A plot of ln(k) versus 1/T for a chemical reaction yields a straight line. The slope of this line is related to:

For the reaction, $2A + B o products$, the active mass of B is kept constant, and that of A is doubled. The rate of reaction will be then

The rate of a reaction triples when the temperature changes from $25^\circ C$ to $45^\circ C$. Calculate the energy of activation. Given: $[R] = 8.314\, J K^{-1} mol^{-1}$, $\log 3 = 0.4771$

Arrhenius equation may not be represented as

For the reaction system

$2{\rm{NO}}\left( {\rm{g}} \right) + {{\rm{O}}_2}\left( {\rm{g}} \right) o 2{\rm{N}}{{\rm{O}}_2}\left( {\rm{g}} \right)$ if the volume of the reaction vessel is reduced to one-third of its original volume, what will be the order of the reaction?

In Arrhenius equation $K = A\;{e^{ - {E_a}/RT}}$, the quantity $- {E_a}/RT$ is referred as:

In a gaseous phase reaction:

${{\rm{A}}_2}\left( {\rm{g}} \right) o {\rm{B}}\left( {\rm{g}} \right) + \left( {1/2} \right){\rm{C}}\left( {\rm{g}} \right),$ the increase in pressure from $100{\rm{ }}\;mm{\rm{ }}\;to\;{\rm{ }}120{\rm{ }}\;mm$ is noticed in 5 minute. The rate of disappearance of ${A_2}\;in\;mm\;{\min ^{ - 1}}$ is:

For a reaction $\frac{1}{2}A o 2B$, rate of disappearance of ‘A’ is related to the rate of appearance of B by the expression

The half-life of a first-order reaction is 200 seconds. If the initial concentration of the reactant is $0.4 \, M$, what will be the concentration after 600 seconds?

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?

For a reaction A + B → C, the rate law is found to be Rate = k[A]²[B]⁻¹. If the concentration of A is tripled while keeping the concentration of B constant, the factor by which the reaction rate changes is: