Concept explainers
A mixture of gases contains 0.31 mol CH4, 0.25 mol C2H6, and 0.29 mol C3H8. The total pressure is 1.50 atm. Calculate the partial pressures of the gases.
Interpretation:
The partial pressures of the given gases have to be calculated.
Concept Introduction:
A mole fraction is the unit less proportion of the number of moles of a mixture constituent and the total number of moles in the mixture.
The number of molecules of gases is known. Since the mole fraction is:
- In a mixture of gases, every gas has an incomplete pressure which is the theoretical stress of that gas if it alone engaged the entire volume of the original combination at the same temperature.
- The sum pressure of an ideal gas mixture is the amount of the partial pressures of the gases in the mixture.
Answer to Problem 5.67QP
The partial pressure of
The partial pressure of
The partial pressure of
Explanation of Solution
First, we calculate the mole fraction Methane from the mixture. Then, we can calculate the partial pressure of each component.
The number of moles of the combined gases is:
The partial pressure of
The partial pressure of
Second, we calculate the mole fraction Ethane from the mixture. Then, we can calculate the partial pressure of each component.
The partial pressure of
The partial pressure of
Third, we calculate the mole fraction Propane from the mixture. Then, we can calculate the partial pressure of each component.
The partial pressure of
The partial pressure of
The partial pressures of the given gases were calculated.
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Chapter 5 Solutions
AVC LOOSELEAF CHEMISTRY W/CONNECT 2 SEM
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