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Questions  

For the non-stoichiometric reaction 2A+BC+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 M0.1 M1.2×10-3
0.1 M0.2 M1.2×10-3
0.2 M0.1 M2.4×10-3

The rate law for the formation of C is

a
dCdt=k[A][B]
b
dCdt=k[A]2[B]
c
dCdt=k[A][B]2
d
dCdt=k[A]

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

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Similar Questions

Following data is given for the reaction,X+YP

Experiment[X] mol L1[Y] mol L1Initial rate mol L1s1
I2.5×10-46×10-55×10-4
II5×10-412×10-54×10-3
III1×10-312×10-51.6×10-2

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


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