The results given in the below table were obtained during kinetic studies of the following reaction: $2 A + B \to C + D$

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 $2.88 \times 10^{- 1}$

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: $2 A + B \to C + D$

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	$2.88 \times 10^{- 1}$

X and Y in the given table are respectively :

Aicharya · Accepted Answer

$ 	ext{Rate} = k[A]^a[B]^b $ from Exp $(1) \& (2)$, $b = 2$ from Exp $(1) \& (3)$, $a = 1$ from Exp $(2) \& (4) ightarrow 3 = \left(\frac{x}{0.1}ight)^1$ so $x = 0.3$ from Exp $(1) \& (5) ightarrow 48 = 3^1\left(\frac{y}{0.1}ight)^2$ $4^2 = \left(\frac{y}{0.1}ight)^2$ so $y = 0.4$

The results given in the below table were obtained during kinetic studies of the following reaction: 2 A + B…

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