The rate of chemical reaction are strongly affected by temperature . Arrhenius (1889) gave following relation between rate contant and temperature .
`k=Ae^(-E_(a)//RT)" ".....(i)`
This equation is called Arrhenius equation. The constant 'A' is caleld Arrhenius of pre-exponential factor. Logarithm of equation (i) given :
`log_(10)k=log_(10)A(E_(a))/(2.3030RT)" ".....(ii)`
The rate constant for a reaction is .
`log_(10)"sec"^(-1)=14-(1.25xx10^(4)K)/(T) " ".....(iii)`
Energy of activation in K cal `"mol"^(-1)` is:

Options

A. `14 K "cal mol"^(-1)`
B. `57.6 K "cal mol"^(-1)`
C. `1.25xx10^(4) K "cal mol"^(-1)`
D. `(14)/(1.25xx10^(4)) K "cal mol"^(-1)`

Answer

B