The reaction has the following Arrhenius coefficient (A), andactivation energy (

Question

The reaction has the following Arrhenius coefficient (A), andactivation energy (Ea) at the temperature 25°C.Determine the rate constant.

Arrhenius coefficient = 99489136 s-1
Activation energy = 58 kJ mol-1
Temperature = 25°C

B2O3 + 3Mg arrow 2B +3MgO The above reaction is found experimentally to obey the rate law. Rate = k[B2O3]^0[Mg]^1 The reaction has the following Arrhenius coefficient (A), andactivation energy (Ea) at the temperature 25degreeC.Determine the rate constant. Arrhenius coefficient = 99489136 s^-1 Activation energy = 58 kJ mol^-1 Temperature = 25degreeC

Explanation / Answer

Formula :                   k = A e-Ea /RT Where k is the first order rate constant            Ais the Arrhenius factor           Ea is the activation energy            Tis the temperature            Ris constant Data :             A = 99489136 s-1
            Ea = 58 * 1000 J / mol             T = 273 + 25 K                 = 298 K             R = 8.314 J / mol .K           lnk = - 58 * 1000 J /mol. / 8.314 J /mol.K * 298 K + ln(99489136 s-1)                  =-23.40 + 18.41                 = -4.99             k = 0.0068s-1            

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