The rate constant is doubled when temperature increases from $27^{\circ} C$ to $37^{\circ} C$. What is the activation energy in $kJ \ mol^{-1}$?

The rate of the process doubles with every $10 \ K$ increase in temperature. When the temperature is increased from $303 \ K$ to $353 \ K$,how much will the rate of the process increase?

An egg takes $4.0 \text{ minutes}$ to boil at sea level where the boiling point of water is $T_1 \text{ K}$,whereas it takes $8.0 \text{ minutes}$ to boil on a mountain top where the boiling point of water is $T_2 \text{ K}$. The activation energy for the reaction that takes place during the boiling of an egg is:

If the rate of a reaction doubles when the temperature increases from $298 \, K$ to $308 \, K$,the activation energy of the reaction is ........... $kJ \, mol^{-1}$.

The specific rate constant of decomposition of a compound is given by $\ln k = 5.0 - \frac{12000}{T}$. The activation energy of decomposition for this compound at $300 \ K$ is

Which one of the following does not represent the Arrhenius equation?