A reaction's rate constant doubles when T increases from 300 K to 310 K.
Approximately what is Eₐ (using Arrhenius)?
- A
100 kJ/mol
- B
26.8 kJ/mol
- Ccheck_circle
53.6 kJ/mol
- D
8.31 kJ/mol
Explanation
ln(k₂/k₁) = (Eₐ/R)(1/T₁ − 1/T₂). ln 2 = (Eₐ/8.314)(1/300 − 1/310) = (Eₐ/8.314)(1.075×10⁻⁴). Eₐ = 0.693·8.314/1.075×10⁻⁴ = 5.36×10⁴ J/mol ≈ 53.6 kJ/mol.