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Introduction

The reaction ...

Question

The reaction $2 A + B + C \to D + E$ is found to be first order in A second order in B and zero order in C.
How many times rate increases if concentrations of A,B and C increases by two times?

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Solution

The correct option is A 8
According to given conditions,
$\frac{d x}{d t} = k [A] [B^{2}]$
Also,
$r_{2} = k [2 A] [2 B]^{2} = 8 k A B^{2} = 8 r_{1}$

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2 A + B + C \to D + E

2 A + B + C \to D + 2 E

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2 A + B + C \to P r o d u c t

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A reaction is first order in A and second order in B:

Write the differential rate equation.

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How is the rate affected when the concentrations of both A and B are doubled?

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