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:

Which statement is correct?

The reaction $2S{O_2}\left( g \right) + {O_2}\left( g \right)\;\leftrightharpoons\;2S{O_3}\left( g \right)$ is carried out in a $1\;d{m^3}$ vessel and $2\;d{m^3}$ vessel separately. The ratio of the reaction velocities will be

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

According to the Arrhenius equation a straight line is to be obtained by plotting the logarithm of the rate constant of a chemical reaction $\left( {\log k} \right)$ against

The rate constant is numerically the same for three reactions of first, second and third order respectively. Which one is true for rate of three reaction?

For a first-order reaction with a rate constant of $2.303 imes 10^{-2} \, min^{-1}$, what percentage of the reactant will remain after 60 minutes?

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 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 a hypothetical reaction

$A + 2B o 3C + D$

$d\left[ C \right]/dt$ is equal to

The branch of chemistry which deals with the reaction rates and reaction mechanism is called: