The following are the data for the reaction A-B- products -A- -B- Initial rate mol L-1s-1i 0-1 M 0-1 M 4-0- 10-4ii 0-2 M 0-2 M 1-6- 10-3iii 0-5 M 0-1 M 1-0- 10-2iv 0-5 M 0-5 M 1-0- 10-2 The reaction rate when the concentration of A and B are 0-4 M and 0-7 M respectively -

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Standard XII

Chemistry

Order of Reaction

The following...

Question

The following are the data for the reaction

$A + B \to$ products

[A] [B] Initial rate $(m o l L^{- 1} s^{- 1})$
(i) 0.1 M 0.1 M $4.0 \times 10^{- 4}$
(ii) 0.2 M 0.2 M $1.6 \times 10^{- 3}$
(iii) 0.5 M 0.1 M $1.0 \times 10^{- 2}$
(iv) 0.5 M 0.5 M $1.0 \times 10^{- 2}$

The reaction rate when the concentration of A and B are 0.4 M and 0.7 M respectively :

6.4 \times 10^{- 2}

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6.4 \times 10^{- 3}

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6.4 \times 10^{- 4}

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6.4 \times 10^{- 5}

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Solution

The correct option is A $6.4 \times 10^{- 3}$
On increasing the concentration of B five times keeping the concentration of A constant, the rate doesn't change therefore the order w.r.t B is zero.

On increasing the concentration of A five times, the rate increases 25 times therefore, the order w.r.t A is two.

Rate $= k [A |^{2} [B]^{0}$

$= (4.0 \times 10^{- 2}) (0.4)^{2} (0.7)^{0}$

$= 4.0 \times 10^{- 2} \times 0.4 \times 0.4 \times 1$

$= 6.4 \times 10^{- 3}$

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Similar questions

Q. The following are the data for the reaction

A + B \to

products

[A] [B] Initial rate

(m o l L^{- 1} s^{- 1})

(i) 0.1 M 0.1 M

4.0 \times 10^{- 4}

(ii) 0.2 M 0.2 M

1.6 \times 10^{- 3}

(iii) 0.5 M 0.1 M

1.0 \times 10^{- 2}

(iv) 0.5 M 0.5 M

1.0 \times 10^{- 2}

The rate constant of the reaction is _________ .

The following are the data for the reaction

A + B \to

products

[A] [B] Initial rate

(m o l L^{- 1} s^{- 1})

(i) 0.1 M 0.1 M

4.0 \times 10^{- 4}

(ii) 0.2 M 0.2 M

1.6 \times 10^{- 3}

(iii) 0.5 M 0.1 M

1.0 \times 10^{- 2}

(iv) 0.5 M 0.5 M

1.0 \times 10^{- 2}

What is the order of the reaction?

Q. The following data are for the reaction

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

:
Conc. A Conc. B Initial Rate
(M) (M) (

m o l L^{- 1} s^{- 1}

)
0.1 0.1

4.0 \times 10^{- 4}

0.2 0.2

1.6 \times 10^{- 3}

0.5 0.1

2.0 \times 10^{- 3}

0.5 0.5

1.0 \times 10^{- 2}

(i) What is the order with respect to A and B for the reaction?
(ii) Calculate the rate constant.
(iii) Determine the reaction rate when the concentrations of A and B are 0.2 M and 0.35 M, respectively.

Q. 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	$[A] / M$	$[B] / M$	Initial rate/ $M m i n$
I	$0.1$	$0.1$	$2.0 \times 10^{- 2}$
II	....	$0.2$	$4.0 \times 10^{- 2}$
III	$0.4$	$0.4$	....
IV	....	$0.2$	$2.0 \times 10^{- 2}$

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:

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:

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The following are the data for the reaction A+B→ products [A] [B] Initial rate (molL−1s−1)(i) 0.1 M 0.1 M 4.0×10−4(ii) 0.2 M 0.2 M 1.6×10−3(iii) 0.5 M 0.1 M 1.0×10−2(iv) 0.5 M 0.5 M 1.0×10−2 The reaction rate when the concentration of A and B are 0.4 M and 0.7 M respectively :