Domanda del libro di testo
The vapor pressure of CCl3F at 300 K is 856 torr. If 3.5 g of CCl3F is enclosed in a 1.0-L container, will any liquid be present? If so, what mass of liquid?
Ch.12 - Liquids, Solids & Intermolecular Forces
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217
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TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving118
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds131
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions82
- Ch.6 - Gases114
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements90
- Ch.10 - Chemical Bonding I: The Lewis Model89
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials47
- Ch.14 - Solutions90
- Ch.15 - Chemical Kinetics115
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases136
- Ch.18 - Aqueous Ionic Equilibrium153
- Ch.19 - Free Energy & Thermodynamics93
- Ch.20 - Electrochemistry106
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry140
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Capitolo 12, Problema 91
The vapor pressure of water at 25 °C is 23.76 torr. If 0.25 g of water is enclosed in a 1.50-L container, will any liquid be present? If so, what mass of liquid?
Guida verificata passo dopo passo1
Calculate the number of moles of water using the formula: \( n = \frac{m}{M} \), where \( m \) is the mass of water (0.25 g) and \( M \) is the molar mass of water (18.02 g/mol).
Use the ideal gas law to calculate the pressure exerted by the water vapor if all the water were to vaporize: \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume (1.50 L), \( n \) is the number of moles calculated in step 1, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin (25 °C = 298 K).
Convert the calculated pressure from atm to torr (1 atm = 760 torr) to compare with the given vapor pressure of water at 25 °C (23.76 torr).
Compare the calculated vapor pressure with the given vapor pressure of water. If the calculated pressure is greater than 23.76 torr, not all water will vaporize, and some liquid will remain.
If liquid remains, calculate the mass of water that remains as liquid by determining the difference between the initial mass and the mass that would vaporize to reach the equilibrium vapor pressure.
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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. For water at 25 °C, the vapor pressure is 23.76 torr, meaning that at this temperature, water molecules escape into the vapor phase until this pressure is reached. Understanding vapor pressure is crucial for determining whether liquid water will remain in a closed container.
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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. In this scenario, it can be used to calculate the number of moles of water vapor that can exist in the 1.50-L container at the given vapor pressure. This helps in assessing whether the amount of water vapor exceeds the capacity of the container, indicating if any liquid water will remain.
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01:15Ideal Gas Law Formula
Phase Equilibrium
Phase equilibrium occurs when the rates of evaporation and condensation of a substance are equal, resulting in a stable amount of liquid and vapor. In this case, if the amount of water vapor produced from the 0.25 g of water exceeds the vapor pressure of 23.76 torr, the system will reach equilibrium with some liquid remaining. Understanding this concept is essential for predicting the presence of liquid water in the container.
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03:22Phase Changes in Diagrams
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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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Domanda del libro di testo
Explain the observed trend in the melting points of the hydrogen halides.
HI -50.8 °C
HBr -88.5 °C
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