NCERT · Class 11 · Chemistry · Chemical ThermodynamicsIf a reaction has $\Delta H = +30.58\text{ kJ mol}^{-1}$ and $\Delta S = +66.1\text{ J K}^{-1}\text{mol}^{-1}$, at what temperature will the reaction reach equilibrium?
Step-by-Step Solution
At equilibrium, $\Delta G = 0 \implies \Delta H - T\Delta S = 0 \implies T = \frac{\Delta H}{\Delta S}$. Converting $\Delta H$ to J: $T = \frac{30580\text{ J mol}^{-1}}{66.1\text{ J K}^{-1}\text{mol}^{-1}} \approx 462.6\text{ K}$.
Detailed Options Breakdown
Option : $462.6\text{ K}$ (Correct Answer)
Correct choice. Refer to the step-by-step verified solution guidelines above for details.
Option 1: $273\text{ K}$
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Thermodynamics.
Option 2: $500\text{ K}$
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Thermodynamics.
Option 3: $300\text{ K}$
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Thermodynamics.
💡 Study Guide: This question tests core syllabus concepts from Chemical Thermodynamics. For formulas, key summaries, and mock exam reference guides, read the full Chemical Thermodynamics Revision Notes.