Domanda del libro di testo
Based on the phase diagram of CO2 shown in Figure 11.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (a) 1 atm
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Ch.12 - Liquids, Solids & Intermolecular Forces
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
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Capitolo 12, Problema 94
A sealed flask contains 0.55 g of water at 28 °C. The vapor pressure of water at this temperature is 28.35 mmHg. What is the minimum volume of the flask in order that no liquid water be present in the flask?
Guida verificata passo dopo passo1
Convert the mass of water from grams to moles using the molar mass of water (18.02 g/mol).
Use the ideal gas law equation, PV = nRT, to find the volume. Here, P is the vapor pressure (converted to atm), n is the number of moles calculated in the previous step, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin (28 °C + 273.15).
Convert the vapor pressure from mmHg to atm by dividing by 760 mmHg/atm.
Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.
Rearrange the ideal gas law equation to solve for V (volume): V = nRT/P, and substitute the known values to find the minimum volume of the flask.
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Vapor Pressure
Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid or solid phase at a given temperature. It indicates the tendency of molecules to escape from the liquid phase into the vapor phase. In this question, the vapor pressure of water at 28 °C is 28.35 mmHg, which is crucial for determining the conditions under which all liquid water will evaporate.
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Percorso guidato
02:40
Raoult's Law and Vapor Pressure
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for calculating the volume of gas produced from the evaporation of water in the flask. By knowing the number of moles of water vapor and the vapor pressure, we can determine the minimum volume required to ensure no liquid water remains.
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Percorso guidato
01:15Ideal Gas Law Formula
Molar Mass and Moles
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole. For water, the molar mass is approximately 18.02 g/mol. Understanding how to convert grams of water to moles is necessary for applying the Ideal Gas Law and calculating the volume of vapor needed to prevent the presence of liquid water in the flask.
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Percorso guidato
02:11Molar Mass Concept
Pratica correlata
Domanda del libro di testo
Air conditioners not only cool air, but dry it as well. A room in a home measures 6.0 m × 10.0 m × 2.2 m. If the outdoor temperature is 30 °C and the partial pressure of water in the air is 85% of the vapor pressure of water at this temperature, what mass of water must be removed from the air each time the volume of air in the room is cycled through the air conditioner? (Assume that all of the water must be removed from the air.) The vapor pressure for water at 30 °C is 31.8 torr.
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Domanda del libro di testo
A sample of steam with a mass of 0.552 g and at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °C. Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?
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