The activation energy of an uncatalyzed reaction is 98 kJ/mol.The addition of a

Question

The activation energy of an uncatalyzed reaction is 98 kJ/mol.The addition of a catalyst lowers the activation energy to 57kJ/mol. a) assuming that the collision factor remains the same, bywhat factor will the catalyst increase the rate of the reaction at28 degrees C? b) assuming that the collision factor remains the same, bywhat factor will the catalyst increase the rate of the reaction at138 degrees C? The activation energy of an uncatalyzed reaction is 98 kJ/mol.The addition of a catalyst lowers the activation energy to 57kJ/mol. a) assuming that the collision factor remains the same, bywhat factor will the catalyst increase the rate of the reaction at28 degrees C? b) assuming that the collision factor remains the same, bywhat factor will the catalyst increase the rate of the reaction at138 degrees C?

Explanation / Answer

According to Arhhenious Equation , rate , K = Ae-Ea /RT Where A = frequancy factor Ea = Activation energy R = gas constant T = Temperature (a)For uncatalised,   K uc = A e -98000/(8.314*301)                                                      = 9.834*10^-18A For catalised K c = A e -(98000-57000)/(8.314*301)                                        = 7.668*10^-8 A Kc / Kuc = 0.7797 * 10^10 (b) simillar to (a) For catalised K c = A e -(98000-57000)/(8.314*301)                                        = 7.668*10^-8 A Kc / Kuc = 0.7797 * 10^10 (b) simillar to (a) Kc / Kuc = 0.7797 * 10^10 (b) simillar to (a)

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