For the P-V diagram given for an ideal gas,wh | vedclass

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(D) From the given $P-V$ diagram,the process follows the relation $P = \frac{	ext{constant}}{V}$,which implies $PV = 	ext{constant}$.According to th

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(D) From the given $P-V$ diagram,the process follows the relation $P = \frac{	ext{constant}}{V}$,which implies $PV = 	ext{constant}$.According to the ideal gas equation $PV = nRT$,if $PV$ is constant,then $T$ must also be constant $(T = 	ext{constant})$.This represents an isothermal process.In a $T-P$ diagram,an isothermal process is represented by a horizontal line (where $T$ remains constant as $P$ changes).Looking at the $P-V$ graph,the pressure $P$ decreases as we move from point $1$ to point $2$ (since $V$ increases).Therefore,in the $T-P$ diagram,the process should be a horizontal line starting from $1$ and moving towards $2$ as $P$ decreases.Among the given options,the graph where $T$ is constant and the transition is from $1$ to $2$ as $P$ decreases is represented by option $(d)$.

For the $P-V$ diagram given for an ideal gas,which of the following correctly represents the $T-P$ diagram?

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