Home
Class 12
CHEMISTRY
For a reaction, the rate constant is exp...

For a reaction, the rate constant is expressed as `k = Ae^(-40000//T)`. The energy of the activation is

A

40000cal

B

88000cal

C

80000cal

D

8000cal

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Similar Questions

Explore conceptually related problems

Rate constant for a chemical reaction taking place at 500K is expressed as K=A. e^(-1000) The activation energy of the reaction is :

The temperature dependence of the rate constant k is expressed as k = Ae^(-Ea//RT) When a plot between logk and 1/T is plotted we get the graph as shown. What is the value of slopw in the graph?

The rate of a reaction depends upon the temperature and is quantitatively expressed as k=Ae^((-Ea)/(RT) i) If a graph is plotted between log k and 1/T, write the expression for the slope of the reaction? ii) If at under different conditions E_(a1)andE_(a2) are the activation energy of two reactions. If E_(a1) = 40 J// "mol and" E_(a2) = 80 J//" mol" . Which of the two has a larger value of the rate constant?

According to Arrhenius equation rate constant k is equal to Ae^(-E_(a)//RT) . Which of the following option. Represents the graph of ln k us (1)/(T) ?

According to Arrhenius equation rate constant k is equal to Ae^(-E_(a)//RT) . Which of the following option. Represents the graph of ln k us (1)/(T) ?

The rate constant for the decompoistion of a certain reaction is described by the equation: log k(s^(-1)) = 14 - (1.25 xx 10^(4) K)/(T) What is the effect on the rate of reaction at 127^(@)C , if in the presence of catalyst, energy of activation is lowered by 10 kJ mol^(-1) ?

Will the rate constant of the reaction depend upon T if the E_act (activation energy) of the reaction is zero?

The slope of the line in the graph of logk (k = rate constant) versus 1/T for a reaction is - 5841 K. Calculate the energy of activation for this reaction. [R = 8.314 JK^(-1) mol^(-) ]