Multiple Choice
A 75.0 g sample of dinitrogen monoxide (N2O) is confined in a 4.12 L vessel. What is the pressure (in atm) at 205°F, assuming ideal gas behavior?
7. Gases
The Ideal Gas Law Applications
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A sample of argon gas has a volume of 735 mL at a pressure of 1.20 atm and a temperature of 112°C. What is the final volume of the gas, in milliliters, when the pressure is changed to 0.85 atm and the temperature is changed to 25°C, assuming the amount of gas remains constant?
A
1200 mL
B
950 mL
C
1020 mL
D
850 mL
Verified step by step guidance1
Identify the initial and final conditions of the gas: Initial volume (V1) = 735 mL, initial pressure (P1) = 1.20 atm, initial temperature (T1) = 112°C, final pressure (P2) = 0.85 atm, and final temperature (T2) = 25°C.
Convert the temperatures from Celsius to Kelvin by adding 273.15 to each temperature. T1 = 112 + 273.15 K and T2 = 25 + 273.15 K.
Use the combined gas law, which is \( \frac{P_1 \cdot V_1}{T_1} = \frac{P_2 \cdot V_2}{T_2} \), to relate the initial and final states of the gas.
Rearrange the combined gas law to solve for the final volume (V2): \( V_2 = \frac{P_1 \cdot V_1 \cdot T_2}{P_2 \cdot T_1} \).
Substitute the known values into the equation and solve for V2 to find the final volume of the gas in milliliters.
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