The temperature-dependent equation for the rate constant is written as:

What will be the effect on the fraction of molecules and the rate constant on increasing temperature?

The rate of a reaction quadruples when the temperature changes from $300 \, K$ to $310 \, K$. The activation energy of this reaction is ........... $kJ \, mol^{-1}$ (Assume activation energy and pre-exponential factor are independent of temperature; $\ln 2 = 0.693$; $R = 8.314 \, J \, mol^{-1} \, K^{-1}$)

Subtract $(i)$ $\ln \, k_1 = - \frac{E_a}{R T_1} + \ln A$ and $(ii)$ $\ln \, k_2 = - \frac{E_a}{R T_2} + \ln A$ and write the resulting equation.

According to the Arrhenius equation,which of the following statements is correct?

What is the slope of the graph between $\ln K$ and $\frac{1}{T}$ according to the Arrhenius equation?