Open Question
Which assumptions of the kinetic–molecular theory explain the behavior of gases described by Charles's law? Explain your answer.
11 Gases
Chemistry Gas Laws
Struggling with Introduction to Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
A sealed container with a movable piston contains a gas with a pressure of 1380 torr, a volume of 820 mL and a temperature of 31°C. What would the volume be if the new pressure is now 2.83 atm, while the temperature decreased to 25°C?
A
0.0253 L
B
0.167 L
C
0.326 L
D
0.516 L
E
1.46 L
Verified step by step guidance1
First, convert all units to the appropriate SI units. Convert the initial pressure from torr to atm using the conversion factor: 1 atm = 760 torr. Use the formula: \( P_{\text{atm}} = \frac{P_{\text{torr}}}{760} \).
Convert the initial volume from mL to L using the conversion factor: 1 L = 1000 mL. Use the formula: \( V_{\text{L}} = \frac{V_{\text{mL}}}{1000} \).
Convert the temperatures from Celsius to Kelvin using the formula: \( T_{\text{K}} = T_{\text{°C}} + 273.15 \). Apply this to both the initial and final temperatures.
Use the combined gas law to find the new volume. The combined gas law is \( \frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2} \). Rearrange the formula to solve for \( V_2 \): \( V_2 = \frac{P_1 V_1 T_2}{P_2 T_1} \).
Substitute the converted values into the rearranged formula to calculate the new volume \( V_2 \).
Related Videos
Related Practice
Chemistry Gas Laws practice set
Problem sets built by lead tutorsExpert video explanations