Q3.4 Reflecting on Differences in Phases Think about what you already know about different phases of matter. Given this figure showing the process of changing from one phase to another, what parameter (physical quantity of a system) serves as an indicator for energy flowing into or out of the molecular system? Gas Cool or compress Heat or reduce pressure Liquid Cool Heat Crystalline solid In the box below, make a claim as to which parameter is represented in the processes in the figure and use your ideas of energy to support your claim.

Q3.4 Reflecting on Differences in Phases Think about what you already know about different phases of matter. Given this figure showing the process of changing from one phase to another, what parameter (physical quantity of a system) serves as an indicator for energy flowing into or out of the molecular system? Gas Cool or compress Heat or reduce pressure Liquid Cool Heat Crystalline solid In the box below, make a claim as to which parameter is represented in the processes in the figure and use your ideas of energy to support your claim.

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.25E: 6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of...

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6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .
he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?
he following demonstration takes place in a two-step process: rst, solid calcium carbide (CaC2j)reacts with liquid water to produce acetylene gas (C2H2)and aqueous calcium hydroxide. Second the acetylene gas produced is then ignited with a match, causing the combustion reaction of acetylene with oxygen gas to produce gaseous carbon dioxide and gaseous water. Write the balanced equations for each reaction that is occurring, including all phases. If a 100.0gsample of calcium carbide (CaC2)is initially reacted with 50.0gof water, which reactant is limiting? Now imagine that the final gases produced are collected in a large bulkier and allowed to cool to room temperature. Using the information from part b ( l00.0gof Cec2reacting with 50.0gof H2O), how many liters of carbon dioxide gas were produced in the balloon at a pressure of 1.00atm and 25C?
There are three sets of sketches below, showing the same pure molecular compound (water, molec sketches are drawn as if a sample of water were under a microscope so powerful that individual ato Use the slider to choose the correct sketch in each set. You may need the following information: EASUREMENT AND MATTER Distinguishing solid, liquid and gas phases of a pure substance ! 1 melting point of H₂O: 0.0°C boiling point of H₂O: 100.0 °C Explanation Q 85. °C A G N NO 2 Check F W S -27, "C it 3 ** X E H D X $ 4 O O 159. C ** 20 R 3 C % 5 LL MacBook Air T V A 6 G Y & 7 H B
Write the balanced chemical equation for the Haber–Bosch process (i.e., the combination of nitrogen and hydrogen to form ammonia, NH3NH3 ). Phase symbols are optional.
An autoclave is used to sterilize surgical equipment. Itis far more effective than steam produced from boilingwater in the open atmosphere because it generates steamat a pressure of 2 atm. Explain why an autoclave is such anefficient sterilization device
6. Below is an outline for the phase diagram for carbon tetrachloride. Label all of the following on the diagram: y-axis & x-axis with appropriate units; gas, liquid and solid phases; triple and critical points. Then answer the questions that follow. Describe what happens when a sample of carbon tetrachloride is heated at constant pressure of а. 0.75 atm from 248K to 254K. Draw an arrow that represents this. b. What phases are present at the point on the graph labeled b? 249.0 250.3
Describe the properties of solidsand liquids and relate them totheir constituent atoms andmolecules.
(a) Two pans of water are on different burners of a stove. Onepan of water is boiling vigorously, while the other is boilinggently. What can be said about the temperature of the waterin the two pans? (b) A large container of water and a smallone are at the same temperature. What can be said about therelative vapor pressures of the water in the two containers?
(a) Identify the major phases (ice, water, vapor) on the unary phase diagram of H2O below.
Ethylene glycol (HOCH2CH2OH) and pentane (C5H12) areboth liquids at room temperature and room pressure, andhave about the same molecular weight. (a) One of these liquidsis much more viscous than the other. Which one doyou predict is more viscous? (b) One of these liquids has amuch lower normal boiling point (36.1 °C) compared to theother one (198 °C). Which liquid has the lower normal boilingpoint? (c) One of these liquids is the major componentin antifreeze in automobile engines. Which liquid wouldyou expect to be used as antifreeze? (d) One of these liquidsis used as a “blowing agent” in the manufacture of polystyrenefoam because it is so volatile. Which liquid would youexpect to be used as a blowing agent?
7. (5)Consider the phase diagram given below atm ス50 T°C aら 50 15 100 |50 200 Identify the normal boiling point, and normal freezing point. fp. Which phase, solid or liquid is most densed? bp Indicate the Triple point and the critical point on the diagram.