∙∙At an altitude of 11,000 m (a typical cruising altitude for a jet airliner), the air temperatu

step 1 at an altitude of 11 ,000 meter the density of air is 0 .364 kilogram per cubic meter and the te

∙∙At an altitude of 11,000 m (a typical cruising altitude...

$\bullet$$\bullet$ At an altitude of $11,000 \mathrm{m}$ (a typical cruising altitude for a jet airliner), the air temperature is $-56.5^{\circ} \mathrm{C}$ and the air density is 0.364 $\mathrm{kg} / \mathrm{m}^{3} .$ What is the pressure of the atmosphere at that altitude? The molar mass of air is 28.8 $\mathrm{g} / \mathrm{mol}$ .

$\bullet$$\bullet$ At an altitude of $11,000 \mathrm{m}$ (a typical cruising altitude for a
jet airliner), the air temperature is $-56.5^{\circ} \mathrm{C}$ and the air density is 0.364 $\mathrm{kg} / \mathrm{m}^{3} .$ What is the pressure of the atmosphere at that altitude? The molar mass of air is 28.8 $\mathrm{g} / \mathrm{mol}$ .

Key Concepts

Ideal Gas Law

The ideal gas law (PV = nRT) is a fundamental equation that relates the pressure, volume, the number of moles, the gas constant, and temperature of an ideal gas. It is used to calculate any one of these variables if the others are known, making it essential for determining atmospheric parameters like pressure when altitude and temperature data are provided.

Air Density

Air density is a measure of mass per unit volume for air and plays a crucial role in various atmospheric calculations. It is used in conjunction with the molar mass of air to determine the number of moles per unit volume, which is then applied in the ideal gas law to find the atmospheric pressure at different altitudes.

Temperature Conversion

Temperature conversion, specifically converting Celsius to Kelvin, is a key step in gas law calculations since the ideal gas law requires the absolute temperature in Kelvin. This conversion is essential for ensuring that the units are consistent and the calculations yield correct results.

Molar Mass

The molar mass of a substance is the mass of one mole of its particles and is used to convert between the mass (or density) of a gas and the number of moles. In the context of the atmospheric pressure calculation, the molar mass of air is used to transform air density into molar density, which is crucial for applying the ideal gas law.

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