Question

The activation energies of two reactions are ${E_1}\;and\;{E_2}({E_1} > {E_2})$. If the temperature of the system is increased from ${T_1}\;and\;{T_2}$, the rate constant of the reactions changes from ${k_1}\;to\;{k_2}$ in the first reaction and ${k_1}\;and\;{k_2}$ in the second reaction. Predict which of the following expression is correct?

Accepted Answer

$\frac{{{k_1}^\prime }}{{{k_1}^\prime }} > \frac{{{k_2}^\prime }}{{{k_2}^\prime }}$

Answer

$\frac{{{k_1}^\prime }}{{{k_1}^\prime }} = \frac{{{k_2}^\prime }}{{{k_2}^\prime }}\;\;$

Answer

$\frac{{{k_1}^\prime }}{{{k_1}^\prime }} < \frac{{{k_2}^\prime }}{{{k_2}^\prime }}$

Answer

$\frac{{{k_1}^\prime }}{{{k_1}^\prime }} = \frac{{{k_2}^\prime }}{{{k_2}^\prime }} = 1$

NEET UG CHEMISTRY MCQ: CHEMICAL KINETICS

More Questions from CHEMICAL KINETICS