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 rate constant of the reaction is -

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Byju's Answer

Standard XII

Chemistry

Characteristics of Equilibrium Constant

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 rate constant of the reaction is _________ .

4.0 \times 10^{- 2}

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3.0 \times 10^{- 2}

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1.0 \times 10^{- 2}

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2.0 \times 10^{- 2}

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Solution

The correct option is D $4.0 \times 10^{- 2}$
Form the data it can be observed that when the concentration of A is kept same and the concentration of B is changed, the rate of the reaction is same. The reaction is of zero-order in B.

When the concentration of A is increased five times, the rate of the reaction increases by 25 times. The reaction is of second order in A.

The expression for the rate constant is $k = \frac{r}{[A]^{2} [B]^{0}} .$

Substitute values in the above expression.

$k = \frac{4.0 \times 10^{- 4}}{(0.1)^{2} (0.1)^{0}} = 4.0 \times 10^{- 2} L m o l^{- 1} s^{- 1} .$

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Similar questions

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?

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 :

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. The following initial rate data were obtained for the reaction:

2 N O (g) + {B r}_{2} (g) \to 2 N O B r (g)

Run	$[N O] / M$	$[{B r}_{2}] / M$	$R a t e / M {m i n}^{- 1}$
$1.$	$1.0$	$1.0$	$1.30 \times 10^{- 3}$
$2.$	$2.0$	$1.0$	$5.20 \times 10^{- 3}$
$3.$	$4.0$	$2.0$	$4.16 \times 10^{- 2}$

Determine the reaction rate law and the value of the rate constant.

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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 rate constant of the reaction is _________ .