For the non-stoichiometry reaction, 2 A + B → C + D , the following kinetic data were obtained in three separate experiments, all at 298 K . Initial Concentration (A) Initial Concentration (B) Initial

Question

For the non-stoichiometry reaction, 2 A + 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 × 1 0 - 3 0.1 M 0.2 M 1.2 × 1 0 - 3 0.2 M 0.1 M 2.4 × 1 0 - 3 The rate law for the formation of C is

TestHub · Accepted Answer

To determine the rate law, we analyze how the initial rate changes with reactant concentrations.

From experiments I and II, doubling [B] while keeping [A] constant does not change the rate, so the reaction is zero order with respect to B ( $y = 0$ ).

From experiments I and III, doubling [A] while keeping [B] constant doubles the rate, so the reaction is first order with respect to A ( $x = 1$ ).

Thus, the rate law is:

$R a t e = k [A]^{1} [B]^{0} = k [A]$

Initial Concentration (A)	Initial Concentration (B)	Initial rate of formation of C $({mol L}^{-} S^{-})$
$0.1 M$	$0.1 M$	$1.2 \times 1 0^{- 3}$
$0.1 M$	$0.2 M$	$1.2 \times 1 0^{- 3}$
$0.2 M$	$0.1 M$	$2.4 \times 1 0^{- 3}$

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