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The activation energy of an uncatalyzed reaction is 95
Chapter , Problem 14.87(choose chapter or problem)
The activation energy of an uncatalyzed reaction is 95 kJ>mol. The addition of a catalyst lowers the activation energy to 55 kJ>mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25 C, (b) 125 C?
Questions & Answers
QUESTION:
The activation energy of an uncatalyzed reaction is 95 kJ>mol. The addition of a catalyst lowers the activation energy to 55 kJ>mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25 C, (b) 125 C?
ANSWER:Problem 14.87The activation energy of an uncatalyzed reaction is 95 kJ/mol. The addition of a catalyst lowersthe activation energy to 55 kJ/mol. Assuming that the collision factor remains the same, by whatfactor will the catalyst increase the rate of the reaction at (a) 25°C, (b) 1 C Step-by-step solution Step 1 of 5 ^(a)The relationship between the rate constant and activation energy of the reaction is as follows:The arrhenius equation is,k = Ae E aRTHere, k is the rate constant, A is the collision factoraE is the activation energy, T is temperatureand R is gas constant.Now, write the rate constant expression for uncatalyzed reaction and catalyzed reaction asfollows: E a1/RTk 1 = Aek = Ae E a2/RT 2Here, k1and 2 are the rate constant for uncatalyzed reaction and catalyzed reactionrespectively.