2) The activation energy of a certain reaction is 75000 joules.When a catalyst is introduced into the system the activation energy decreases by 23000 joules.Calculate how many times the reaction rate increases after adding a catalyst . if we assume that both reactions occur at 25^circ C

Question

2) The activation energy of a certain reaction is 75000 joules.When a catalyst is introduced into the system the activation energy decreases by 23000 joules.Calculate how many times the reaction rate increases after adding a catalyst . if we assume that both reactions occur at 25^circ C

Answer 1

To calculate how many times the reaction rate increases after adding a catalyst, we can use the Arrhenius equation:k = A * e^(-Ea/RT)where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.Given that the activation energy of the reaction is 75000 joules and the activation energy decreases by 23000 joules when a catalyst is introduced, we can calculate the new activation energy:New activation energy = 75000 - 23000 = 52000 joulesNow, we can calculate the ratio of the rate constants before and after adding the catalyst:Ratio = k2 / k1 = e^(-Ea1/RT) / e^(-Ea2/RT)Since both reactions occur at the same temperature (25°C), we can simplify the equation:Ratio = e^(-(Ea1 - Ea2) / RT)Substituting the given values:Ratio = e^(-(75000 - 52000) / (8.314 * 298))Ratio ≈ e^(-0.693)Ratio ≈ 0.5Therefore, the reaction rate increases by a factor of 2 (or 2 times) after adding a catalyst.

Вопрос

2) The activation energy of a certain reaction is 75000 joules.When a catalyst is introduced into the system the activation energy decreases by 23000 joules.Calculate how many times the reaction rate increases after adding a catalyst . if we assume that both reactions occur at 25^circ C

Решения

Ответ