Ans ; we are going to calculate the activation energy for giving first temperatu

Question

Ans ; we are going to calculate the activation energy for giving first temperature and rate cofficient in arrhenius equation T = 117 degree C = 273.15+117=390.15k , k = 5.1*109   By the formula of arrhenius equation k = Ae-Ea/RT    e-Ea/0.0083kj/mol K*390.15K = 5.1*109   1/eEa/3.238kj/mol = 5.1*109 eEa/3.238kj/mol = 1/5.1*109 = 0.19*10-9 Ea/3.238 = log(0.19*10-9) = -0.72-9 = -9.72 Ea = -9.72*3.238 = -31.47kj/mol because energy is not in a negative so the activation energy Ea   = 31.47kj/mol By the second temperature and rate cofficient's value T = 273.15+57 = 330.15 k , k = 2.6*108 by the formula 1/eEa/0.0083kj/mol K*330.15K   =     2.6*108 eEa/2.74kj/mol = 1/2.6*108 = 0.38*10-8 Ea/2.74kj/mol = log(0.38*10-8) = log(0.38) + (-8log10) = -0.42-8 =-8.42 Ea = -8.42*2.74 = -23.07 kj/mol Thus , Ea = 23.07 kj/mol

Explanation / Answer

O KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate Ea from k versus T data The rate constant k for a certain reaction is measured at two different temperatures temperaturek 1170 .c 5.1x 10 570 c 2.6 x 108 12.6× Assuming the rate constant obeys the Arhenius equation, calculate the activation energy Ea for this reaction. Round your answer to 2 significant digits. kJ mol

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