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Chapter 12: Problem 56

Trace the phase changes that occur as a sample of \(\mathrm{H}_{2} \mathrm{O}(\mathrm{g}),\) originally at \(1.00 \mathrm{mmHg}\) and \(-0.10^{\circ} \mathrm{C},\) is compressed at constant temperature until the pressure reaches 100 atm.

Short Answer

Expert verified
The $H_{2}O_{(g)}$ sample goes through phase changes from gas to liquid and then to solid as the pressure increases from 1.00 mmHg to 100 atm at a constant temperature of -0.10°C.

Step by step solution

01

Identify initial state

The sample of water begins as gas (\(H_{2}O_{(g)}\)) and is under low pressure (1.00 mmHg) and low temperature (-0.10°C). Utilize the phase diagram of water to initially place the state.
02

Follow the isotherm

Start from the initial position identified in Step 1, and trace horizontally along the isotherm (constant temperature) line as the pressure increases. The phase will change from gas to liquid as the pressure reaches the vapor pressure line for -0.10°C.
03

Reach final state

Keep tracing along the isotherm line until pressure reaches 100 atm. As the pressure keeps increasing, the phase will then change from liquid to solid - contrary to most substances but characteristic for water due to its density anomalies.

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Most popular questions from this chapter

Why is the triple point of water (ice-liquid-vapor) a better fixed point for establishing a thermometric scale than either the melting point of ice or the boiling point of water?

Of the compounds \(\mathrm{HF}, \mathrm{CH}_{4}, \mathrm{CH}_{3} \mathrm{OH}, \mathrm{N}_{2} \mathrm{H}_{4},\) and \(\mathrm{CHCl}_{3},\) hydrogen bonding is an important intermolecular force in (a) none of these; (b) two of these; (c) three of these; (d) all but one of these; (e) all of these.

Explain why vaporization occurs only at the surface of a liquid until the boiling point temperature is reached. That is, why does vapor not form throughout the liquid at all temperatures?

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Sketch a plausible phase diagram for hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right)\) from the following data: triple point \(\left(2.0^{\circ} \mathrm{C}\right)\) and \(3.4 \mathrm{mm} \mathrm{Hg}\) ), the normal melting point \(\left(2^{\circ} \mathrm{C}\right),\) the normal boiling point \(\left(113.5^{\circ} \mathrm{C}\right),\) and the critical point \(\left(380^{\circ} \mathrm{C} \text { and } 145 \mathrm{atm}\right) .\) The density of the liquid is less than that of the solid. Label significant data points on this diagram. Are there any features of the diagram that remain uncertain? Explain.
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