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Anonymous asked in Science & MathematicsChemistry · 2 months ago

Activation Energy question?

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  • 2 months ago
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    Arrhenius equation: ln(k₁/k₂) = (Eₐ/R) [(1/T₂) - (1/T₁)]

    Hence, Eₐ = R ln(k₁/k₂) / [(1/T₂) - (1/T₁)]

    Activation energy, Eₐ

    = 8.314 × ln[(3.12 × 10³)/(2.70 × 10⁴) / [(1/300) - (1/275)] J/mol

    = 59200 J/mol

    = 59.2 kJ/mol

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