The reason for almost doubling the rate of reaction on increasing the temperature of the reaction system by $10^\circ C$ is

The rate of the reaction

${\rm{CC}}{{\rm{l}}_3}{\rm{CHO}} + {\rm{NO}} o {\rm{CHC}}{{\rm{l}}_3} + {\rm{NO}} + {\rm{CO}}$ is equal to rate $k\left[ {{\rm{CC}}{{\rm{l}}_3}{\rm{CHO}}} \right]\left[ {{\rm{NO}}} \right]$.

If concentration is expressed in mol/L. The unit of k is

The units of rate of reaction are

For the reaction $2{N_2}O5 o 4N{O_2} + {O_2}$ rate and rate constant are $1.02 imes {10^{ - 4}}\,\,mol.{L^{ - 1}}.{\sec ^{ - 1}}$ and $3.4 imes {10^{ - 5}}{\sec ^{ - 1}}$ respectively then concentration of ${N_2}{O_5}$ at that time will be

At a certain temperature, the equilibrium constant $K_c$ for the synthesis of ammonia is 4. If the equilibrium concentrations of $N_2$ and $H_2$ are 1 M and 3 M respectively, what is the equilibrium concentration of $NH_3$?

Effect of temperature on reaction rate is given by

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

For the reaction,

$2{N_2}{O_5}\left( g \right) o 4N{O_2}\left( g \right) + {O_2}\left( g \right)$

If the concentration of $N{O_2}$ increase by $5.2 imes {10^{ - 3}}\;M$ in 100 s then the rate of the reactions

The unit and value of rate constant and that of rate of reaction are same for

The activation energy of a reaction is zero. The rate constant for the reaction

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