Question:
A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be \( k_1 \) and \( k_2 \) respectively. Then
A chemical reaction was carried out at 300 K and 280 K. The rate constants were found to be \( k_1 \) and \( k_2 \) respectively. Then
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The rate constant doubles for every 10°C rise in temperature according to the Arrhenius equation.
Updated On: Jan 6, 2026
- \( k_2 = 4k_1 \)
- \( k_2 = 2k_1 \)
- \( k_2 = 0.5k_1 \)
- \( k_2 = 0.25k_1 \)
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The Correct Option is C
Solution and Explanation
Step 1: Use the temperature dependence of rate constants.
The rate constant increases with temperature, and the rate constant ratio is related to the activation energy.
Step 2: Conclusion.
Thus, the rate constant at 280 K is half that at 300 K.
Final Answer: \[ \boxed{C} \]
The rate constant increases with temperature, and the rate constant ratio is related to the activation energy.
Step 2: Conclusion.
Thus, the rate constant at 280 K is half that at 300 K.
Final Answer: \[ \boxed{C} \]
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