The Effect of Temperature on the Rate Constant

The factors which influence the rate of reaction are :

Concentration: Greater the concentrations of the reactants, faster is the rate of reaction.

Temperature: The rate of reaction increases with increase in temperature. For most of the reactions, the rate of reaction becomes almost double with 10o rise in temperature.

Presence of catalyst: A catalyst generally increases the speed of a reaction.

Answer the following question :

A small increase in temperature of the reacting system, the rate of reaction exceed to large extend. The most appropriate reason for this is-

Plot the graph of kinetic energy versus fraction of molecules for a reaction at different temperature.

Define frequency factor.

The temperature coefficient of the rate of a reaction is $2.3$. How many times will the rate of the reaction increase if the temperature is raised by $25\mathrm{K}?$ Give answer to the nearest integer.

The activation energy for a reaction at the temperature $\mathrm{T} \mathrm{K}$ was found to be $2.303\mathrm{RT} \mathrm{J} {\mathrm{mol}}^{-1}$. The ratio of the rate constant to Arrhenius factor is

Activation energy of a chemical reaction can be determined by ______.

A small increase in temperature of the reacting system, the rate of reaction exceed to large extend. The most appropriate reason for this is-

Explain, with the help of potential energy barrier, how does increase in temperature increases the rate of a reaction.

For the given chemical reactions,

$\text{A}\to \text{B}; {\text{k}}_1=10^{10}{\text{e}}^{-20\text{,}000/\text{T}}$

$\text{C}\to \text{D}; {\text{k}}_2=10^{12}{\text{e}}^{-24\text{,}606/\text{T}}$

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

For a reaction, if the temperature is increased by 10^oC, how much faster will the equilibrium be attained?

At what conditions exponential factor is zero for a reaction

(i) At infinite temperature

(ii) For free radical combination

(iii) When energy of activation$=$Threshold energy

Which of the following statement is/are correct ?

Which of the following parameters is/are temperature independent ?

In the start of summer, a given sample of milk turns sour at room temperature $\left({27}^{o}C\right)$ in  $48 hour$. In a refrigerator at $2^{o}C$, milk can be stored three times before it sours.

For souring of milk, At $2^{o}C$, the reaction is three times slower than at ${27}^{o}C$. The activation energy of the souring of milk is $\left(\mathrm{in} \mathrm{kJ} {\mathrm{mol}}^{-1}\right)$.

For a reaction ${\mathrm{E}}_{\mathrm{a}}=0$ and $\mathrm{k}=3.2\times {10}^8{\mathrm{s}}^{-1}$ at $325 \mathrm{K}$. The value of $\mathrm{k}$ at $335 \mathrm{K}$ would be:

For the reaction:

$\left[\mathrm{Cr}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{3+}+\left[{\mathrm{SCN}}^{\mathrm{\Theta }}\right]\to \left[\mathrm{Cr}\right({\mathrm{H}}_2\mathrm{O}{)}_5\mathrm{NCS}{]}^{+2}+{\mathrm{H}}_2\mathrm{O}$

The rate law, $\mathrm{r}=\mathrm{k} \left[\mathrm{Cr}\right({\mathrm{H}}_2\mathrm{O}{)}_6{]}^{3+}] \left[{\mathrm{SCN}}^{\mathrm{\Theta }}\right].$

The value of k is $2.0\times {10}^{-6}\mathrm{L}{\mathrm{mol}}^{-1}{\mathrm{s}}^{-1}\mathrm{at}{14}^{\mathrm{o}}\mathrm{C}$and $2.2\times {10}^{-5}\mathrm{L}{\mathrm{mol}}^{-1}{\mathrm{s}}^{-1}\mathrm{at} {30}^{\mathrm{o}}\mathrm{C}$.

What is the value of ${\mathrm{E}}_{\mathrm{a}}$?

Consider two reactions having same Arrhenius factor A, but different energies of activation.
(i) $\mathrm{A}\to \mathrm{B}; \mathrm{E}{\mathrm{a}}_1=\mathrm{20 }\mathrm{kJ}$
(ii) $\mathrm{C}\to \mathrm{D}; \mathrm{E}{\mathrm{a}}_2=\mathrm{30 }\mathrm{kJ}$
Both are at temperature $25°\mathrm{C}$
If temperature in both reaction is increased slightly in such a way that change in temperature in both case is same then, choose the correct option.

The decomposition of ethane into ethene and hydrogen involves 5 different steps, having rate constants K₁, K₂, K₃, K₄ and K₅. The rate law is given by:
$\frac{-d\left[C_2{H}_6\right]}{dt}={\left(\frac{K_1{K}_3{K}_4}{K_5}\right)}^{1/2}\left[C_2{H}_6\right]$
If $E_{a_1}$ (10 kJ/mol), $E_{a_3}$ (5 kJ/mol), $E_{a_4}$ (3 kJ/mol) and $E_{a_5}$ (0) are the energies of activation associated with 1^st, 3^rd, 4^th and 5^th steps respectively, find the overall energy of activation in kJ/mol for ethane decomposition.

The first order gaseous decomposition of ${\mathrm{N}}_2{\mathrm{O}}_4 \mathrm{into} {\mathrm{NO}}_2$ has a rate constant value $\mathrm{K} = 4.5 \times {10}^3 {\mathrm{s}}^{–1}$ at $1°\mathrm{C}$and energy of activation $58 \mathrm{kJ} {\mathrm{mol}}^{-1}$. What should be the rise in temperature in $(°\mathrm{C})$ to get the value of $\mathrm{K} = 1.00 \times {10}^4 {\mathrm{s}}^{-1}. (\log 2.2 = 0.3424)$