A2-2B- 2AB -A2- -B- -d-B-dt 0-1 0-2 1- 10-2Ms-1 0-2 0-2 2- 10-2Ms-1 0-2 0-4 8- 10-2Ms-1Order of reaction w-r-t- A2- B and rate constant are respectively-

The correct option is A 1, 2 and 1.25 #160; #160; [A_2] [B] #160; d[B/dt ] #160;Rate #160;1. #160;0.1 #160;0.2 1× ...

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Byju's Answer

Standard XII

Chemistry

Order of Reaction

A2+2B→ 2AB [...

Question

$A_{2} + 2 B \to 2 A B$
$[A_{2}]$ $[B]$ ${- d [B] / d t}$
$0.1$ $0.2$ $1 \times 10^{- 2} M s^{- 1}$
$0.2$ $0.2$ $2 \times 10^{- 2} M s^{- 1}$
$0.2$ $0.4$ $8 \times 10^{- 2} M s^{- 1}$
Order of reaction w.r.t. $A_{2}$ , $B$ and rate constant are respectively.

1, 2

and

1.25

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2, 1

and

5

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1, 2

and

2.5

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2, 2

and

2.5

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Solution

The correct option is A $1, 2$ and $1.25$
$[A_{2}]$ $[B]$ $- d [B / d t$ ] Rate
1. 0.1 0.2 $1 \times 10^{- 2} {M s}^{- 1}$ $5 \times 10^{- 3} {M s}^{- 1}$
2. 0.2 0.2 $2 \times 10^{- 2} {M s}^{- 1}$ $1 \times 10^{- 2} {M s}^{- 1}$
3. 0.2 0.4 $8 \times 10^{- 2} {M s}^{- 1}$ $4 \times 10^{- 2} {M s}^{- 1}$
$A_{2} + 2 B ⟶ 2 A B$
rate $= \frac{- d [A_{2}]}{d t} = \frac{- 1}{2} \frac{d [B]}{d t} = \frac{1}{2} \frac{d [A B]}{d t}$
$A_{2} + 2 B ⟶ 2 A B$
rate $= \frac{- d [A_{2}]}{d t} = \frac{- 1}{2} \frac{d [B]}{d t} = \frac{1}{2} \frac{d [A B]}{d t}$
From $(1) & (2)$
Order wrt $A_{2} = 1$
From $(2) & (3)$
Order wrt $B = 2$
Rate $= K [A_{2}] {[B]}^{2}$
Now,
From(1)
$5 \times 10^{- 3} {M s}^{- 1} = k (0.1) ({0.2)}^{2} k = \frac{5 \times 10^{- 3}}{4 \times 10^{- 3}} M^{- 2} s^{- 1} k = 1.25 M^{- 2} s^{- 1}$

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Similar questions

S. No	$[A]$	$[B]$	$[C]$	Rate of reaction
$1$	$0.2$	$0.2$	$0.2$	$2 \times 10^{- 4}$
$2$	$0.2$	$0.2$	$0.4$	$4 \times 10^{- 4}$
$3$	$0.2$	$0.4$	$0.2$	$2 \times 10^{- 4}$
$4$	$0.4$	$0.2$	$0.2$	$8 \times 10^{- 4}$

(i)

Find the order of the reaction.

(i i)

Find the rate constant.

(i i i)

Find the rate of appearance of

(i)

when

[A] = 0.1, [B] = 0.1, [C] = 0.1

Q. 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:

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	$[A] / m o l L^{- 1}$	$B] / m o l L^{- 1}$	Initial rate/ $m o l L^{- 1} m i n^{- 1}$
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 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. Find the values of A, B and C in the following table for the reaction :

X + Y ⟶ Z

The reaction is first order with respect to

X

and zero order with respect to

Y

$E x p$	$[X] (m o l L^{- 1})$	$[Y] (m o l L^{- 1})$	$I n i t i a l r a t e (m o l L^{- 1} s - 1)$
1.	$0.1$	$0.1$	$2 \times 10^{- 2}$
2.	$A$	$0.2$	$4 \times 10^{- 2}$
3.	$0.4$	$0.4$	$B$
4.	$C$	$0.2$	$2 \times 10^{- 2}$

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$[A_{2}]$	$[B]$	${- d [B] / d t}$
$0.1$	$0.2$	$1 \times 10^{- 2} M s^{- 1}$
$0.2$	$0.2$	$2 \times 10^{- 2} M s^{- 1}$
$0.2$	$0.4$	$8 \times 10^{- 2} M s^{- 1}$

	$[A_{2}]$	$[B]$	$- d [B / d t$ ]	Rate
1.	0.1	0.2	$1 \times 10^{- 2} {M s}^{- 1}$	$5 \times 10^{- 3} {M s}^{- 1}$
2.	0.2	0.2	$2 \times 10^{- 2} {M s}^{- 1}$	$1 \times 10^{- 2} {M s}^{- 1}$
3.	0.2	0.4	$8 \times 10^{- 2} {M s}^{- 1}$	$4 \times 10^{- 2} {M s}^{- 1}$

A2+2B→2AB[A2][B]{−d[B]/dt}0.10.21×10−2Ms−10.20.22×10−2Ms−10.20.48×10−2Ms−1Order of reaction w.r.t. A2, B and rate constant are respectively.

$A_{2} + 2 B \to 2 A B$
$[A_{2}]$ $[B]$ ${- d [B] / d t}$
$0.1$ $0.2$ $1 \times 10^{- 2} M s^{- 1}$
$0.2$ $0.2$ $2 \times 10^{- 2} M s^{- 1}$
$0.2$ $0.4$ $8 \times 10^{- 2} M s^{- 1}$
Order of reaction w.r.t. $A_{2}$ , $B$ and rate constant are respectively.