CBSE · Class 11 · Chemistry · Chemical ThermodynamicsWhat is the relationship between enthalpy change ($\Delta H$) and internal energy change ($\Delta U$) for a gaseous reaction?
Step-by-Step Solution
The correct relationship for a chemical reaction involving gases at constant temperature and pressure is given by $\Delta H = \Delta U + \Delta n_g RT$, where $\Delta n_g$ is the difference between moles of gaseous products and gaseous reactants.
Detailed Options Breakdown
Option : $\Delta H = \Delta U + \Delta n_g RT$ (Correct Answer)
Correct choice. Refer to the step-by-step verified solution guidelines above for details.
Option 1: $\Delta U = \Delta H + \Delta n_g RT$
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Thermodynamics.
Option 2: $\Delta H = \Delta U - \Delta n_g RT$
Incorrect choice. This distractor represents a common misunderstanding of the core principles of Chemical Thermodynamics.
Option 3: $\Delta H = \frac{\Delta U}{\Delta n_g RT}$
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.