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(C) For an ideal gas,the equation of state is given by the ideal gas law:$PV = nRT$where $P$ is pressure,$V$ is volume,$n$ is the number of moles,$R$

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(C) For an ideal gas,the equation of state is given by the ideal gas law:$PV = nRT$where $P$ is pressure,$V$ is volume,$n$ is the number of moles,$R$ is the universal gas constant,and $T$ is the absolute temperature.Since $n$ and $R$ are constants for a given amount of gas,we have:$PV \propto T$This implies that the graph of $PV$ versus $T$ should be a straight line passing through the origin,as $PV$ is directly proportional to $T$.Therefore,the correct graph is the one showing a linear increase of $PV$ with respect to $T$ passing through the origin.

Which of the following graphs represents the behavior of an ideal gas? Symbols have their usual meaning.

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