Ea = 2.303xRx{T1xT2/(T2-T1)}x log k2/k1
Where Ea = Energy of activation = 25.24 kJ/mol
= 25240 J/mol
R = molar gas constant = 8.314J/degree/mole
T1 = 361 K, k1 = rate constant at T1
T2 = ? , k2 = rate constant at T2 = 3.50 k1,
Substituting all these values in the equation
Ea = 2.303xRx{T1xT2/(T2-T1)}x log k2/k1
25240 = 2.303 * 8.314J/degree/mole * { 361 * T2/(T2-361 )}* log 3.50
1318.2 = { 361 * T2/(T2-361 )}* 0.544
2423.18 = 361 * T2/(T2-361
2423.18 T2 - 872346.4 = 361 * T2
872346.4 =2062.18 T2
T2 = 424.2 K
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