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Ch.15 - Chemical Equilibrium
All textbooksBrown 14th EditionCh.15 - Chemical EquilibriumProblem 98e
Chapter 15, Problem 98e

The phase diagram for SO2 is shown here. (e) At which of the three red points does SO2(g) behave least ideally?
Phase diagram for SO2 showing solid, liquid, gas, and critical points with marked points A, B, C, D.

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1
Identify the three red points on the phase diagram: A, B, and C.
Recall that gases behave least ideally at high pressures and low temperatures.
Examine the phase diagram to determine the pressure and temperature at each of the three points.
Compare the pressures and temperatures at points A, B, and C to determine which point has the highest pressure and/or lowest temperature.
Conclude that the point with the highest pressure and/or lowest temperature is where SO2(g) behaves least ideally.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ideal Gas Behavior

Ideal gas behavior refers to the theoretical behavior of gases that follow the ideal gas law (PV=nRT) perfectly, where pressure (P), volume (V), temperature (T), and the number of moles (n) are related. Real gases deviate from this behavior under high pressure and low temperature, where intermolecular forces and molecular volume become significant. Understanding these deviations is crucial for determining conditions under which a gas behaves least ideally.
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Phase Diagrams

A phase diagram is a graphical representation that shows the phases of a substance (solid, liquid, gas) as a function of temperature and pressure. It includes critical points, triple points, and phase boundaries, which indicate the conditions under which different phases coexist. Analyzing phase diagrams helps predict the state of a substance under varying conditions and is essential for understanding the behavior of SO2 in the given question.
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Critical Point

The critical point on a phase diagram marks the end of the liquid-gas phase boundary, beyond which the distinction between liquid and gas phases disappears, resulting in a supercritical fluid. At this point, properties of the substance change dramatically, and it can exhibit behaviors of both phases. Understanding the critical point is vital for identifying conditions where SO2 behaves least ideally, as gases near this point often show significant deviations from ideal behavior.
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Related Practice
Textbook Question

The following equilibria were measured at 823 K: CoO(s) + H2(g) ⇌ Co(s) + H2O(g) Kc = 67 H2(g) + CO2(g) ⇌ CO(g) + H2O(g) Kc = 0.14 (a) Use these equilibria to calculate the equilibrium constant, Kc, for the reaction CoO(s) + CO(g) ⇌ Co(s) + CO2(g) at 823 K.

Textbook Question

The following equilibria were measured at 823 K: CoO(s) + H2(g) ⇌ Co(s) + H2O(g) Kc = 67 H2(g) + CO2(g) ⇌ CO(g) + H2O(g) Kc = 0.14 (d) If the reaction vessel from part (c) is heated to 823 K and allowed to come to equilibrium, how much CoO(s) remains?

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Textbook Question

The phase diagram for SO2 is shown here. (d) At which of the three points marked in red does SO2(g) most closely approach ideal-gas behavior?

Textbook Question

In Section 11.5, we defined the vapor pressure of a liquid in terms of an equilibrium. (a) Write the equation representing the equilibrium between liquid water and water vapor and the corresponding expression for Kp.

Textbook Question

In Section 11.5, we defined the vapor pressure of a liquid in terms of an equilibrium. (b) By using data in Appendix B, give the value of Kp for this reaction at 30 C.