A first order reaction has a half life period of `69.3` s. The rate of reaction when the concentration of reactant is `0.1M`.
`10^(-4)Ms^(-1)`
`10^(-3)Ms^(-1)`
`10^(-1)Ms^(-1)`
`6.93times10^(-1)Ms^(-1)`

The half-life period of a first order reaction having rate constant k=0.231×10^(−10)s^(−1) will be:

The rate constant of first order reaction is 10^(-2)"min"^(-1) . The half-life period of reaction is

After how many seconds will the concentration of the reactant in a first order reaction be halved if the rate constant is 1.155xx10^(-3)s^(-1) ?

The rate of first-order reaction is 1.5 xx 10^(-2) M "min"^(-1) at 0.5 M concentration of reactant. The half-life of reaction is

A first order reaction is found to have a rate constant k= 5.5 xx 10^(-14)s^(-1) . Find half-life of the reaction.

Identify the reaction order from each of the following rate : k=3.1 xx 10^(-4) s^(-1)

The rate of a reaction increases four-fold when the concentration of reactant is increased 16 times. If the rate of reaction is 4 xx 10^(-6) mol L^(-1) s^(-1) when the concentration of the reactant is 4 xx 10^(-4) mol L^(-1) . The rate constant of the reaction will be

A first order reaction has a rate constant of 0.0051 "min"^(-1) . If we begin with 0.10M concentration of the reaction , what concentration of reactant will remain in solution after 3 hours ?