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Ch.6 - Gases
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 6th EditionCh.6 - GasesProblema 72
Capitolo 6, Problema 72

A 275-mL flask contains pure helium at a pressure of 752 torr. A second flask with a volume of 475 mL contains pure argon at a pressure of 722 torr. If we connect the two flasks through a stopcock and we open the stopcock, what is the partial pressure of argon?

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Convert the pressure of argon from torr to atm if necessary, using the conversion factor: 1 atm = 760 torr.
Calculate the initial moles of argon using the ideal gas law: \( PV = nRT \), where \( P \) is the pressure, \( V \) is the volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is the temperature in Kelvin. Assume the temperature is constant and the same for both gases.
Determine the total volume after the stopcock is opened by adding the volumes of the two flasks: \( V_{\text{total}} = V_{\text{flask 1}} + V_{\text{flask 2}} \).
Use the ideal gas law again to find the new partial pressure of argon after the stopcock is opened, using the total volume and the initial moles of argon calculated earlier.
The partial pressure of argon is the pressure exerted by argon alone in the combined volume, calculated using the formula: \( P_{\text{argon}} = \frac{nRT}{V_{\text{total}}} \).

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Dalton's Law of Partial Pressures

Dalton's Law states that in a mixture of gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle allows us to calculate the pressure of a specific gas in a mixture by considering its contribution to the total pressure, which is essential for solving problems involving multiple gases.
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Gas Laws and Volume Relationships

Understanding the relationships between pressure, volume, and temperature of gases is crucial. According to Boyle's Law, for a given amount of gas at constant temperature, the pressure of a gas is inversely proportional to its volume. This concept helps in determining how the pressures of gases change when they are allowed to mix in different volumes.
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Ideal Gas Behavior

The ideal gas law (PV=nRT) describes the behavior of an ideal gas, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. While real gases may deviate from this behavior under certain conditions, the ideal gas law provides a foundational understanding for calculating pressures and volumes in gas mixtures, which is relevant for this question.
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