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(C) According to the van der Waals equation for real gases,the pressure is given by $P_{real} = P_{ideal} - a(n/V)^2$. Here,the term $a(n/V)^2$ repres

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$> P$

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(C) According to the van der Waals equation for real gases,the pressure is given by $P_{real} = P_{ideal} - a(n/V)^2$. Here,the term $a(n/V)^2$ represents the reduction in pressure due to intermolecular forces of attraction. If these intermolecular forces are absent (i.e.,$a = 0$),the observed pressure $P$ would be equal to the ideal pressure,which is higher than the pressure observed when forces are present. Therefore,the observed pressure in the absence of such forces will be greater than the pressure $P$ observed with them.

Temperature	Pressure thermometer $A$	Pressure thermometer $B$
Triple-point of water	$1.250 \times 10^{5} \; Pa$	$0.200 \times 10^{5} \; Pa$
Normal melting point of sulphur	$1.797 \times 10^{5} \; Pa$	$0.287 \times 10^{5} \; Pa$

In the absence of intermolecular forces of attraction,the observed pressure $P$ will be

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