Multiple Choice
A large balloon is initially filled to a volume of 25.0 L at 353 K and a pressure of 2575 mm Hg. What volume of gas will the balloon contain at 1.35 atm and 253 K, assuming ideal gas behavior?
7. Gases
The Ideal Gas Law
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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
950 mL
B
650 mL
C
800 mL
D
1100 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 expressed as (P1 * V1) / T1 = (P2 * V2) / T2, to relate the initial and final states of the gas.
Rearrange the combined gas law equation to solve for the final volume (V2): V2 = (P1 * V1 * T2) / (P2 * T1).
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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