Textbook Question
(a) What are the mole fractions of O2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
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Ch.10 - Gases
Chapter 10, Problem 72b
(b) What is the partial pressure in atm of each component of this mixture if its held in a 15.50-L vessel at 15 °C?
Verified step by step guidance1
Identify the components of the gas mixture and their respective amounts (in moles) if given, or determine them from additional information provided in the problem.
Convert the temperature from degrees Celsius to Kelvin by adding 273.15 to the Celsius temperature. This is necessary because gas law calculations require temperature in Kelvin.
Use the ideal gas law, PV = nRT, to calculate the total pressure of the gas mixture. Here, P is the total pressure, V is the volume of the container (15.50 L), n is the total number of moles of gas, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.
Determine the mole fraction of each component in the mixture. The mole fraction is calculated by dividing the number of moles of a particular gas by the total number of moles of all gases in the mixture.
Calculate the partial pressure of each component by multiplying its mole fraction by the total pressure of the gas mixture. This is based on Dalton's Law of Partial Pressures, which states that the partial pressure of a gas in a mixture is equal to the mole fraction of that gas times the total pressure.
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Related Practice
Textbook Question
(a) What are the mole fractions of N2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
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Textbook Question
(a) What are the mole fractions of H2 in a mixture of 15.08 g of O2, 8.17 g of N2, and 2.64 g of H2?
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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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Textbook Question
A sample of 3.00 g of SO2(g) originally in a 5.00-L vessel at 21 °C is transferred to a 10.0-L vessel at 26 °C. A sample of 2.35 g of N2(g) originally in a 2.50-L vessel at 20 °C is transferred to this same 10.0-L vessel. (a) What is the partial pressure of SO2(g) in the larger container? (b) What is the partial pressure of N2(g) in this vessel?
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Textbook Question
A sample of 3.00 g of SO2(g) originally in a 5.00-L vessel at 21 °C is transferred to a 10.0-L vessel at 26 °C. A sample of 2.35 g of N2(g) originally in a 2.50-L vessel at 20 °C is transferred to this same 10.0-L vessel. (c) What is the total pressure in the vessel?