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 -

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

A reaction proceeds 5 times more at 60^(@)C , as it does at 30^(@)C . Calculate the energy of activation.

A reaction proceeds 5 times more at 60^(@)C , as it does at 30^(@)C . Calculate the energy of activation.

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