Which of the following statements about the Arrhenius equation is correct?

• A. It describes the relationship between pressure and volume for an ideal gas.
• B. It shows that the rate constant decreases as temperature increases.
• C. It is used to calculate the equilibrium constant of a reaction.
• D. It relates the rate constant k to temperature and activation energy.

Answer: (D)

Verified step by step guidance

1. Understand that the Arrhenius equation is a fundamental formula in chemical kinetics that relates the rate constant \(k\) of a reaction to the temperature \(T\) and the activation energy \(E_a\).
2. Recall the Arrhenius equation: \[k = A \times e^{-\frac{E_a}{RT}}\] where \(A\) is the frequency factor, \(E_a\) is the activation energy, \(R\) is the gas constant, and \(T\) is the absolute temperature in kelvin.
3. Recognize that this equation shows how the rate constant \(k\) changes with temperature and activation energy, specifically that \(k\) increases as temperature increases or activation energy decreases.
4. Note that the Arrhenius equation does not describe relationships involving pressure and volume (which is related to the ideal gas law), nor does it directly calculate equilibrium constants (which are related to thermodynamics, not kinetics).
5. Conclude that the correct statement is that the Arrhenius equation relates the rate constant \(k\) to temperature and activation energy, explaining how reaction rates depend on these factors.