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Grade: 12th pass
        he activation energy of a certain reaction at 300 k is 76 kj/mol . the activation energy id lowered by19 kj/mol by the ude of catalyst .by what factor the rate of reaction is incresed?
2 years ago

Answers : (1)

Gopal
54 Points
							
 activation energy of catylised reaction is = 76-19=57kJ/mol
Acoording to Arrhenius equation , Rate constatnts or rate of reaction are related as
For uncatalysed reaction
logk1= logA-\frac{Ea1}{2.303RT}
for catalysed reaction
logk1= logA-\frac{Ea2}{2.303RT}
 
log \frac{k2}{k1} =\frac{19}{2.303*8.314*10^{-3}*300}
 
log \frac{k2}{k1} =3.308
taking antilog k2 = 2.032 X 10^{3} K1
 
2 years ago
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