$10^{23}$ molecules of nitrogen, argon and carbon dioxide each are confined in three closed boxes of a large fixed volume V, at the same temperature T. Knowing the molecular weights of the gases are in the order $M_{C O_{2}}$ > $M_{N_{2}}$ > $M_{A_{r}}$ , what can you say about the pressures of the gases in each container?

$P_{A_{r}}$ > $P_{N_{2}}$ > $P_{C O_{2}}$

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$P_{C O_{2}}$ > $P_{N_{2}} = P_{A_{r}}$

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$P_{C O_{2}}$ > $P_{N_{2}}$ > $P_{C O_{2}}$

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$P_{A_{r}} = P_{N_{2}} = P_{C O_{2}}$

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Solution

The correct option is D
$P_{A_{r}} = P_{N_{2}} = P_{C O_{2}}$

At low densities, all real gases seem to obey the ideal gas equation PV=nRT.

This suggests, at constant volume, quantity, and temperature, $P = (\frac{n R T}{v})$ will be same for all gases.

$∴$ In our discussion, $P_{A_{r}} = P_{N_{2}} = P_{C O_{2}}$ .

The molecular masses won't play any real role at low densities

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$10^{23}$ molecules of nitrogen, argon and carbon dioxide each are confined in three closed boxes of a large fixed volume V, at the same temperature T. Knowing the molecular weights of the gases are in the order $M_{C O_{2}}$ > $M_{N_{2}}$ > $M_{A_{r}}$ , what can you say about the pressures of the gases in each container?

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1023 molecules of nitrogen, argon and carbon dioxide each are confined in three closed boxes of a large fixed volume V, at the same temperature T. Knowing the molecular weights of the gases are in the order MCO2>MN2>MAr, what can you say about the pressures of the gases in each container?