Question:
The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy of the reaction?
The rate constant of a reaction at temperature 200 K is 10 times less than the rate constant at 400 K. What is the activation energy of the reaction?
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Activation energy can be determined using the Arrhenius equation when rate constants at two different temperatures are known.
Updated On: Jan 6, 2026
- 1842.4 R
- 460.6 R
- 203 k
- 921.2 R
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The Correct Option is B
Solution and Explanation
Step 1: Use the Arrhenius equation.
Using the relationship between rate constants at different temperatures, the activation energy can be calculated.
Step 2: Conclusion.
Thus, the activation energy of the reaction is \( 460.6 R \).
Final Answer: \[ \boxed{460.6 R} \]
Using the relationship between rate constants at different temperatures, the activation energy can be calculated.
Step 2: Conclusion.
Thus, the activation energy of the reaction is \( 460.6 R \).
Final Answer: \[ \boxed{460.6 R} \]
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