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)

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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