For a reaction with the rate law: Rate = k[A]^[1/2][B], if the concentration of B is doubled while keeping [A] constant, how does the half-life change?

Unit of frequency factor $\left( A \right)$ is

The rate constant of a reaction at temperature $200\;K$ is 10 times less than the rate constant at $400\;K$. What is the activation energy (${E_a}$ ) of the reaction?

The hydrolysis of ethyl acetate was carried out separately with $0.05\;{\rm{M }}\;{\rm{HCl }}\;{\rm{and}}\;0.05\;{\rm{M}}\;{{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}{\rm{.}}$ The rate constants were found to be ${k_1}\;{\rm{and}}\;{k_2}$ respectively then

Which statement is false regarding the plot of $\ln k$ versus $\frac{1}{T}$ according to the Arrhenius equation?

For the reaction ${N_2}{O_5}(g) o 2N{O_2}(g)\; + \;\frac{1}{2}{O_2}(g),$ the rate of disappearance of ${N_2}{O_5}$ is $6.25 imes {10^{ - 3}}\;{\rm{mol}}\;{{\rm{L}}^{ - 1}}\;{{\rm{s}}^{ - 1}}.$ The rate of formation of $N{O_2}$ and ${O_2}$ will be respectively.

For the two gaseous reactions, following data are given,

$A o B;\;{k_1} = {10^{10}}\;{e^{ - 20,000/T}}$

$C o D;\;{k_2} = {10^{12}}\;{e^{ - 24,606/T}}$

The temperature at which ${k_1}$ becomes equal to ${k_2}$ is

For the non-equilibrium process, $A + B o products$, the rate is first order with respect to $A$ and second order respect to $B$. If $1.0\;mole$ each of $A$ and $B$ are introduced into a 1 litre vessel and the initial rate was $1.0 imes {10^{ - 2}}\;{\rm{mol}}/{\rm{litre}}\;\;{\rm{sec}}{\rm{.}}$ The rate (in ${\rm{mol}}\;{\rm{litr}}{{\rm{e}}^{ - 1}}{\sec ^{ - 1}}$ ) when half of the reactants have been used:

If a plot of $\ln k$ versus $\frac{1}{T}$ for a reaction yields a straight line with a slope of -5000 K, what is the activation energy ($E_a$) of the reaction? (R = 8.314 J/mol·K)

For a given reaction, pressure of catalyst reduces the energy of activation by $2\;{\rm{k}}\;{\rm{cal }}\;{\rm{at}}\;27^\circ C.$ The rate of reaction will be increased by:

The rate constant for a first order reaction is $4.606\,\, imes \,\,{10^{ - 3}}\,{{\rm{s}}^{ - 1}}$. The time required to reduce ${\rm{2}}{\rm{.0}}\,\,{\rm{g}}$ of the reactant to ${\rm{0}}{\rm{.2}}\,\,{\rm{g}}$ is: