Gas Laws Test Flashcards
Charles law
V1/T1 = V2/T2
Gay-lussac’s law
P1/T1 = P2/T2
Combined gas law
P1V1/T1 = P2V2/T2
According to gay-lussac’s law, at constant volume, as the temperature increases, the pressure always ___________.
Increases
According to Boyle’s law, at constant temperature, as the volume increases, the pressure always ____________.
Decreases
According to Charles’ law, at constant pressure, as the temperature increases, the volume always __________.
Increases
At constant temperature, the volume of a gas expands from 10 L to 23 L. If the initial pressure was 103.72 kPa, what is the final pressure?
45.1 kPa
The volume of a gas was originally 3.6 L; it’s pressure was 116 kPa and its temperature was 293 K. The volume of the gas expanded to 7.2 L and it’s pressure decreased to 102 kPa. What is the temperature of the gas?
513.3 K
At constant pressure, a gas is heated from 200 K to 400K. After heating, the volume of the gas was 10 L. What was the initial volume of the gas?
5 L
What is the molar mass of a gas at 20 degrees C with a volume of 5.6 L and a pressure of 115 kPa if there are 17 grams of it?
64.3 g/mol
Oxygen gas has a pressure of 315 kPa in a container of 53 L and a temperature of 6 degrees C. What is the mass of the gas?
230.3 g
What is STP?
101.325 kPa, 273 K
A quantity of oxygen gas was collected over water at 10 degrees C in a 6.75 ml container. The pressure in the container was measured to be 95 kPa. How many grams of oxygen gas were collected?
0.0086 g
Oxygen gas was collected over water at 25 degrees C. The pressure in the 3.1 L container was 121 kPa. If the container was allowed to expand to 9.3 L and if the temperature was decreased to -25 degrees C, what is the final pressure of the dry oxygen gas?
32.7 kPa
How is vaporization of water affected by temperature?
As the temperature increases, the vaporization of water increases
Nitrogen gas can be produced by reacting Na3N with chlorine gas. If the reaction was carried out at STP with 34.8 g of Na3N, what volume of nitrogen gas can be produced? (List steps)
1) balanced equation
2) MPV=mRT to find moles Na3N
3) convert
Answer: 4.7 L N2
How many grams of sodium are required to produce 31.9 L of H2 at 97 kPa and 290 K according to the following balanced equation?
2HNO3 + 2Na –> 2NaNO3 + H2
(List steps)
1) PV=nRT to find moles
2) change moles of H2 from PV=nRT to mol of Na
3) convert mol to g
58.9 g Na
Boyles law
(P1)(V1) = (P2)(V2)
