The rate constant for a first order reaction at 25°C is 0.24 s⁻¹. If the energy of activation of the reaction is 88 kJ mol⁻¹, at what temperature would this reaction have rate constant of 4 x 10⁻² s⁻¹.
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Explanation:
log k2/k1 = ea/ 2.303 R ( T2 -T1)
log 4/24 = 88 x 10-3 / 2.303 x 8.314 ( t / 298 - 1/t2 )
T2 = 293.7k
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