"Activation energies are low for fast reaction and high for slow reactions" a) Justify the statement. b) The rate of a reaction quadruples when the temperature changes from 310 K to 330 K. Calculate the activation, energy of the reaction `R=8.314 Jk^(-1) (mol)^(-1)`

Explanation

If `(E)_(a)` is low. large number of molecules can have this energy. So number of effective collision will be large. So such reactions have high speed. If the activation energy is high, less number of molecules have the activation energy, so reaction rate will be low.
b. `log (k)_(2))(k)_(1)=(Ea)(2.303R)[((T)_(2)-(T)_(1))(T)_(1) (T)_(2)`
`log 4=(E)_(a)(2.303 * 8.314) (20)(310 * 330)`
`0.6021=(E)_(a) * 20)(2.303 xx 8.314 xx 310 xx 330)`
`E_(a)=(0.6021 * 2.303 * 8.314 * 310 * 330)(20)`
=58968=58.97 (kJ) / (mol)`