Which among the following is correct when energy of activation,$E_a$ of the catalyzed reaction decreases at constant temperature and for same concentration?

The rate constant of a first order reaction was doubled when the temperature was increased from $300 \ K$ to $310 \ K$. What is its approximate activation energy (in $kJ \cdot mol^{-1}$)? ($R = 8.3 \ J \cdot mol^{-1} \cdot K^{-1}$; $\log 2 = 0.3$)

Collision theory is used to explain how chemical species undergo a reaction. Using this theory and the kinetic molecular model,which of the following does $NOT$ influence the rate of a chemical reaction?

In the Arrhenius equation,the pre-exponential factor represents ...

The Arrhenius equation expressing the effect of temperature on the rate constant of a reaction is

The rate coefficient $(k)$ for a particular reaction is $1.3 \times 10^{-4} \ M^{-1} \ s^{-1}$ at $100 \ ^oC$ and $1.3 \times 10^{-3} \ M^{-1} \ s^{-1}$ at $150 \ ^oC$. What is the energy of activation $(E_a)$ (in $kJ \ mol^{-1}$) for this reaction? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$