For the non‑stoichiometre reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments, all at 298 K. Initial Concentration (A) Initial Concentration (B) Initial rate of Formation of C (mol L–S–) 0.1 M 0.1 M 1.2 × 10–3 0.1 M 0.2 M 1.2 × 10–3 0.2 M 0.1 M 2.4 × 10

Engineering

Chemistry

Methods of Determination of Order of Reaction

Question

For the non‑stoichiometre reaction 2A + B → C + D, the following kinetic data were obtained in three separate experiments, all at 298 K.

Initial Concentration (A)	Initial Concentration (B)	Initial rate of Formation of C (mol L^–S^–)
0.1 M	0.1 M	1.2 × 10^–3
0.1 M	0.2 M	1.2 × 10^–3
0.2 M	0.1 M	2.4 × 10^–3

The rate law for the formation of C is

$\frac{dc}{dt} = k [A] {[B]}^{2}$

$\frac{dc}{dt} = k [A] [B]$

$\frac{dc}{dt} = k [A]$

$\frac{dc}{dt} = k {[A]}^{2} [B]$

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Rate = k[A]^x [B]^y

${[\frac{A_{1}}{A_{2}}]}^{x} {[\frac{B_{1}}{B_{2}}]}^{y}$

From 1 and 2

$\frac{1 .2 \times 10^{- 3}}{1 .2 \times 10^{- 3}} = {[\frac{0 .1}{0 .1}]}^{x} {[\frac{0 .1}{0 .2}]}^{y}$

y = 0

From 1 and 3

$= \frac{1 .2 \times 10^{- 3}}{2 .4 \times 10^{- 3}} = {[\frac{0 .1}{0 .2}]}^{x} {[\frac{0 .1}{0 .1}]}^{y}$

x = 1

$Rate = \frac{dc}{dt} = k [A]$