How much faster would a reaction proceed at `25^(@)C` than at `0^(@)C` if the activation energy is 65 kJ?

The rate of reaction ((dx)/(dt)) varies with nature, physical state and concentration of reactants, temperature, exposure to light and catalyst, whereas rate constant (K) varies with temperature and catalyst only. The rate constant K is given as K=Ae^(-E_(a)//RT) where A is Arrhenius parameter or pre-exponential factor and E_(a) is energy of activation. The minimum energy required for a reaction is called threshold energy and the additional energy required by reactant molecules to attain threshold energy level is called energy of activation. How much faster would a reaction proceed at 25^(@)C than at 0^(@)C if the activation energy is 2 cal?

The rate of a reaction at 75^(@) C is 30.0 times that at 25^(@) C . What is its activation energy?

The rate of a reaction at 37^(@)C is twice the rate of the reaction at 27^(@)C . The activation energy (kJ.mol^(-1)) of the reaction is -

A reaction proceeds five times more at 60^(@)C as it does at 30^(@)C . Estimate energy of activation.

The energy of activation for a reaction is 100 kJ/mol at 57^(@)C . Presence of catalyst lower activation energy by 25%. The rate of reaction is increased by 10^(x) the value of x is

The ezyme catalysed reaction is faster than a metal catalysed reaction because its activation energy is :

A 1st order reaction is 50% complete in 30 minute at 27^(@)C and in 10 minute at 47^(@)C . Calculate the: (a) Rate constant for reaction at 27^(@)C and 47^(@)C . (b) Energy of activation for the reaction. (c ) Energy of activation for the reverse reaction if heat of reaction is -50 kJ mol^(-1) .