When the temperature is increased, heat is supplied which increases the kinetic energy of the reacting molecules. This shall increase the number of collisions and ultimately the rate of reaction shall be enhanced. Arrhenius suggested a equation which describes `K` as a function of temperature, i.e.
`k=Ae^(-E_(a)//RT)`
where
`k=` rate constant
`A=` a constant (frequency factor)
`E_(a)=` energy of activation
`log_(10)k=log_(10)A-(E_(a))/(2.303R)[(1)/(R )]`
`Y=C+MX`
It is the equation of straight line with negative slope. On plotting `log_(10)k` against `[(1)/(T)]` we get a straight line as shown below :

The slope gives activation energy and intercept gives frequency factor.
Also `log.(k_(2))/(k_(1))=(E_(a))/(2.303)[(T_(2)-T_(1))/(T_(1)T_(2))]`
The rate of certain reaction increases by `2.5` times when the temperature is raised from `300K` to `310K`. If `k` is the rate constant at `300K` then rate constant at `310K` will be equal to

Options

A. `k`
B. `2k`
C. `2.5k`
D. `13k`

Answer

C