if it takes 80 h to completely recrystallize an aluminum sheet at 250 c and 6 h at 3000, calculate the activvation energy in cal/mol?
Arrhenius equation k = A e-Ea/RT
where k = rate of reaction
A = collision frequency
Ea = activation energy
R= universal gas constant = 1.987 cal/K/mol
T = temperature
Arrhenius equation can be written as
In (k2/k1) = Ea/R [(1/T1 - 1/T2)]
Ea = R [ln (k2/k1)] / [(1/T1) - (1/T2) ]
Given that it takes 80 h to completely recrystallize an aluminum sheet at 250oC and 6 h at 3000oC.
Hence, Initial rate of reaction = k1 = 80 h
Final rate of reaction k2 = 6 h
Initial temperature T1 = 250oC = 250 + 273 K = 523 K
Final temperature T2 = 3000oC = 3000 + 273 K = 3273 K
Substitute all these velues in eq (1),
Ea = R [ln (k2/k1)] / [(1/T1 - 1/T2)] -- Eq (1)
= (1.987 cal/K/mol) [ In (6/80)] / [(1/523) - (1/3273)]
= -0.0083 cal/mol
Ea = -0.0083 cal/mol
Therefore, activation energy of the reaction = -0.0083 cal/mol
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