A wine-dispensing system uses argon canisters to pressurize and preserve wine in the bottle.

1. An argon canister for the system has a volume of 55.0 mL and contains 26.0 g of argon. Assuming ideal gas behavior, what is the pressure (in atm) in the canister at 22.0°C?

Pressure of canister:

2. 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 22.0°C?

Wine bottle count:

According to the ideal gas law, PV = nRT, pressure, volume, number of moles, and temperature are related to each other by the ideal gas constant (R). P = nRT/V, where n is the number of moles, R is the ideal gas constant, T is the temperature in Kelvin, and V is the volume. Let us first convert the volume of the canister from milliliters (mL) to liters (L):55.0 mL × (1 L/1000 mL) = 0.0550 L

Next, we need to calculate the number of moles of argon in the canister. We can use the molar mass of argon to convert from grams to moles:26.0 g Ar × (1 mol Ar/39.95 g Ar)

= 0.651 mol Ar Now we can use the ideal gas law to solve for pressure:P

= nRT/V

= (0.651 mol)(0.0821 L atm/mol K)(295 K)/(0.0550 L)

≈ 2.81 atm

Let's first convert the volume of a wine bottle from milliliters (mL) to liters (L):750.0 mL × (1 L/1000 mL) = 0.7500 LNext, let's convert the temperature to Kelvin:22.0°C + 273

= 295 KNow we can solve for the number of moles of argon required to fill a wine bottle at 1.20 atm and 295 K:P

= nRT/Vn

= PV/RT

= (1.20 atm)(0.7500 L)/(0.0821 L atm/mol K)(295 K)

≈ 0.0368 mol Ar Finally, we can use the number of moles in the canister to determine the maximum number of bottles that can be purged:n

= 0.651 mol Ar × (1 bottle/0.0368 mol Ar)

≈ 17.7 bottles (rounded down to the nearest whole number) Pressure of canister:

≈ 2.81 atm; Wine bottle count: 17

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