A 31.4 mL sample of nitrogen gas was collected over water at 23.7°C and a total pressure of 706 torr. What mass of nitrogen gas was collected

Explanation:

Hello!

In this case, since the collection of gases over at certain conditions implies the usage of the ideal gas equation and computation of the pressure of the gas by subtracting the vapor pressure of water (21.7 torr at 23.7 °C) to the total pressure as shown below:

Next step is to compute the moles of nitrogen at the given conditions:

Final step is to compute the mass by knowing that gaseous nitrogen has a molar mass of 28.02 g/mol:

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hey there!

boiling point is the temperature at which the vapor pressure of the liquid equals atmospheric pressure. the vapor pressure of solvent molecules is decreased when a solute is added, so a higher temperature is required to increase the number of solvent molecules in the gas phase above the liquid.

at the freezing point, the vapor pressures of the solid and liquid are equal; a lower temperature is needed to reduce the number of solvent particles above the liquid.

hope this you

tobey

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