Question

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

• A. \( \frac{k_2}{k_1} = e^{\frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right)} \)
• B. \( \frac{k_2}{k_1} = e^{\frac{E_a}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)} \)
• C. \( \ln \frac{k_2}{k_1} = \frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right) \)
• D. \( \frac{k_2}{k_1} = \frac{E_a}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right) \)

Hint:

Arrhenius equation relates the rate constant to temperature and activation energy.

Answer 1

The Correct Option is A

Step 1: Arrhenius equation.
The Arrhenius equation shows the dependence of the rate constant on temperature and activation energy. The correct form is: \[ \frac{k_2}{k_1} = e^{\frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right)} \] which is option (A).

Step 2: Conclusion.
Thus, the correct answer is option (A).

Final Answer: \[ \boxed{\text{(A) } \frac{k_2}{k_1} = e^{\frac{E_a}{R} \left( \frac{1}{T_1} - \frac{1}{T_2} \right)}} \]