A reaction has a rate constant 'k' at temperature T₁ and k' at T₂ (T₂ > T₁). If the activation energy is Ea, which expression correctly relates k, k', T₁, and T₂ according to the Arrhenius equation?

The rate of the elementary reaction, $2{\rm{NO}} + {{\rm{O}}_2} o 2{\rm{N}}{{\rm{O}}_2},$ when the volume of the reaction vessel is doubled:

For a gaseous reaction, the units of rate of rate of reaction are

The rate of a chemical reaction doubles for every 10\,^\circ C rise of temperature. If the temperature is raised by 50\,^\circ C, the rate of the reaction increases by about

The rate constant is given by the equation $K = A{e^{ - {E_a}/RT}}$ which factor should register a decrease for the reaction to proceed more rapidly?

The rate constant of a first order reaction is $3 imes {10^{ - 6}}$ per second and initial concentration is $0.10\;{\rm{ }}M.$ Then the initial rate of reaction is

The rate of reaction becomes 2 times for every $10^\circ C$ rise in temperature. How the rate of reaction will increase when temperature is increased from $30^\circ C\;to\;80^\circ C?$

The rate constant of a reaction at $293 K$ is $k_1$. At $313 K$, the rate constant becomes $2k_1$. Calculate the activation energy ($E_a$) for the reaction. (Given: $R = 8.314 \, J K^{-1} mol^{-1}$)

The rate constants ${K_1}$ and ${K_2}$ for two different reactions are ${10^{16}}{e^{ - 2000/T}}$ and ${10^{15}}{e^{ - 1000/T}}$, respectively. The temperature at which${K_1} = {K_{2\;}}$ is:

An elementary reaction is given as 2P+Q⟶ products. If concentration of Q is kept constant and concentration of P is doubled then rate of reaction is:

For the reaction $A + B o C$ it is found that doubling the concentration of $A$ increases the rate by four times and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?