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Ch.5 - Gases
All textbooksTro 4th EditionCh.5 - GasesProblem 47
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Chapter 5, Problem 47

A wine-dispensing system uses argon canisters to pressurize and preserve wine in the bottle. An argon canister for the system has a volume of 55.0 mL and contains 26.0 g of argon. When the argon is released from the canister, it expands to fill the wine bottle. How many 750.0-mL wine bottles can be purged with the argon in the canister at a pressure of 1.20 atm and a temperature of 295 K? Assuming ideal gas behavior, what is the pressure in the canister at 295 K?

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1
Calculate the number of moles of argon in the canister using the molar mass of argon (approximately 39.95 g/mol).
Use the ideal gas law equation \( PV = nRT \) to find the pressure in the canister. Here, \( P \) is the pressure, \( V \) is the volume of the canister, \( n \) is the number of moles calculated in the previous step, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), and \( T \) is the temperature in Kelvin.
Convert the volume of the canister from mL to L for consistency in units.
Calculate the total volume of argon gas at 1.20 atm and 295 K using the ideal gas law, rearranging it to solve for \( V \) (volume).
Determine how many 750.0-mL wine bottles can be filled by dividing the total volume of argon gas by the volume of one wine bottle (converted to liters).
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Which gas sample has the greatest pressure? Assume that all the samples are at the same temperature. Explain.

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Textbook Question

This picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 °C. Draw a similar picture showing what would happen to the sample if the volume were reduced to 0.5 L and the temperature were increased to 250 °C. What would happen to the pressure?

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