As the reaction progresses, the rate of reaction

The rate constant of a reaction increases by 5% when its temperature is raised from $27^\circ C\;{\rm{to}}\;28^\circ C$. The activation energy of the 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 $30^\circ C\;to\;80^\circ C?$

For the reaction, $2N{H_3}(g) o {N_2}(g) + 3{H_2}(g) - \frac{{d\left[ {N{H_3}} \right]}}{{dt}} = {K_1}\left[ {N{H_3}} \right]$; $\frac{{ + d\left[ {{N_2}} \right]}}{{dt}} = {K_2}\left[ {N{H_3}} \right];\frac{{ + d\left[ {{H_2}} \right]}}{{dt}} = {K_3}\left[ {N{H_3}} \right];$ the relation between ${K_1},{K_2}$ and ${K_3}$ is

For a reaction, the rate of reaction was found to increase about 1.8 times when the temperature was increased by $10^\circ C$. The increase in rate is due to:

The activation energy of a chemical reaction can be determined if one knows the value of:

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 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?

The temperature coefficient of most of the reactions lies between

According to Arrhenius equation, the rate constant $\left( k \right)$ is related to temperature $\left( T \right)$ as

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?