Are you more likely to see the density of a gas reported in g/mL, g/L, or kg/cm³?

Verified step by step guidance

Understand the concept of density: Density is defined as mass per unit volume. In chemistry, it is often used to describe how much mass is contained in a given volume of a substance.

Consider the typical units used for gases: Gases are usually measured in terms of volume in liters (L) because they occupy larger spaces compared to solids and liquids. Therefore, density for gases is often reported in grams per liter (g/L).

Evaluate the practicality of other units: While g/mL is a common unit for liquids and solids, it is less practical for gases because gases occupy larger volumes. Similarly, kg/cm³ is not commonly used for gases as it is more suited for very dense materials.

Recognize the standard reporting practice: In scientific literature and textbooks, the density of gases is most commonly reported in g/L due to the convenience of measuring gas volumes in liters.

Conclude with the most likely unit: Based on the above considerations, the density of a gas is most likely to be reported in g/L.

Key Concepts

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

Density

Density is defined as mass per unit volume and is a critical property of substances. It is typically expressed in units such as grams per milliliter (g/mL), grams per liter (g/L), or kilograms per cubic centimeter (kg/cm³). Understanding density helps in comparing the compactness of different materials and is essential in various applications, including gas behavior and buoyancy.

Units of Measurement

Different units of measurement are used to express density depending on the state of matter and the context. For gases, density is most commonly reported in grams per liter (g/L) because gases occupy much larger volumes compared to solids and liquids. This unit is more practical for expressing the low mass of gases in relation to their volume.

Gas Behavior

Gases exhibit unique behaviors that differ from solids and liquids, primarily due to their low density and high compressibility. The density of a gas can change significantly with temperature and pressure, which is described by the Ideal Gas Law. Understanding these properties is essential for accurately reporting and interpreting gas densities in scientific contexts.

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Ideal Gas Law Formula

Related Practice

Textbook Question

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (a) At room temperature, all three real gases have a pressure less than the ideal gas. Which van der Waals constant, a or b, accounts for the influence intermolecular forces have in lowering the pressure of a real gas?

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Textbook Question

The graph below shows the change in pressure as the temperature increases for a 1-mol sample of a gas confined to a 1-L container. The four plots correspond to an ideal gas and three real gases: CO2, N2, and Cl2. (b) Use the van der Waals constants in Table 10.3 to match the labels in the plot (A, B, and C) with the respective gases 1CO2, N2, and Cl22.

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Textbook Question

Which of the following statements is false? (a) Gases are far less dense than liquids. (b) Gases are far more compressible than liquids. (c) Because liquid water and liquid carbon tetrachloride do not mix, neither do their vapors. (d) The volume occupied by a gas is determined by the volume of its container.

(b) Which units are appropriate for expressing atmospheric pressures, N, Pa, atm, kg/m²?

A person weighing 75 kg is standing on a threelegged stool. The stool momentarily tilts so that the entire weight is on one foot. If the contact area of each foot is 5.0 cm2, calculate the pressure exerted on the underlying surface in (a) bars

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