Home
Class 12
CHEMISTRY
Consider the reaction. The rate co...

Consider the reaction.

The rate constant for two parallel reactions were found to be `10^(-2) dm^(-2)mol^(-1)s^(-1)` and `4xx10^(-2)dm^(-3)mol^(-1)s^(-1)` . If the corresponding energies of activation of the parallel reaction are 100 and 120 kJ/mol respectively, what is the net energy of activation `(E_(a))` of A

A

100 kJ/mol

B

120 kJ/mol

C

116 kJ/mol

D

220 kJ/mol

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Similar Questions

Explore conceptually related problems

The substance undergoes first order decomposition.The decomposition follows two parallel first order reactons as : K_1=10^(-2) sec^(-1) and K_2=4 * 10^(-2)sec^(-1) If the corresponding activation energies of parallel reaction are 100 and 120 kJ "mol"^(-1) then the net activation energy of A is/are:

The value of rate constant for a second order reaction is 6.7 xx 10^(-5) mol^(-) L s^(-) at 298 K and 1.64 xx 10^(-4) mol^(-) L s^(-) at 313 K. Find the Arrhenius frequency factor A and activation energy of the reaction.

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4kJ/mol respectively. The reaction is:

The rate constant of a reaction is 1.2 xx10^(-3) s^(-1) at 30^@C and 2.1xx10^(-3)s^(-1) at 40^@C . Calculate the energy of activation of the reaction.

Rate constant k = 1.2 xx 10^(3) mol^(-1) L s^(-1) and E_(a) = 2.0 xx 10^(2) kJ mol^(-1) . When T rarr oo :

The rate constant for the reaction in gaseous phase O+O_(3) rarr 2O_(2) is 8.0xx10^(-15)" cm"^(3)" molecule"^(-1) s^(-1) at 298 K. Corresponding value in dm^(3)" mol"^(-1) s^(-1) is :