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 What is the order of the reaction-

The correct option is A 2The expression for the rate of the reaction, #160;Rate =k[A]^m[B]^n. From first experiment 4.0× 10^ 4=k(0.1)^m(0.1)^n .... ...

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Byju's Answer

Standard XII

Chemistry

Rate 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 $1.0 \times 10^{- 2}$

What is the order of the reaction?

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Solution

The correct option is A 2
The expression for the rate of the reaction,
Rate $= k [A]^{m} [B]^{n} .$

From first experiment $4.0 \times 10^{- 4} = k (0.1)^{m} (0.1)^{n}$ ......(1)

From third experiment $1.0 \times 10^{- 2} = k (0.5)^{m} (0.1)^{n}$ ......(2)

From the fourth experiment $1.0 \times 10^{- 2} = k (0.5)^{m} (0.5)^{n}$ ........(3)

Divide equation (2) with equation (1) :

$\frac{1 \times 10^{- 2}}{4.0 \times 10^{- 4}} = \frac{k (0.5)^{m} (0.1)^{n}}{k (0.1)^{m} (0.1)^{n}}$

$25 = (5)^{m}; m = 2$

From third and fourth experiments $\frac{1.0 \times 10^{- 2}}{1.0 \times 10^{- 2}} = \frac{k (0.5)^{m} (0.1)^{n}}{k (0.5)^{m} (0.5)^{n}}$

$1 = (\frac{1}{5})^{n} = (\frac{1}{5})^{0} = n = 0$

Total order of the reaction is $2 + 0 = 2$ .

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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}

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. For the given reaction

A + B ⟶

Products, following data were obtained:

	$[A_{0}]$	$[B_{0}]$	$R_{0} (m o l {l i t r e}^{- 1} {s e c}^{- 1})$
$1.$	$0.1$ $M$	$0.2$ $M$	$0.05$
$2.$	$0.2$ $M$	$0.2$ $M$	$0.10$
$3.$	$0.1$ $M$	$0.1$ $M$	$0.05$

(i) Write the rate law expression.
(ii) Find 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 What is the order of the reaction?