An ideal gas follows a process PT = text{cons | vedclass

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(C) Given the process: $PT = 	ext{constant}$.From the ideal gas equation, we know that $PV = nRT$, which implies $T = \frac{PV}{nR}$.Substituting thi

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(C) Given the process: $PT = 	ext{constant}$.From the ideal gas equation, we know that $PV = nRT$, which implies $T = \frac{PV}{nR}$.Substituting this into the given process equation:$P \left( \frac{PV}{nR} ight) = 	ext{constant}$Since $n$ and $R$ are constants, we get:$P^2 V = 	ext{constant}$This can be rewritten as $P^2 = \frac{k}{V}$, or $P = \frac{k'}{\sqrt{V}}$, where $k$ and $k'$ are constants.This represents a curve where $P$ decreases as $V$ increases, specifically following the form $P \propto V^{-1/2}$. This corresponds to the graph shown in option $C$.

An ideal gas follows a process $PT = \text{constant}$. The correct graph between pressure $(P)$ and volume $(V)$ is:

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