Domanda del libro di testo
A gas mixture contains 1.25 g N2 and 0.85 g O2 in a 1.55 L container at 18 °C. Calculate the mole fraction and partial pressure of each component in the gas mixture.
2513
views
1
rank
Ch.5 - Gases
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831
Non è quello che usi tu?Cambia libro di testoScegli un libro di testo diverso
TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving136
- Ch.2 - Atoms & Elements112
- Ch.3 - Molecules, Compounds & Chemical Equations159
- Ch.4 - Chemical Quantities & Aqueous Reactions140
- Ch.5 - Gases118
- Ch.6 - Thermochemistry106
- Ch.7 - Quantum-Mechanical Model of the Atom62
- Ch.8 - Periodic Properties of the Elements103
- Ch.9 - Chemical Bonding I: The Lewis Model104
- Ch.10 - Chemical Bonding II: Molecular Shapes & Valence Bond Theory89
- Ch.11 - Liquids, Solids & Intermolecular Forces73
- Ch.12 - Solids and Modern Material59
- Ch.13 - Solutions110
- Ch.14 - Chemical Kinetics140
- Ch.15 - Chemical Equilibrium78
- Ch.16 - Acids and Bases155
- Ch.17 - Aqueous Ionic Equilibrium176
- Ch.18 - Free Energy and Thermodynamics108
- Ch.19 - Electrochemistry118
- Ch.20 - Radioactivity and Nuclear Chemistry82
- Ch.21 - Organic Chemistry150
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Capitolo 5, Problema 63
A 1.20-g sample of dry ice is added to a 755 mL flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas), and the mixture returns to 25.0 °C. What is the total pressure in the flask?
Guida verificata passo dopo passo1
Convert the mass of dry ice (CO₂) to moles using its molar mass (44.01 g/mol).
Use the ideal gas law, PV = nRT, to calculate the pressure exerted by the CO₂ gas. Use the moles of CO₂ calculated, the volume of the flask (755 mL converted to liters), the temperature in Kelvin (25.0 °C converted to 298.15 K), and the ideal gas constant R (0.0821 L·atm/mol·K).
Convert the initial pressure of nitrogen gas from mmHg to atm for consistency with the ideal gas law calculations.
Add the pressure exerted by the CO₂ gas to the initial pressure of the nitrogen gas to find the total pressure in the flask.
Ensure the final total pressure is expressed in the desired units, either atm or mmHg, by converting if necessary.
Risposta video verificata per un problema simile:
Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
4mConcetti chiave
Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.
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 understanding how gases behave under varying conditions and is crucial for calculating the total pressure in the flask after the dry ice sublimates.
Video consigliato:
Percorso guidato
01:15
Ideal Gas Law Formula
Sublimation
Sublimation is the process where a solid transitions directly to a gas without passing through the liquid phase. In this scenario, dry ice (solid CO2) sublimates into gaseous CO2, contributing to the total pressure in the flask, which must be accounted for in the calculations.
Video consigliato:
Percorso guidato
01:52Sublimation Phase Change Example
Dalton's Law of Partial Pressures
Dalton's Law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas present. This concept is vital for determining the total pressure in the flask after the dry ice sublimates, as it allows for the addition of the partial pressure of the newly formed CO2 gas to the existing nitrogen gas pressure.
Video consigliato:
Percorso guidato
00:27Dalton's Law and Partial Pressure
Pratica correlata
Domanda del libro di testo
A 275-mL flask contains pure helium at a pressure of 752 torr. A second flask with a volume of 475 mL contains pure argon at a pressure of 722 torr. If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of argon?
3192
views
Domanda del libro di testo
A gas mixture with a total pressure of 745 mmHg contains each of the following gases at the indicated partial pressures: CO2, 125 mmHg; Ar, 214 mmHg; and O2, 187 mmHg. The mixture also contains helium gas. What is the partial pressure of the helium gas? What mass of helium gas is present in a 12.0-L sample of this mixture at 273 K?
5930
views
Domanda del libro di testo
What is the mole fraction of oxygen gas in air (see Table 5.3)? What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm?
2667
views
1
rank
1
comments
Domanda del libro di testo
A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 °C and a pressure of 753 mmHg. Find the molar mass of the gas.
1825
views
1
comments
Domanda del libro di testo
A gas mixture contains each of the following gases at the indicated partial pressures: N2, 215 torr; O2, 102 torr; and He, 117 torr. What is the total pressure of the mixture? What mass of each gas is present in a 1.35-L sample of this mixture at 25.0 °C?
3669
views