Question

Write Arrhenius equation.

Hint:

The Arrhenius equation is crucial for understanding how temperature affects the rate of chemical reactions, and is widely used in reaction kinetics.

Answer 1

Step 1: Understand the Arrhenius Equation.
The Arrhenius equation describes the relationship between the rate of a chemical reaction and the temperature. It is given by the equation: \[ k = A e^{-\frac{E_a}{RT}} \] Where: - \( k \) is the rate constant of the reaction. - \( A \) is the pre-exponential factor (frequency factor), which represents the number of collisions that result in a reaction. - \( E_a \) is the activation energy of the reaction. - \( R \) is the universal gas constant (8.314 J/mol·K). - \( T \) is the temperature in Kelvin.
Step 2: Explanation.
This equation shows that the rate constant \( k \) increases with temperature, as the exponential factor \( e^{-\frac{E_a}{RT}} \) becomes larger as \( T \) increases. Thus, higher temperatures result in more frequent and energetic collisions, which speeds up the reaction.
Final Answer: The Arrhenius equation relates the rate constant of a reaction to the temperature and activation energy, given by: \[ k = A e^{-\frac{E_a}{RT}} \]
Final Answer: \[ \boxed{k = A e^{-\frac{E_a}{RT}}} \]