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The activation energy of a certain uncatalysed reaction at 300K is 76 kJ/mol.The activation energy is lowered by 19 kJ/mol by the use of catalyst. By what factor, the rate of catalysed reaction is lowered?
K = Ae-E/RT (E is activation energy) rate(R)= K(a)n (k=rate constant & a is concentration , n is order of reaction) rate directily proportional to rate constant so R1/R2 = K1/K2 = e[-E1+E2]/RT =e[-76+19]/RT R1/R2 = e-2.28 (e = 2.8 approx) R2 = 8R1
K = Ae-E/RT (E is activation energy)
rate(R)= K(a)n (k=rate constant & a is concentration , n is order of reaction)
rate directily proportional to rate constant so
R1/R2 = K1/K2 = e[-E1+E2]/RT
=e[-76+19]/RT
R1/R2 = e-2.28 (e = 2.8 approx)
R2 = 8R1
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