A sealed flask contains 0.55 g of water at 28^∘ C. The vapor pressure of water at this temperat

step 1 In this question we want to determine the volume. And for us to simplify these calculations, we

A sealed flask contains 0.55 g of water at 28^∘ C. The...

A sealed flask contains $0.55 \mathrm{~g}$ of water at $28^{\circ} \mathrm{C}$. The vapor pressure of water at this temperature is $28.36 \mathrm{mmHg}$. What is the minimum volume of the flask in order that no liquid water be present in the flask?

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Key Concepts

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid (or solid) phase at a given temperature. It is an intrinsic property of the substance and determines the conditions under which the substance will exist as a vapor, critical for understanding phase transitions.

Phase Equilibrium

Phase equilibrium occurs when the rate of evaporation equals the rate of condensation, resulting in no net change between phases. In this context, the vapor pressure represents the equilibrium pressure of water vapor above its liquid, ensuring that if the partial pressure reaches this value, no additional liquid is present.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates the pressure, volume, number of moles, gas constant, and temperature of a gas. It is used to calculate the minimum flask volume required to contain a given amount of water vapor when the vapor is at its equilibrium (saturation) pressure.

Mole Concept

The mole concept allows conversion between the mass of a substance and the number of moles, using the substance's molar mass. This conversion is essential when applying the ideal gas law to determine the volume needed for the vapor in the flask.

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