Concept explainers
Atop Mt. Everest, the atmospheric pressure is 210 mmHg and the air density is 0.426 kg/m3. (a) Calculate the air temperature, given that the molar mass of air is 29.0 g/mol. (b) Assuming no change in air composition, calculate the percent decrease in oxygen gas from sea level to the top of Mt. Everest.
(a)
Interpretation:
The air temperature and the percent decrease in oxygen gas from sea level have to be calculated.
Concept Introduction:
Ideal gas is the most usually used form of the ideal gas equation, which describes the relationship among the four variables P, V, n, and T. An ideal gas is a hypothetical sample of gas whose pressure-volume-temperature behavior is predicted accurately by the ideal gas equation.
Mt. Everest to the moles of
Answer to Problem 5.133QP
The air temperature
Explanation of Solution
To convert density to units of g/L
Let’s assume a volume of 1.00 L of air. This air sample will have a mass of 0.426 g.
We can substitute into the ideal gas equation to calculate the air temperature.
Theair temperature iscalculated by plugging in the values the moles of air, volume and pressure. The air temperature was found to be
(b)
Interpretation:
The air temperature and the percent decrease in oxygen gas from sea level have to be calculated.
Concept Introduction:
Ideal gas is the most usually used form of the ideal gas equation, which describes the relationship among the four variables P, V, n, and T. An ideal gas is a hypothetical sample of gas whose pressure-volume-temperature behavior is predicted accurately by the ideal gas equation.
Mt. Everest to the moles of
Answer to Problem 5.133QP
As a result, the percent decrease in oxygen gas from sea level to the top of Mt. Everest is
Explanation of Solution
In order to determine the percent decrease in oxygen gas, let’s compare moles of
The above calculation shows that there is only
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Chapter 5 Solutions
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