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Question

Consider the reaction, $$2A + B \rightarrow$$ Products, When concentration of B alone was doubled, the rate did not change. When the concentration of A alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is:


A
s1
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B
L mol1s1
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C
Unitless
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D
 mol L1s1
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Solution

The correct option is A $$s^{-1}$$
When the concentration of B alone was doubled, the rate did not change. Hence the reaction is zero order in B.

When the concentration of A alone was doubled, the rate increased by two times. Hence, the reaction is of first-order in A.

$$r=k\left [ A \right ]^{1}\left [ B \right ]^{0}$$

The overall order of the reaction is 1.

For the first-order reaction, the unit of k is $$sec^{-1}$$.

Hence, the correct option is $$\text{A}$$

Chemistry

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