For the reaction A 2 -2B- 2AB- the following data were observed-Exp- No- - A - - B - Rate mol L -1 s -1 1- 0-1 0-01 1-5- 10 -3 2- 0-1 0-04 6-0- 10 -3 3- 0-2 0-01 3-0- 10 -3The overall order of the reaction will be-

The correct option is B 2 Let rate = k[A_z]^x[B]^y 1.5× 10^ 3=k(0.1)^x(0.01)^y (1) 6× 10^ 3=k(0.1)^x(0.04)^y (2) 3× 10^ 3=k(0.2)^x(0.01 ...

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Byju's Answer

Standard XII

Chemistry

Activation Energy

For the react...

Question

For the reaction $A_{2} + 2 B ⟶ 2 A B$ , the following data were observed:
Exp. No. $[A]$ $[B]$ Rate
$(m o l L^{- 1} s^{- 1})$
$1.$ $0.1$ $0.01$ $1.5 \times 10^{- 3}$
$2.$ $0.1$ $0.04$ $6.0 \times 10^{- 3}$
$3.$ $0.2$ $0.01$ $3.0 \times 10^{- 3}$
The overall order of the reaction will be:

1

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Solution

The correct option is B $2$
Let rate = $k [A_{z}]^{x} [B]^{y}$
$1.5 \times 10^{- 3} = k (0.1)^{x} (0.01)^{y}$ -(1)
$6 \times 10^{- 3} = k (0.1)^{x} (0.04)^{y}$ -(2)
$3 \times 10^{- 3} = k (0.2)^{x} (0.01)^{y}$ -(3)
From (1) and (2), $\frac{1.5}{6} = (\frac{1}{4})^{y} => y = 1$
From (1) and (3), $\frac{1.5}{3} = (\frac{1}{2})^{x} => x = 1$
Overall order $= x + y = 2$

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Similar questions

Q. For a reaction

A + 2 B \to C + D

, the following data were obtained.
Excpt. Initial concentration Initial Rate of formation of D
(moles

{l i t r e}^{- 1}

)

{l i t r e}^{- 1} {m i n}^{- 1}

)
[A] [B]
1.

0.1

0.1

6.0 \times 10^{- 3}

0.3

0.2

7.2 \times 10^{- 2}

0.3

0.4

2.8 \times 10^{- 1}

0.4

0.1

2.4 \times 10^{- 2}

The correct rate law expression will be:

Q. For a reaction

A + 2 B \to C + D

, the following data were obtained

The correct rate law expression will be

Q. Following data are given for the reaction between

A

and

B

$[A] / m o l L^{- 1}$	$[B] / m o l L^{- 1}$	Initial rate/ $m o l L^{- 1} s^{- 1}$ at $300 K$	$320 K$
$2.5 \times 10^{- 4}$	$3.0 \times 10^{- 5}$	$5.0 \times 10^{- 4}$	$2.0 \times 10^{- 3}$
$5.0 \times 10^{- 4}$	$6.0 \times 10^{- 5}$	$4.0 \times 10^{- 3}$	-
$1.0 \times 10^{- 3}$	$6.0 \times 10^{- 5}$	$1.6 \times 10^{- 2}$	-

The rate constant at

300 K

is:

Expt. No.	$[A]$ $(m o l L^{- 1})$	$[B]$ $(m o l L^{- 1})$	Initial rate $(m o l L^{- 1} s^{- 1})$
Expt. No.	$[A]$ $(m o l L^{- 1})$	$[B]$ $(m o l L^{- 1})$	300K	320K
(1)	$2.5 \times 10^{- 4}$	$3.0 \times 10^{- 5}$	$5.0 \times 10^{- 4}$	$2.0 \times 10^{- 3}$
(2)	$5.0 \times 10^{- 4}$	$6.0 \times 10^{- 5}$	$4.0 \times 10^{- 3}$	$. . .$
(3)	$1.0 \times 10^{- 3}$	$6.0 \times 10^{- 5}$	$1.6 \times 10^{- 2}$	$. . .$

From the data given above for the reaction between

A

and

B

, calculate the following:
(i) The order of the reaction with respect to

A

and with respect to

B

,
(ii) The rate constant at

300

K

(iii) The energy of activation and
(iv) The pre-exponential factor.

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 _________ .

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Exp. No.	$[A]$	$[B]$	Rate $(m o l L^{- 1} s^{- 1})$
$1.$	$0.1$	$0.01$	$1.5 \times 10^{- 3}$
$2.$	$0.1$	$0.04$	$6.0 \times 10^{- 3}$
$3.$	$0.2$	$0.01$	$3.0 \times 10^{- 3}$

For the reaction A2+2B⟶2AB, the following data were observed:Exp. No.[A][B] Rate(mol L−1s−1)1.0.10.011.5×10−32.0.10.046.0×10−33.0.20.013.0×10−3The overall order of the reaction will be:

The correct option is B 2Let rate =k[Az]x[B]y1.5×10−3=k(0.1)x(0.01)y-(1)6×10−3=k(0.1)x(0.04)y-(2)3×10−3=k(0.2)x(0.01)y-(3)From (1) and (2), 1.56=(14)y=>y=1From (1) and (3), 1.53=(12)x=>x=1Overall order=x+y=2

For the reaction $A_{2} + 2 B ⟶ 2 A B$ , the following data were observed:
Exp. No. $[A]$ $[B]$ Rate
$(m o l L^{- 1} s^{- 1})$
$1.$ $0.1$ $0.01$ $1.5 \times 10^{- 3}$
$2.$ $0.1$ $0.04$ $6.0 \times 10^{- 3}$
$3.$ $0.2$ $0.01$ $3.0 \times 10^{- 3}$
The overall order of the reaction will be: