NEET 2017 · ChemistryPrevious Year Question

A gas is allowed to expand in a well insulated container against a constant external pressure of $2.5 atm$ from an initial volume of $2.50 L$ to a final volume of $4.50 L$ . The change in internal energy $Δ U$ of the gas in joules will be

Answer: (C) $- 505 J$ . \textbf{Answer:} (C) $- 505 J$ \textbf{Solution:} A well-insulated container means the process is adiabatic, so $q = 0$ .

A. $1136.25 J$
B. $- 500 J$
C. $- 505 J$ ✓
D. $+ 505 J$

Correct Answer

Solution & Explanation

\textbf{Answer:} (C) $- 505 J$ \textbf{Solution:} A well-insulated container means the process is adiabatic, so $q = 0$ . By the first law $Δ U = q + w = w$ . The work done on the gas against a constant external pressure is $w = - p_{e x t} Δ V = - 2.5 atm \times (4.50 - 2.50) L = - 5 L atm$ . Converting, $- 5 \times 101.3 J \approx - 506.5 J \approx - 505 J$ .

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A gas is allowed to expand in a well insulated container against a constant external pressure of 2.5 atm from an initial volume of 2.50 L to a final volume of 4.50 L. The change in internal energy ΔU of the gas in joules will be

Solution & Explanation

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A gas is allowed to expand in a well insulated container against a constant external pressure of $2.5 atm$ from an initial volume of $2.50 L$ to a final volume of $4.50 L$ . The change in internal energy $Δ U$ of the gas in joules will be