Textbook Question
The atmospheric concentration of CO2 gas is presently 407 ppm (parts per million, by volume; that is, 407 L of every 106 L of the atmosphere are CO2). What is the mole fraction of CO2 in the atmosphere?.
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Ch.10 - Gases
Chapter 10, Problem 68
A sample of 5.00 mL of diethylether 1C2H5OC2H5, density = 0.7134 g>mL2 is introduced into a 6.00-L vessel that already contains a mixture of N2 and O2, whose partial pressures are PN2 = 21.08 kPa and PO2 = 76.1 kPa. The temperature is held at 35.0 °C, and the diethylether totally evaporates. (b) Calculate the total pressure in the container.
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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 relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. This law is essential for understanding how gases behave under varying conditions and is crucial for calculating the total pressure in a container when new gases are introduced.
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01:15
Ideal Gas Law Formula
Partial Pressure
Partial pressure is the pressure exerted by an individual gas in a mixture of gases. According to Dalton's Law, the total pressure of a gas mixture is the sum of the partial pressures of each component. This concept is vital for determining the contribution of diethylether to the overall pressure in the vessel after it evaporates.
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00:48Partial Pressure Calculation
Density and Molar Mass
Density is defined as mass per unit volume and is crucial for converting the volume of a liquid into mass. Molar mass, the mass of one mole of a substance, allows for the calculation of the number of moles present. In this problem, the density of diethylether is used to find its mass, which is then converted to moles to apply the Ideal Gas Law.
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Related Practice
Textbook Question
A plasma-screen TV contains thousands of tiny cells filled
with a mixture of Xe, Ne, and He gases that emits light of
specific wavelengths when a voltage is applied. A particular
plasma cell, 0.900 mm * 0.300 mm * 10.0 mm, contains
4% Xe in a 1:1 Ne:He mixture at a total pressure of 66.66 kPa.
Calculate the number of Ne atoms in the cell and
state the assumptions you need to make in your calculation.
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Textbook Question
A piece of dry ice (solid carbon dioxide) with a mass of 20.0 g is
placed in a 25.0-L vessel that already contains air at 50.66 kPa
and 25 °C. After the carbon dioxide has totally sublimed, what
is the partial pressure of the resultant CO2 gas, and the total
pressure in the container at 25 °C?
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Textbook Question
A rigid vessel containing a 3:1 mol ratio of carbon dioxide
and water vapor is held at 200 °C where it has a total pressure
of 202.7 kPa. If the vessel is cooled to 10 °C so that all of the
water vapor condenses, what is the pressure of carbon dioxide?
Neglect the volume of the liquid water that forms on cooling.
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Textbook Question
At an underwater depth of 100 m, the pressure is 1.106 MPa.
What should the partial pressure of oxygen be in the diving
gas for the mole fraction of oxygen in the mixture to be 0.21,
the same as in air?
1268
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Textbook Question
A quantity of N2 gas originally held at 531.96 kPa pressure
in a 1.00-L container at 26 °C is transferred to a 12.5-L container
at 20 °C. A quantity of O2 gas originally at 531.96 kPa
and 26 °C in a 5.00-L container is transferred to this same
container. What is the total pressure in the new container?
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