Multiple Choice
A cylinder contains 30.0 L of oxygen gas at a pressure of 1.9 atm and a temperature of 307 K. How many moles of gas are in the cylinder?
7. Gases
The Ideal Gas Law
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
A sample of argon gas has a volume of 0.240 L, a pressure of 0.900 atm, and a temperature of 27.0°C. At what temperature (°C) will the argon have a volume of 80.0 mL and a pressure of 3.20 atm?
A
150°C
B
273°C
C
327°C
D
100°C
Verified step by step guidance1
First, convert all given temperatures from degrees Celsius to Kelvin by adding 273.15. For the initial temperature, T1 = 27.0°C + 273.15 = 300.15 K.
Convert the final volume from milliliters to liters to maintain consistent units. V2 = 80.0 mL = 0.080 L.
Use the combined gas law, which is expressed as \( \frac{P_1 \cdot V_1}{T_1} = \frac{P_2 \cdot V_2}{T_2} \), where P is pressure, V is volume, and T is temperature in Kelvin.
Substitute the known values into the combined gas law equation: \( \frac{0.900 \cdot 0.240}{300.15} = \frac{3.20 \cdot 0.080}{T_2} \).
Solve for \( T_2 \) by rearranging the equation: \( T_2 = \frac{3.20 \cdot 0.080 \cdot 300.15}{0.900 \cdot 0.240} \). After finding \( T_2 \) in Kelvin, convert it back to degrees Celsius by subtracting 273.15.
Related Videos
Related Practice
The Ideal Gas Law practice set
Problem sets built by lead tutorsExpert video explanations