The number of correct statement/s from the following is _____ .
A.Larger the activation energy, smaller is the value of the rate constant.
B. The higher is the activation energy, higher is the value of the temperature coefficient.
C. At lower temperatures, increase in temperature causes more change in the value of $k$ than at higher temperature.
D. A plot of $\ln k$ vs $\frac{1}{T}$ is a straight line with slope equal to $- \frac{Ea}{R}$

Question

The number of correct statement/s from the following is _____ .

A.Larger the activation energy, smaller is the value of the rate constant.

B. The higher is the activation energy, higher is the value of the temperature coefficient.

C. At lower temperatures, increase in temperature causes more change in the value of $k$ than at higher temperature.

D. A plot of $\ln k$ vs $\frac{1}{T}$ is a straight line with slope equal to $- \frac{Ea}{R}$

Aicharya · Accepted Answer

A : k = Ae - Ea RT (Arrhenius rate equation) As Ea (Activation energy) increases k (rate constant) decreases B :Higher activation energy, greater is the effect of given temperature rise on rate constant 'k'. Activation energy is the minimum energy needed for the reaction to occur. When temperature increases, Kinetic Energy also increases; as temperature increases, more molecules have higher Kinetic Energy, and thus the fraction of molecules that have high enough Kinetic Energy to overcome the energy barrier also increases. Temperature coefficient = k T + 10 k T Option (C) is wrong. &#916;k may be greater or lesser depending on temperature. D : &#160; lnk = lnA - Ea RT in this equation the slope is - E a R .

The number of correct statement/s from the following is _____ . A.Larger the activation energy, smaller is…

Solution