Final answer:
The correct relationship between activation energy and rate constants at two different temperatures is given by option B: ln k₂/k₁ = -E₊/R(1/T₁ - 1/T₂), which is derived from the Arrhenius equation. Therefore, the correct option is B.
Step-by-step explanation:
The activation energy (E₊) and rate constants (k₁ and k₂) of a chemical reaction at two different temperatures (T₁ and T₂) are related by the Arrhenius equation, which can be expressed as:
ln k = ln A - E₊/RT
By rearranging this equation for two different temperatures and then taking the difference, we get the following relationship:
ln k₂/k₁ = -E₊/R(1/T₁ - 1/T₂)
From the options provided by the question, the correct expression that relates the rate constants and the activation energy is:
B. ln k₂/k₁ = -E₊/R(1/T₁ - 1/T₂)