Chemistry - Thermodynamics - I Question with Solution | TestHub

ChemistryThermodynamics - IHeat & Heat CapacityMedium2 minQB

ChemistryMediummultiple choice

Select the correct statement(s) :

Options:(select one or more)

Answer:

B, C

Solution:

Statement (A) is incorrect: Heat ( $q$ ) is a path function, not a state property of a system.

Statement (B) is correct: Enthalpy is defined as $H = U + P V$ , so $Δ H = Δ U + Δ (P V)$ holds true universally for any system (ideal or real gas).

Statement (C) is correct: For an isobaric process ( $Δ P = 0$ ), the entropy change formula $Δ S = n C_{P, m} ln \frac{T _{2}}{T _{1}}$ is derived purely from $d H = n C_{P, m} d T$ and $d S = \frac{d H}{T}$ , which applies to both ideal and real gases under constant pressure.

Statement (D) is incorrect: The expression $Δ S = n R ln \frac{V _{2}}{V _{1}}$ assumes the ideal gas law ( $P = \frac{n RT}{V}$ ) during derivation, making it invalid for real gases.

Stream:JEESubject:ChemistryTopic:Thermodynamics - ISubtopic:Heat & Heat Capacity

⏱ 2mℹ️ Source: QB

Doubts & Discussion

Loading discussions...