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The rate constant of a reaction is 1.5×10⁻³ at 25°C and 2.1×10⁻² at 60°C. The activation energy is:
The rate constant of a reaction is 1.5×10⁻³ at 25°C and 2.1×10⁻² at 60°C. The activation energy is:
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Use absolute temperatures while applying Arrhenius equation.
Updated On: Mar 23, 2026
- \( \dfrac{35}{333}R\log_e\!\left(\dfrac{2.1\times10^{-2}}{1.5\times10^{-2}}\right) \)
- \( \dfrac{298\times333}{35}R\log_e\!\left(\dfrac{21}{1.5}\right) \)
- \( \dfrac{298\times333}{35}R\log_e(2.1) \)
- (298)/(35)Rlogₑ((1.5)/(2.1))
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The Correct Option is B
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