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

What is the activation energy for a reaction if its rate doubles when the temperature is raised from $20 \,^{\circ}C$ to $35 \,^{\circ}C$ in $kJ \,mol^{-1}$? $(R = 8.314 \,J \,mol^{-1} \,K^{-1})$

Find True $(T)$ and False $(F)$ statements in the following:
$1.$ Effective collision depends on rate.
$2.$ When the reactant converts into product,the bonds in the reactant break and new bonds form.
$3.$ The breaking of old bonds and the formation of new bonds take place simultaneously.

An exothermic reaction $X \rightarrow Y$ has an activation energy of $30 \ kJ \ mol^{-1}$. If the energy change $\Delta E$ during the reaction is $-20 \ kJ \ mol^{-1}$,then the activation energy for the reverse reaction in $kJ \ mol^{-1}$ is $...$.

The velocity constant of a reaction at $290 \ K$ was found to be $3.2 \times 10^{-3}$. At $300 \ K$ it will be

$A$ reaction rate constant is given by $k = 1.2 \times 10^{14} \, e^{-25000/RT} \, sec^{-1}$. It means