Use the molar volume of a gas at STP to calculate the density (in g/L) of carbon dioxide 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 carbon dioxide (CO_2). Carbon has a molar mass of 12.01 g/mol and oxygen has a molar mass of 16.00 g/mol. Therefore, CO_2 has a molar mass of 12.01 + 2(16.00) g/mol.

Use the formula for density: \( \text{Density} = \frac{\text{Mass}}{\text{Volume}} \).

Substitute the molar mass of CO_2 for the mass and the molar volume (22.4 L) for the volume in the density formula.

Calculate the density of CO_2 in g/L by dividing the molar mass by the molar volume.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 various properties such as density.

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 a gas, one can use the formula: density = mass/volume. Understanding how to derive the mass of carbon dioxide from its molar mass and the volume it occupies at STP is essential for this calculation.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) refers to a set of conditions commonly used in gas calculations, defined as 0 degrees Celsius (273.15 K) and 1 atmosphere of pressure. At STP, the behavior of gases can be predicted using the ideal gas law, and it provides a reference point for comparing gas properties, including density and molar volume.

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