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 62
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?
Guida verificata passo dopo passo1
Identify the total pressure of the gas mixture, which is given as 745 mmHg.
List the partial pressures of the known gases: CO2 is 125 mmHg, Ar is 214 mmHg, and O2 is 187 mmHg.
Use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of all gases in the mixture. Set up the equation: P_total = P_CO2 + P_Ar + P_O2 + P_He.
Rearrange the equation to solve for the partial pressure of helium (P_He): P_He = P_total - (P_CO2 + P_Ar + P_O2).
To find the mass of helium, use the ideal gas law: PV = nRT. Solve for n (moles of He) using the partial pressure of He, the volume (12.0 L), and the temperature (273 K). Then, convert moles to grams using the molar mass of helium (4.00 g/mol).
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.
Dalton's Law of Partial Pressures
Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle allows us to calculate the partial pressure of an unknown gas in a mixture by subtracting the known partial pressures from the total pressure.
Video consigliato:
Percorso guidato
00:27
Dalton's Law and Partial 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 mass of a gas when its volume, temperature, and pressure are known, as it allows us to determine the number of moles and subsequently convert to mass using the molar mass.
Video consigliato:
Percorso guidato
01:15Ideal Gas Law Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the number of moles of a gas and its mass. Knowing the molar mass of helium (approximately 4.00 g/mol) enables us to calculate the mass of helium present in the gas mixture once we determine the number of moles using the Ideal Gas Law.
Video consigliato:
Percorso guidato
02:11Molar Mass Concept
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 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?
2978
views
Domanda del libro di testo
A sample of gas has a mass of 38.8 mg. Its volume is 224 mL at a temperature of 55 °C and a pressure of 886 torr. Find the molar mass of the gas.
2066
views
1
rank
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