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A reaction takes place in three steps wi...

A reaction takes place in three steps with individual rate constant and activation energy Ea1 = 180 KJ/mol Ea2 = 80 KJ/mol Ea3 = 50 KJ/mol
overall rate constant `k=((k_(1)k_(2))/(k_(3)))^(2//3)`
overall activation energy of the reaction will be

A

140 kJ/mol

B

150 kJ/mol

C

130 kJ/mol

D

120 kJ/mol

Text Solution

Verified by Experts

`Ae^(-E_(a)//RT) = [(Ae^(-E_(a1)//RT) xx Ae^(-E_(a2)//RT))/(Ae^(-E_(a3)//RT))]^(2//3) = [Ae^((-E_(a1) - E_(a2) + E_(a3))//RT)]^(2//3)`
`E_(a) = (2)/(3)[E_(a1) + E_(a2) - E_(a3)] = (2)/(3)[180 + 80 - 50] = 140 kJ//mol`
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