The chemical composition of air that is exhaled (expired) is different from ordinary air. A typical analysis of expired air at 37 °C and 1.00 atm, expressed as percent by volume, is 74.2% N 2 .15.2% O 2 , 3.8% CO 2 , 5.9% H 2 O, and 0.9% Ar. The composition of ordinary air is given practice Example 6-12B. a. What is the ratio of the partial pressure of CO 2 (g)in expired air to that in ordinary air? b. Would you expect the density of expired air to greater or less than that of ordinary air at the same temperature and pressure? Explain. c. Confirm your expectation by calculating the densities of ordinary air and expired air at 37 °C and 1.00 atm.
The chemical composition of air that is exhaled (expired) is different from ordinary air. A typical analysis of expired air at 37 °C and 1.00 atm, expressed as percent by volume, is 74.2% N 2 .15.2% O 2 , 3.8% CO 2 , 5.9% H 2 O, and 0.9% Ar. The composition of ordinary air is given practice Example 6-12B. a. What is the ratio of the partial pressure of CO 2 (g)in expired air to that in ordinary air? b. Would you expect the density of expired air to greater or less than that of ordinary air at the same temperature and pressure? Explain. c. Confirm your expectation by calculating the densities of ordinary air and expired air at 37 °C and 1.00 atm.
Solution Summary: The author explains that the ratio of partial pressure of CO 2 (g) in expired air to that in ordinary air should be calculated.
The chemical composition of air that is exhaled (expired) is different from ordinary air. A typical analysis of expired air at 37 °C and 1.00 atm, expressed as percent by volume, is 74.2% N2.15.2% O2, 3.8% CO2, 5.9% H2O, and 0.9% Ar. The composition of ordinary air is given practice Example 6-12B. a. What is the ratio of the partial pressure of CO2(g)in expired air to that in ordinary air? b. Would you expect the density of expired air to greater or less than that of ordinary air at the same temperature and pressure? Explain. c. Confirm your expectation by calculating the densities of ordinary air and expired air at 37 °C and 1.00 atm.
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A gas mixture was prepared to contain 50% by mass of O₂ and Ne.
When the total pressure of the mixture is 1.50 atm, what is the partial
pressure of O₂?
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Question 29 of 30
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The ideal gas law describes the relationship among
the volume of an ideal gas (V), its pressure (P), its
absolute temperature (T), and number of moles (
n):
PV = nRT
Under standard conditions, the ideal gas law does
a good job of approximating these properties for
any gas. However, the ideal gas law does not
account for all the properties of real gases such as
intermolecular attraction and molecular volume,
which become more pronounced at low
temperatures and high pressures. The van der
Waals equation corrects for these factors with the
constants a and b, which are unique to each
substance:
(P+ ²) (V-nb) = nRT
an²
The gas constant R is equal to 0.08206
L.atm/(K-mol).
Part A
A 3.00-L flask is filled with gaseous ammonia, NH3. The gas pressure measured at 16.0 °C is 2.45 atm . Assuming
ideal gas behavior, how many grams of ammonia are in the flask?
Express your answer to three significant figures and include the appropriate units.
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mass of NH3 =
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▾ Part B
HÅ…
Stoichiometry with Partial Pressure
Gas jar
Gas collects
here
Trough of
water
Bee hive
shelf
Reaction
mixture
2 KCIO,
3(s)
+
> 2 KCI
(s),
30
2(g)
A sample of KCIO3 is partially decomposed by heating, producing O2 gas that is collected
safely over water. The volume of total gas collected is 2.50 x 10-4 m³ at 26 °C, giving 101.99
kPa total pressure. How many grams of KCIO3 were decomposed? What atom was
oxidized? What atom was reduced? The pressure of water vapor at 26 °C is 25 torr.
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Chapter 6 Solutions
General Chemistry: Principles And Modern Applications Plus Mastering Chemistry With Pearson Etext -- Access Card Package (11th Edition)
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