A gaseous sample expands from 200 , cm^3 to 5 | vedclass

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(D) Given: Heat absorbed $q = +1.5 \, J$. Expansion volume $\Delta V = 500 \, cm^3 - 200 \, cm^3 = 300 \, cm^3 = 0.3 \, L$. External pressure $P = \fr

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$-28.1$

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(D) Given: Heat absorbed $q = +1.5 \, J$. Expansion volume $\Delta V = 500 \, cm^3 - 200 \, cm^3 = 300 \, cm^3 = 0.3 \, L$. External pressure $P = \frac{750}{760} \, atm \approx 0.9868 \, atm$. Work done $W = -P_{ext} \Delta V = -0.9868 \, atm 	imes 0.3 \, L = -0.29604 \, atm \cdot L$. Converting work to Joules: $W = -0.29604 	imes 101.3 \, J \approx -29.99 \, J$ (using standard conversion $1 \, atm \cdot L = 101.3 \, J$). Using the First Law of Thermodynamics: $\Delta U = q + W$. $\Delta U = 1.5 \, J - 29.6 \, J = -28.1 \, J$.

$A$ gaseous sample expands from $200 \, cm^3$ to $500 \, cm^3$ against a constant external pressure of $750 \, torr$ while absorbing $1.5 \, J$ of heat. What is the change in internal energy of the system in $J$? $(1 \, atm \cdot L = 101.3 \, J)$

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