Domanda del libro di testo
If 2.00 g of N2 gas has a volume of 0.40 L and a pressure of 6.0 atm, what is its Kelvin temperature?
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Ch.10 - Gases: Their Properties & Behavior
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 10, Problema 54
If 15.0 g of CO2 gas has a volume of 0.30 L at 300 K, what is its pressure in millimeters of mercury?
Guida verificata passo dopo passo1
Identify the ideal gas law equation: $PV = nRT$.
Calculate the number of moles of CO2 using its molar mass: \(n = \frac{\text{mass}}{\text{molar mass}}\).
Substitute the known values into the ideal gas law equation: \(P = \frac{nRT}{V}\).
Convert the pressure from atmospheres to millimeters of mercury using the conversion factor: \(1 \text{ atm} = 760 \text{ mmHg}\).
Solve for the pressure in millimeters of mercury.
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Ideal Gas Law
The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of a gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature in Kelvin. This law allows us to calculate one property of a gas if the others are known.
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Percorso guidato
01:15
Ideal Gas Law Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For carbon dioxide (CO2), the molar mass is approximately 44.01 g/mol, calculated from the atomic masses of carbon and oxygen. Knowing the molar mass is essential for converting between grams and moles, which is necessary for using the Ideal Gas Law.
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02:11Molar Mass Concept
Pressure Units
Pressure is a measure of force exerted per unit area and can be expressed in various units, including atmospheres (atm), pascals (Pa), and millimeters of mercury (mmHg). To convert between these units, it is important to know that 1 atm is equivalent to 760 mmHg. Understanding pressure units is crucial for accurately reporting and interpreting gas behavior in experiments.
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Percorso guidato
01:15Pressure Units
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