Assuming the energy of activation for most of the reactions is 52 kJ, what conclusions you draw about the effect of temperature on the rate of a reaction?

Explanation

To analyze the effect of temperature on the rate of a reaction given an activation energy of 52 kJ, we can use the Arrhenius equation. Here’s a step-by-step solution:

### Step 1: Understand the Arrhenius Equation
The Arrhenius equation is given by:
\[ k = A e^{-\frac{E_a}{RT}} \]
where:
- \( k \) = rate constant
- \( A \) = pre-exponential factor (frequency factor)
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