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The rate equation for the reaction $2A+B\rightarrow C$ is found to be : rate $=k\left [ A \right ]\left [ B \right ].$ The correct statement in relation to this reaction is that the

Option 1)
unit of $k$ must be s^-1

Option 2)
$t_{1/2}$ is a constant

Option 3)
rate of formation of $C$ is twice the rate of disappearance of $A$

Option 4)
value of $k$ is independent of the initial concentrations of $A$ and $B$

Answers (1)

best_answer

As we learnt in

First Order Reaction -

The rate of the reaction is proportional to the first power of the concentration of the reaction

- wherein

Formula:

R $\rightarrow$ P

a 0

a-x x

$rate[r]=K[R]^{1}$

$\frac{-d(a-x)}{dt}=K(a-x)$

$\frac{-dx}{dt}=K(a-x)$ [differentiate rate law]

$ln \:[\frac{a}{a-x}]=kt \:(Integrated rate law)$

Unit of $k=sec^{-1}$

$t_\frac{1}{2}=\frac{0.693}{k}$

rate= k[A] [B]

According to rate law equation order of reaction with respect to A and with respect to B is first order so value of k is independent of the initial concentration of A and B.

Option 1)

unit of $k$ must be s^-1

Incorrect Option

Option 2)

$t_{1/2}$ is a constant

Incorrect Option

Option 3)

rate of formation of $C$ is twice the rate of disappearance of $A$

Incorrect Option

Option 4)

value of $k$ is independent of the initial concentrations of $A$ and $B$

Correct Option

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