Define activation energy of a reaction.

Arrhenius studies the effect of temperature on the rate of a reaction and postulted that rate constant varies with temperature exponentially as k=Ae^(E_(a)//RT) . Thuis method is generally used for finding the activation energy of a reaction. Keeping temperature constant, the effect of catalyst on the activation energy has also been studied. If the rate of reaction doubles for 10^(@)C rise of temperature form 290K to 300K, the activation energy of the reaction will be approximately: a) 40 Kcal mol^(-1) b) 12 Kcal mol^(-1) c) 60 Kcal mol^(-1) d) 70 Kcal mol^(-1)

True or False : Higher the activation energy of a reaction, faster is the reaction.

What is Arrhenius equation to describe the effect of temperature on rate of a reaction ? How can it be used to calculate the activation energy of a reaction ?

The activation energy of a reaction can be determined by

The rate of a particular reaction triples, when temperature changes from 50^(@)C to 100^(@). Calculate the activation energy of the reaction.

Enzymes are biocatalysts. They catalyse biochemical reactions. In general they reduce activation energy of reactions. Many physico-chemical processess are enzyme mediate. Some examples of enzyme mediated reactions are given below. Tick the wrong entry:

At 27^@C in the presence of a catalyst, the activation energy of a reaction is lowered by 10 kJ mol^-1 . The ratio of log k (catalyst)/k (uncatalysed) is