The results given in the below table were obtained during kinetic studies of the following reaction: 2 A + B → C + D Experiment A / molL - 1 B / molL - 1 Initial rate/ molL - 1 min - 1 I 0 . 1 0 . 1 6 . 00 × 10 - 3 II 0 . 1 0 . 2 2 . 40 × 10 - 2 III 0 . 2 0 . 1 1 . 20 × 10 - 2 IV X 0 . 2 7 . 20 × 10 - 2 V 0 . 3 Y 2 . 88 × 10 - 1 X and Y in the given table are respectively :

Question

The results given in the below table were obtained during kinetic studies of the following reaction: 2 A + B → C + D Experiment A / molL - 1 B / molL - 1 Initial rate/ molL - 1 min - 1 I 0 . 1 0 . 1 6 . 00 × 10 - 3 II 0 . 1 0 . 2 2 . 40 × 10 - 2 III 0 . 2 0 . 1 1 . 20 × 10 - 2 IV X 0 . 2 7 . 20 × 10 - 2 V 0 . 3 Y 2 . 88 × 10 - 1 X and Y in the given table are respectively :, 0 . 4 , 0 . 4, 0 . 4 , 0 . 3, 0 . 3 , 0 . 4, 0 . 3 , 0 . 3

MARKS App · Accepted Answer

Rate = k [ A ] a [ B ] b from Exp 1 & 2 b = 2 from Exp 1 & 3 a = 1 from Exp 2 & 4 ⇒ 3 = x 0 . 1 1 so x = 0 . 3 from Exp 1 & 5 ⇒ 48 = 3 1 y 0 . 1 2 4 2 = y 0 . 1 2 so y = 0 . 4

Experiment	$[A] / {molL}^{- 1}$	$[B] / {molL}^{- 1}$	Initial rate/ ${molL}^{- 1} \min^{- 1}$
I	$0.1$	$0.1$	$6.00 \times 10^{- 3}$
II	$0.1$	$0.2$	$2.40 \times 10^{- 2}$
III	$0.2$	$0.1$	$1.20 \times 10^{- 2}$
IV	X	$0.2$	$7.20 \times 10^{- 2}$
V	$0.3$	Y	$2.88 \times 10^{- 1}$

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