The rate of a reaction triple when temperature changes from 20°C to 50°C. Calculate energy of activation for the reaction. (R=8.314 JK−1mol−1)

The Arrhenius equation is,log10k2k1=EaR×2.303T2−T1T1T2 Given: k2k1=3;R=8.314JK-1 mol-1;T1=20+273=293 Kand T2=50+273=323 KSubstituting the given values in the Arrhenius equation,log103=Ea8.314×2.303323−293323×293Ea=2.303×8.314×323×293×0.47730=28811.8 J mol−1Ea=28.81 kJ mol−1