Given that; The activation energy of a certain un-catalyzed reaction = 76 kJ/mol

Question

Given that;

The activation energy of a certain un-catalyzed reaction = 76 kJ/mol.

The activation energy of catalyzed reaction = 52 kJ/mol.

Temperature 20 C or 293.15 K

Reaction rate is proportional to the exp(-Ea/RT), where Ea- activation energy in Joules, R-gas constant and T -temperature in K.

So, the ration of rate constants of catalyzed and not catalyzed reactions will be equal to exp(-Ea1/RT) / exp(-Ea2/RT) = exp((Ea2-Ea1)/RT), where Ea1 - activation energy of catalyzed reaction and Ea1 - activation energy of not catalyzed reaction.

ratio = exp((76000-52000)/8.314/293.15)

= exp(9.85)

=1.8*10^4

Explanation / Answer

Part Il: Free Response. Show your work clearly on mathematical problems. toothpaste" demonstration conducted in class involves the catalyzed decomposition of hydrogen peroxide according to the chemical equation below. At 20.0 °C the uncatalyzed reaction has an Ea :76k /mol. when the reaction is catalyzed by 1- asnthe demonstration,52k mol at the same temperature. How many times faster is the catalyzed reaction compared to the uncatalyzed reaction, assuming that the frequency factor does not change? pts)

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