If the activation energy of a reaction is 50 kJ mol^(-1), then prove that increasing the temperature from 300K to 310K...

What is the activation energy (KJ/mol) for a reaction if its rate constant doubles when the temperature is raised from 300 K to 400 K ? (R="8.314 J mol"^(-1)"K"^(-1))

The activation energy of a reaction is 9.0 kcal//mol . The increase in the rate consatnt when its temperature is increased from 298 K to 308 K is

The activation energy for most of the reaction is approximately 50 kJ mol^(-1) The value of temperature coefficient for such reaction will be

A reaction has an activation energy of 209 KJ "mol"^(-1) . The rate increase 10-fold when the temperature is increased from 27^(@)C to X ""^(@)C . The temperature X is closed to [Gas constant, R = 8.314 J "mol"^(-1) K^(-1) ]