Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a gas at the pressure shown. What is the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant? (We can neglect the volume of the capillary tubing connecting the bulbs.)
Ch.10 - Gases
Chapter 10, Problem 107c
Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (c) How many grams of glucose (C6H12O6) would need to be metabolized to produce this quantity of CO2? (The chemical reaction is the same as that for combustion of C6H12O6. See Section 3.2 and Problem 10.57.)

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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows us to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. In this context, understanding stoichiometry is essential to determine how many grams of glucose are needed to produce a specific amount of carbon dioxide.
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Combustion of Glucose
The combustion of glucose (C6H12O6) is a biochemical process where glucose reacts with oxygen to produce carbon dioxide and water, releasing energy. The balanced equation for this reaction is C6H12O6 + 6 O2 → 6 CO2 + 6 H2O. Knowing this reaction is crucial for calculating the amount of glucose required to generate a given quantity of CO2, as it directly relates the moles of glucose to the moles of CO2 produced.
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Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between the mass of a substance and the number of moles, which is necessary for stoichiometric calculations. In this problem, calculating the molar mass of glucose will enable us to convert the moles of glucose needed to produce the specified amount of CO2 into grams.
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Related Practice
Textbook Question
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Textbook Question
Assume that a single cylinder of an automobile engine has a volume of 524 cm3. (a) If the cylinder is full of air at 74 C and 99.3 kPa, how many moles of O2 are present? (The mole fraction of O2 in dry air is 0.2095.) (b) How many grams of C8H18 could be combusted by this quantity of O2, assuming complete combustion with formation of CO2 and H2O?
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Textbook Question
Assume that an exhaled breath of air consists of 74.8% N2, 15.3% O2, 3.7% CO2, and 6.2% water vapor. (a) If the total pressure of the gases is 99.8 kPa, calculate the partial pressure of water vapor.
999
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Textbook Question
An 8.40-g sample of argon and an unknown mass of H2
are mixed in a flask at room temperature. The partial pressure
of the argon is 44.0 kPa, and that of the hydrogen is
57.33 kPa. What is the mass of the hydrogen?
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Textbook Question
An ideal gas at a pressure of 152 kPa is contained in a bulb
of unknown volume. A stopcock is used to connect this
bulb with a previously evacuated bulb that has a volume
of 0.800 L as shown here. When the stopcock is opened,
the gas expands into the empty bulb. If the temperature
is held constant during this process and the final pressure
is 92.66 kPa, what is the volume of the bulb that was
originally filled with gas?
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Textbook Question
The density of a gas of unknown molar mass was measured as a function of pressure at 0 C, as in the table that follows. (a) Determine a precise molar mass for the gas. [Hint: Graph d>P versus P.]
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