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

Solution

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

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