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Energy of activation of a reactant is re...

Energy of activation of a reactant is reduced by:

A

Increased temperature

B

Reduced temperature

C

Reduced pressure

D

Increased pressure

Text Solution

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The correct Answer is:
To solve the question regarding how the energy of activation of a reactant can be reduced, we will follow these steps: ### 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 - \( E_a \) = activation energy - \( R \) = gas constant - \( T \) = temperature (in Kelvin) ### Step 2: Identify the Role of Activation Energy The activation energy \( E_a \) is the minimum energy required for a reaction to occur. A lower \( E_a \) means that the reaction can proceed more easily and quickly. ### Step 3: Analyze the Effect of Temperature From the Arrhenius equation, we see that \( E_a \) is in the exponent. If we want to reduce the effect of \( E_a \) on the rate constant \( k \), we can manipulate the temperature \( T \): - Increasing the temperature \( T \) will decrease the fraction \( \frac{E_a}{RT} \), which in turn increases \( k \). ### Step 4: Conclusion To reduce the activation energy in practical terms, we can increase the temperature. This effectively lowers the impact of the activation energy on the reaction rate, allowing the reaction to proceed faster. ### Final Answer The energy of activation of a reactant is reduced by **increasing the temperature**. ---
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