The vapor pressure of I2( s) at 30^∘ C is 0.466 mm Hg . (a) How many milligrams of iodine will s

step 1 the vapor pressure given the vapor pressure of iodine at 30 degrees Celsius and 0 .446 466 milli

The vapor pressure of I2( s) at 30^∘ C is 0.466 mm Hg . (a)...

The vapor pressure of $\mathrm{I}_2(\mathrm{~s})$ at $30^{\circ} \mathrm{C}$ is 0.466 mm Hg . (a) How many milligrams of iodine will sublime into an evacuated 1.00-L flask? (b) If 2.0 mg of $\mathrm{I}_2$ is used, what will the final pressure be? (c) If 10.0 mg of $\mathrm{I}_2$ is used, what will the final pressure be?

The vapor pressure of $\mathrm{I}_2(\mathrm{~s})$ at $30^{\circ} \mathrm{C}$ is 0.466 mm Hg .
(a) How many milligrams of iodine will sublime into an evacuated 1.00-L flask?
(b) If 2.0 mg of $\mathrm{I}_2$ is used, what will the final pressure be?
(c) If 10.0 mg of $\mathrm{I}_2$ is used, what will the final pressure be?

Key Concepts

Ideal Gas Law

The Ideal Gas Law (PV = nRT) is a fundamental principle that relates the pressure, volume, temperature, and amount (in moles) of an ideal gas. It is used to calculate any one of these properties when the others are known, and it is particularly useful for determining the number of gas moles present in a container from the measured pressure and known temperature and volume.

Phase Equilibrium

Phase equilibrium refers to the state in which the physical properties of different phases (solid, liquid, gas) of a substance remain constant over time because the rates of phase transition between them are equal. In the context of sublimation, if an ample supply of a solid is available, the vapor phase will reach and maintain its equilibrium vapor pressure; however, if the amount of solid is limited, the vapor pressure will be lower than the equilibrium value.

Vapor Pressure

Vapor pressure is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature. It is a characteristic property of a substance that indicates the tendency of its molecules to escape into the gas phase, and it remains constant (given enough condensed phase) regardless of the volume of the container.

Sublimation

Sublimation is the phase transition in which a substance goes directly from its solid phase to its gas phase without passing through the liquid phase. This process occurs when the vapor pressure of the solid exceeds the ambient pressure, leading to the formation of vapor which can reach an equilibrium value in a closed or evacuated container.

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