An ideal gas expands isothermally from volume | vedclass

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(D) $1$. In the $p-V$ diagram,the isothermal expansion from $A$ to $B$ follows the curve $AB$. The adiabatic compression from $B$ to $C$ follows the c

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$p_2 > p_1, W < 0$

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(D) $1$. In the $p-V$ diagram,the isothermal expansion from $A$ to $B$ follows the curve $AB$. The adiabatic compression from $B$ to $C$ follows the curve $BC$.$2$. From the graph,it is clear that the final pressure $p_2$ at point $C$ is greater than the initial pressure $p_1$ at point $A$ $(p_2 > p_1)$.$3$. The net work done $W$ by the gas in a cyclic process is equal to the area enclosed by the cycle $ABCA$. Since the process is counter-clockwise (expansion $A 	o B$ followed by compression $B 	o C$),the work done by the gas is negative $(W $4$. Alternatively,the area under the adiabatic curve $BC$ (which is the work done on the gas during compression) is greater than the area under the isothermal curve $AB$ (which is the work done by the gas during expansion). Thus,the net work done by the gas is negative.$5$. Therefore,$p_2 > p_1$ and $W < 0$.

An ideal gas expands isothermally from volume $V_1$ to volume $V_2$. It is then compressed to the original volume $V_1$ adiabatically. If $p_1$ and $p_2$ represent the initial pressure and final pressure respectively,and $W$ represents the net work done by the gas during the entire process,then:

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