Domanda del libro di testo
(b) What is the molar volume of an ideal gas at STP?
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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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 10, Problema 31
Suppose you are given two 1-L flasks and told that one contains a gas of molar mass 30 and the other a gas of molar mass 60, both at the same temperature. The pressure in flask A is x atm, and the mass of gas in the flask is 1.2 g. The pressure in flask B is 0.5x atm, and the mass of gas in that flask is 1.2 g. Which flask contains the gas of molar mass 30, and which contains the gas of molar mass 60?
Guida verificata passo dopo passo1
Calculate the number of moles of gas in each flask using the formula: number of moles (n) = mass (g) / molar mass (g/mol).
Apply the Ideal Gas Law, PV = nRT, to each flask to find the relationship between the pressure and the number of moles. Since the volume (V) and temperature (T) are constant and the same for both flasks, and R is a constant, focus on how P varies with n.
For Flask A, substitute the calculated moles from step 1 into the Ideal Gas Law rearranged as P = (nRT)/V, and note that R, T, and V are constants.
Repeat step 3 for Flask B, using the moles calculated for Flask B and noting that the pressure is 0.5x atm.
Compare the calculated pressures relative to the moles of gas in each flask to determine which flask must contain the gas with the molar mass of 30 g/mol and which contains the gas with the molar mass of 60 g/mol.
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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 allows us to understand how gases behave under different conditions and is essential for solving problems involving gas properties, such as pressure and molar mass.
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Percorso guidato
01:15
Ideal Gas Law Formula
Molar Mass and Density
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). The density of a gas can be calculated using its molar mass and the Ideal Gas Law, which helps in determining the relationship between mass, volume, and pressure of gases in different flasks.
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Percorso guidato
02:11Molar Mass Concept
Relationship Between Pressure and Molar Mass
For gases at the same temperature and volume, the pressure is inversely related to the molar mass when the mass of the gas is constant. This means that a gas with a lower molar mass will exert a higher pressure compared to a gas with a higher molar mass, allowing us to deduce which flask contains which gas based on their pressures.
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Percorso guidato
02:11Molar Mass Concept
Pratica correlata
Domanda del libro di testo
Complete the following table for an ideal gas:
Domanda del libro di testo
Suppose you are given two flasks at the same temperature, one of volume 2 L and the other of volume 3 L. The 2-L flask contains 4.8 g of gas, and the gas pressure is x atm. The 3-L flask contains 0.36 g of gas, and the gas pressure is 0.1x. Do the two gases have the same molar mass? If not, which contains the gas of higher molar mass?
Domanda del libro di testo
(d) If you measure pressure in bars instead of atmospheres, calculate the corresponding value of R in L-bar/mol-K.
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