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Ch.15 - Chemical Equilibrium
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.15 - Chemical Equilibrium문제 98d
15장, 문제 98d

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?
Phase diagram for SO2 showing solid, liquid, and gas phases with points A, B, C, and D marked.

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1
Identify the conditions under which a gas behaves ideally: low pressure and high temperature.
Examine the phase diagram and locate the points A, B, C, and D.
Determine the pressure and temperature at each point: A (low pressure, low temperature), B (low pressure, moderate temperature), C (moderate pressure, high temperature), D (high pressure, high temperature).
Compare the conditions at each point to the ideal gas conditions.
Conclude that the point with the lowest pressure and highest temperature is where SO2(g) most closely approaches ideal-gas behavior.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Ideal Gas Behavior

Ideal gas behavior refers to the theoretical condition where a gas perfectly follows the ideal gas law (PV=nRT) without deviations. This occurs at high temperatures and low pressures, where intermolecular forces are negligible, and the volume of gas particles is insignificant compared to the volume of the container. Understanding this concept is crucial for identifying conditions under which real gases, like SO2, behave more like ideal gases.
추천 영상:
가이드 코스
01:15
Ideal Gas Law Formula

Phase Diagram

A phase diagram is a graphical representation that shows the phases of a substance (solid, liquid, gas) at various temperatures and pressures. It helps visualize the conditions under which a substance exists in different states and the transitions between these states. In the context of the question, the phase diagram for SO2 indicates the regions where the gas phase is stable and where it may exhibit ideal behavior.
추천 영상:
가이드 코스
03:22
Phase Changes in Diagrams

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. At this point, the substance exhibits unique properties, and the behavior of gases can deviate significantly from ideal conditions. Recognizing the critical point is essential for understanding where SO2 may approach ideal gas behavior, particularly in relation to the marked points in the diagram.
추천 영상:
가이드 코스
03:05
Boiling Point Elevation
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교과서 질문

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.

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교과서 질문

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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교과서 질문

The phase diagram for SO2 is shown here. (e) At which of the three red points does SO2(g) behave least ideally?

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교과서 질문

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.

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