Question

For a reaction rate constant (k) is given by
\[ k = A e^{\frac{-E_a}{RT}} \] Calculate activation energy (E\(_a\))

• A. 23.28 KJ/mol
• B. 56 KJ/mol
• C. 232.8 KJ/mol
• D. 5600 KJ/mol

Hint:

The Arrhenius equation provides a relationship between the rate constant and temperature, which allows the calculation of activation energy by measuring the rate constants at different temperatures.

Answer 1

The Correct Option is A

Step 1: Given relation for \( E_a \).
We are given the relation:
\[ \frac{E_a}{R} = 2800 \]
Step 2: Solving for \( E_a \).
By rearranging the equation, we get:
\[ E_a = 2800 \times R \]
Step 3: Substituting the value of \( R \).
Substitute the value of \( R = 8.314 \, \text{J/mol·K} \) into the equation:
\[ E_a = \frac{2800 \times 8.314}{1000} \, \text{KJ/mol} \]
Step 4: Calculating the final result.
Now, calculating the value:
\[ E_a = 23.28 \, \text{KJ/mol} \] Final Answer: \( E_a = 23.28 \, \text{KJ/mol} \)