ $0.05 M$ $7.5 \times 10^{- 5}$
The overall order of the reaction is:

1

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2

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1.5

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Between

0

and

1

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Solution

The correct option is A Between $0$ and $1$
We see $[B]$ has no impact on the rate.
Conversely on doubling $[A] :$
$\frac{v_{2}}{v_{1}} = \frac{{k [A]}^{a} {[B]}^{o}}{k {[A]}^{a} {[B]}^{o}} . 2^{a} = 7.5 / 5 2^{a} = 1.5 a \sim \frac{1}{2} \in [0, 1]$

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Similar questions

Q. For a reaction between

A

and

B

, the initial rate of reaction is measured for various initial concentrations of

A

and

B

. The data provided are

	$[A]$	$[B]$	Initial reaction rate
(a)	$0.20 M$	$0.30 M$	$5 \times 10^{- 5}$
(b)	$0.20 M$	$0.10 M$	$5 \times 10^{- 5}$
(c)	$0.40 M$	$0.05 M$	$7.5 \times 10^{- 5}$

The overall order of the reaction is

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

Q. Rate For the reaction

A + B \to p r o d u c t s

, what will be the order of reaction with respect of

A

and

B

Exp.	$[A] (m o l L^{- 1})$	$[B] (m o l L^{- 1})$	Initial rate $(m o l L^{- 1} s^{- 1})$
$1.$	$2.5 \times 10^{- 4}$	$3 \times 10^{- 5}$	$5 \times 10^{- 4}$
$2.$	$5 \times 10^{- 4}$	$6 \times 10^{- 5}$	$4 \times 10^{- 3}$
$3.$	$1 \times 10^{- 3}$	$6 \times 10^{- 5}$	$1.6 \times 10^{- 2}$

Q. For the non-stoichiometric reaction,

2 A + B ⟶ C + D

, the following kinetic data were obtained in three separate experiments, all at

298 K

Initial Concentration $[A]$	Initial Concentration $[B]$	Initial rate of formation of $C$ $(m o l L^{- 1} s^{- 1})$
$0.1 M$	$0.1 M$	$1.2 \times 10^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 10^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 10^{- 3}$

The rate law for the formation of

C

is:

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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Expt. No.	$[A]$	$[B]$	Initial reaction rate $(m o l L^{- 1} s^{- 1})$
$1.$	$0.2 M$	$0.3 M$	$5 \times 10^{- 5}$
$2.$	$0.2 M$	$0.1 M$	$5 \times 10^{- 5}$
$3.$	$0.4 M$	$0.05 M$	$7.5 \times 10^{- 5}$

For a reaction between A and B, the initial rate of reaction is measured for various initial concentrations of A and B. The data provided are:Expt. No.[A][B]Initial reaction rate (mol L−1s−1)1.0.2 M0.3 M5×10−52.0.2 M0.1 M5×10−53.0.4 M0.05 M7.5×10−5The overall order of the reaction is:

The correct option is A Between 0 and 1We see [B] has no impact on the rate. Conversely on doubling [A]: v2v1=k[A]a[B]ok[A]a[B]o.2a=7.5/52a=1.5a∼12∈[0,1]

The correct option is A Between $0$ and $1$
We see $[B]$ has no impact on the rate.
Conversely on doubling $[A] :$
$\frac{v_{2}}{v_{1}} = \frac{{k [A]}^{a} {[B]}^{o}}{k {[A]}^{a} {[B]}^{o}} . 2^{a} = 7.5 / 5 2^{a} = 1.5 a \sim \frac{1}{2} \in [0, 1]$