At 273 K and 1 atm pressure, 1 mol of an ideal gas occupies 22.4 L. (Section 10.4) (b) Looking at Figure 18.1, we see that the temperature is lower at 85 km altitude than at 50 km. Does this mean that one mole of an ideal gas would occupy less volume at 85 km than at 50 km? Explain.

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Identify the relationship between temperature, pressure, and volume for an ideal gas using the Ideal Gas Law: \( PV = nRT \).

Recognize that at a constant pressure, the volume of a gas is directly proportional to its temperature (Charles's Law): \( V \propto T \).

Understand that if the temperature decreases, the volume of the gas will also decrease, assuming pressure remains constant.

Consider the information given: the temperature is lower at 85 km altitude than at 50 km altitude.

Conclude that, under the assumption of constant pressure, one mole of an ideal gas would occupy less volume at 85 km than at 50 km due to the lower temperature.

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Key Concepts

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

Ideal Gas Law

The Ideal Gas Law, represented as PV=nRT, describes the relationship between pressure (P), volume (V), temperature (T), and the number of moles (n) of an ideal gas. It states that for a given amount of gas at a constant pressure, the volume is directly proportional to the temperature. This law is fundamental in understanding how changes in temperature and pressure affect the volume of a gas.

Effect of Temperature on Gas Volume

According to the Ideal Gas Law, as temperature decreases, the volume of an ideal gas also decreases if pressure remains constant. This is because lower temperatures result in lower kinetic energy of gas molecules, leading to a reduction in the space they occupy. Therefore, at higher altitudes where temperatures are lower, one mole of an ideal gas would occupy less volume compared to lower altitudes.

Altitude and Atmospheric Pressure

As altitude increases, atmospheric pressure decreases. This reduction in pressure can influence the behavior of gases, but in the context of the question, the primary factor is the temperature difference at varying altitudes. At 85 km, the lower temperature contributes more significantly to the volume change of the gas than the decrease in pressure, leading to a smaller volume for the gas at that altitude.