Exams › JEE Advanced › Chemistry

An ideal gas starts from initial state A and undergoes three different adiabatic processes, each ending at the same final pressure. The adiabatic reversible process ends at point B, and the adiabatic single-step irreversible process ends at point C. On a P-V diagram (with the final pressure as a horizontal line), B lies to the left of C. Where does the adiabatic free expansion (against zero external pressure) to the same final pressure end up?

1. A
2. P
3. Q
4. R

Correct answer: R

Solution

Ranking of final volumes at the same pressure: reversible adiabatic gives minimum volume (B), irreversible single-step gives larger volume (C), and free expansion gives the largest volume (R) because temperature stays at its initial value and V = nRT_initial/P_final is maximum. R is the rightmost point on the final pressure line.

Related JEE Advanced Chemistry questions

• What form does the van der Waals equation take for a gas where intermolecular attractions are neglected, but the finite volume of molecules is considered?
• In the van der Waals equation, what does the term (a)/(V²) signify?
• A sealed container holds 10 g of an ideal gas X at 300 K, exerting a pressure of 2 atm. When 80 g of a different ideal gas Y is introduced at the same temperature, the pressure rises to 6 atm. What is the ratio of the root mean square speeds of X and Y at 300 K?
• The compressibility factor Z of a Van der Waals gas is 0.5 at 27 degrees C and 24 atm. Given b = 0.10 L/mol and R = 0.08 L-atm/(K-mol), find the Van der Waals constant a in atm-L²/mol².
• Identify the INCORRECT statement about real gases:
• Which combination of conditions is most favourable for the melting of ice into water?

⚔️ Practice JEE Advanced Chemistry free + battle 1v1 →