Multiple Choice
A gas bottle initially contains 0.800 mol of gas at a pressure of 730 mm Hg. If the final pressure is increased to 1.15 atm, how many moles of gas were added to the bottle, assuming constant temperature and volume?
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7. Gases
The Ideal Gas Law
Multiple Choice
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 0.80 atm and the temperature to 25 °C, assuming the amount of gas remains constant?
A
735 mL
B
900 mL
C
500 mL
D
1,200 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) = 0.80 atm, and final temperature (T2) = 25 °C.
Convert the temperatures from Celsius to Kelvin by adding 273.15 to each: 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: \( V_2 = \frac{1.20 \text{ atm} \cdot 735 \text{ mL} \cdot (25 + 273.15) \text{ K}}{0.80 \text{ atm} \cdot (112 + 273.15) \text{ K}} \).
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