Domanda del libro di testo
At an underwater depth of 250 ft, the pressure is 8.38 atm. What should the mole percent of oxygen be in the diving gas for the partial pressure of oxygen in the mixture to be 0.21 atm, the same as in air at 1 atm?
Ch.10 - Gases
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
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Capitolo 10, Problema 68b
A sample of 5.00 mL of diethyl ether (C2H5OC2H5,density=0.7134 g/mL) is introduced into a 6.00-L vessel that already contains a mixture of N2 and O2, whose partial pressures are 𝑃N2=0.751atm and 𝑃O2=0.208atm. The temperature is held at 35.0°C, and the diethyl ether totally evaporates. b. Calculate the total pressure in the container.
Guida verificata passo dopo passo1
Calculate the mass of diethyl ether using its volume and density: \( \text{mass} = \text{volume} \times \text{density} \).
Convert the mass of diethyl ether to moles using its molar mass: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \).
Use the ideal gas law to find the partial pressure of diethyl ether: \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin.
Add the partial pressures of N2, O2, and diethyl ether to find the total pressure in the container: \( P_{\text{total}} = P_{\text{N2}} + P_{\text{O2}} + P_{\text{ether}} \).
Ensure all pressures are in the same units (e.g., atm) before adding them to find the total pressure.
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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 a container after the diethyl ether evaporates.
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Percorso guidato
01:15
Ideal Gas Law Formula
Partial Pressure
Partial pressure is the pressure exerted by an individual gas in a mixture of gases. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each component. This concept is vital for determining the total pressure in the vessel after the diethyl ether has evaporated and contributed to the gas mixture.
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Percorso guidato
00:48Partial Pressure Calculation
Density and Mass Calculation
Density is defined as mass per unit volume and is used to convert between the volume of a substance and its mass. In this problem, the density of diethyl ether allows us to calculate the mass of the ether introduced into the vessel, which is necessary for determining the number of moles of gas produced upon evaporation.
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Percorso guidato
03:12Molar Mass Calculation Example
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Domanda del libro di testo
At an underwater depth of 250 ft, the pressure is 8.38 atm. What should the mole percent of oxygen be in the diving gas for the partial pressure of oxygen in the mixture to be 0.21 atm, the same as in air at 1 atm?