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Question

Reaction $$\:A+2B+C\rightarrow product$$, follows the rate law$$\displaystyle-\frac{d\left[C\right]}{d\,t}\,=\,k\left[A\right]^2$$
False statement regarding the above reaction is :


A
On doubling the conc. of B and C the rate of the reaction remains unaffected
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B
Reducing the conc. of A to half, the rate becomes one-fourth
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C
Half life period of the reaction depends upon the conc. of B
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D
Half life period of the reaction is inversely proportional to the first power conc. of A
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Solution

The correct option is C Half life period of the reaction depends upon the conc. of B
Half life period of the reaction depends upon the concentration of A and is independent of the concentration of B.     

Chemistry
NCERT
Standard XII

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