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Ch.5 - Gases
Tro - Chemistry: A Molecular Approach 4th Edition
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Tutti i libri di testoTro 4th EditionCh.5 - GasesProblema 54
Capitolo 5, Problema 54

Use the molar volume of a gas at STP to calculate the density (in g/L) of nitrogen gas at STP.

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Identify the molar volume of a gas at STP, which is 22.4 L/mol.
Determine the molar mass of nitrogen gas (N₂). Since nitrogen has an atomic mass of approximately 14.01 g/mol, the molar mass of N₂ is 2 x 14.01 g/mol.
Use the formula for density: \( \text{Density} = \frac{\text{Mass}}{\text{Volume}} \).
Substitute the molar mass of nitrogen gas for the mass and the molar volume for the volume in the density formula.
Calculate the density of nitrogen gas at STP using the values obtained in the previous steps.

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Molar Volume of a Gas

The molar volume of a gas at standard temperature and pressure (STP) is the volume occupied by one mole of an ideal gas, which is approximately 22.4 liters. This value is crucial for calculations involving gases, as it allows for the conversion between moles and volume, facilitating the determination of properties like density.
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The Ideal Gas Law: Molar Mass

Density of a Gas

Density is defined as mass per unit volume, typically expressed in grams per liter (g/L) for gases. To calculate the density of nitrogen gas at STP, one must use the mass of one mole of nitrogen (approximately 28 grams) and divide it by the molar volume (22.4 L), resulting in a density value that reflects how compact the gas is under standard conditions.
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Gas Density Example

Standard Temperature and Pressure (STP)

STP refers to a standard set of conditions for measuring gases, defined as 0 degrees Celsius (273.15 K) and 1 atmosphere of pressure. These conditions are essential for consistent calculations in gas laws and properties, ensuring that comparisons and calculations involving gases are reliable and standardized across different scenarios.
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Standard Temperature and Pressure
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