Questions

For the non-stoichiometric 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^-1s^-1)
0.1 M 0.1 M $1.2 \times 10^{- 3}$
0.1 M 0.2 M $1.2 \times 10^{- 3}$
0.2 M 0.1 M $2.4 \times 10^{- 3}$
The rate law for the formation of C is

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dCdt=k[A][B]

dCdt=k[A]2[B]

dCdt=k[A][B]2

dCdt=k[A]

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detailed solution

Correct option is D

This problem can be solved by determining the order of reaction with respect to each reactant and then writing rate law equation of the given equation accordingly as,R=dCdt=k[A]x[B]ywhere, x = order of reaction w.r.t A y = order of reaction w.r.t B 1.2×10−3=k(0.1)x(0.1)y1.2×10−3=k(0.1)x(0.2)y2.4×10−3=k(0.2)x(0.1)yor R=k[A]1[B]0

Similar Questions

Following data is given for the reaction, $X + Y \to P$

Experiment	$[X] mol L^{- 1}$	$[Y] mol L^{- 1}$	Initial rate $(mol L^{- 1} s^{- 1})$
I	$2.5 \times 10^{- 4}$	$6 \times 10^{- 5}$	$5 \times 10^{- 4}$
II	$5 \times 10^{- 4}$	$12 \times 10^{- 5}$	$4 \times 10^{- 3}$
III	$1 \times 10^{- 3}$	$12 \times 10^{- 5}$	$1.6 \times 10^{- 2}$

The order of reaction with respect to X and Y respectively are

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Initial concentration [A]	Initial concentration [B]	Initial rate of formation of C (mol L^-1s^-1)
0.1 M	0.1 M	$1.2 \times 10^{- 3}$
0.1 M	0.2 M	$1.2 \times 10^{- 3}$
0.2 M	0.1 M	$2.4 \times 10^{- 3}$