Temperature Dependence of Reaction Rates (Arrhenius Equation)

If the definition of the temperature coefficient of the reaction holds good for a reaction between $27°\mathrm{C}$ and $37°\mathrm{C}$, the activation energy for the reaction in $\mathrm{kJ}.{\mathrm{mol}}^{-1}$ is

What is the increase in rate of the reaction, on raising the temperature by $25°\mathrm{C}$ if the temperature coefficient of a reaction is $3$?

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 rate of a reaction is doubled for every $10^{\mathrm{o}}\mathrm{C}$ rise in temperature. The increase in reaction rate as a result of temperature rise from $10^{\mathrm{o}}\mathrm{C}$ to $100^{\mathrm{o}}\mathrm{C}$ is

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.

Two first order reactions proceed at $\text{25 °C}$ temperature at the same rate. Temperature coefficient of the first reaction is $\text{2}$ and that of second reaction is $\text{3}$. Find the ratio of the rate of these reaction at ${\text{75}}^{\text{o}}\text{C}$.

At a given temperature, the energy of activation of two reactions is same if :

The rate constant of a first order reaction is ${10}^{–3}$ ${\mathrm{m}\mathrm{i}\mathrm{n}}^{-1}\mathrm{ }\mathrm{a}\mathrm{t}\mathrm{ }300\mathrm{ }\mathrm{K}.$ The temperature coefficient of the reaction is 2. What is the rate constant of the reaction at 350 K approximately?

If the rate of reaction grows 15.6 times on increasing the temperature by 30 K, the temperature coefficient of the reaction will be approximately:

The temperature coefficient of a reaction is:

The rate constant of a first order reaction is ${10}^{-3}{\min }^{-1}$ at $300\mathrm{ }\mathrm{K}$. The temperature coefficient of the reaction is $2$. What is the rate constant of the reaction at $350\mathrm{ }\mathrm{K}$ approximately?

By what factor does the rate of reaction increases when the temperature is increased from $30°\mathrm{C}$ to $60°\mathrm{C}$?

The rate of a chemical reaction doubled for every $10\mathrm{℃}$ rise in temperature. If the temperature is increased by $60\mathrm{℃}$ the rate of reaction increase by

The temperature coefficient of most of the reactions lies between which of the following ranges?

Find out the temperature coefficient of most of the reactions lies between:

Temperature coefficient of a reaction is 2. When temperature is increased from $30℃$ to $100℃$, rate of the reaction increases by

The rate constant of a first order reaction at $27℃$ is ${10}^{-3} \mathrm{m}\mathrm{i}{\mathrm{n}}^{-1}$. The temperature coefficient of this reaction is 2. What is the rate constant (in $\mathrm{m}\mathrm{i}{\mathrm{n}}^{-1}$) at $17℃$ for this reaction?

The activation energy for most of the reactions is approximately $50 \mathrm{kJ} \mathrm{m}\mathrm{o}{\mathrm{l}}^{-1}$. The value of temperature coefficient for such reactions is:

The velocity constant of a reaction at $290 \mathrm{K}$ was found to be $3.2\times {10}^{-3}$at $300 \mathrm{K}$, it will be:

In a zero-order reaction for every 10^oC rise of temperature the rate is doubled. If the temperature is increased from 10^o C to 100^o C, the rate of the reaction will become: