Catalyst A reduces the activation energy for a reaction by 10 kJ mol–1 at 300 K.
The ratio of rate constants,
\(\frac{Κ′ , Catalysed}{Κ,Uncatalysed}\)
is ex. The value of x is ____.[nearest integer]
[Assume that the pre-exponential factor is same in both the cases Given R = 8.31 J K–1 mol–1]
Catalyst A reduces the activation energy for a reaction by 10 kJ mol–1 at 300 K.
The ratio of rate constants,
\(\frac{Κ′ , Catalysed}{Κ,Uncatalysed}\)
is ex. The value of x is ____.[nearest integer]
[Assume that the pre-exponential factor is same in both the cases Given R = 8.31 J K–1 mol–1]
Correct Answer: 4
Solution and Explanation
The correct answer is 4
\(In \frac{Κ′}{Κ} = \frac{E_a - E′_a}{RT} \)
\(= \frac{10 × 10³}{8.314 × 300}\)
In \(\frac{Κ′}{Κ}\) \(= \frac{100}{8.314 × 3}\)
\(\frac{Κ′}{Κ} = e^4\)
Therefore , x = 4
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Concepts Used:
Catalysis
All reactants need to overcome certain energy, better known as activation energy in order to form products. This activation energy is the difference between the energy of the transition state and the reactant species.
Types of Catalysis:
Catalysis of chemical reactions is generally divided into two categories:
- Homogeneous Catalysis: Homogeneous catalysis of chemical reactions is a process where the reactants involved in the reaction and the catalyst are in the same phase. For example hydrolysis of sugar in the presence of sulphuric acid.
- Heterogeneous Catalysis: Heterogeneous catalysis of chemical reactions is a process where the reactants involved in the reaction and the catalyst are in different phases. For example reaction of hydrogen and nitrogen in the presence of finely divided iron to form ammonia.