Gas Laws #1
When considering the relationship between temperature and volume, what condition must be kept constant?
Pressure
Temperature is measured in
What is Kelvin?
Gay-Lussac's Law formula is ...
... P1/T1=P2/T2.
P1: 735 kPa
T1: 707.9 K
T2: 465.66 K
Wanted: P2 in kilopascals?
Correct answer is 483 kPa
What is the formula for Charles's Law?
V1/T1=V2/T2
What is the ideal gas law equation?
PV=nRT
The pressure in Gay-Lussac's Law increases when ...
... the temperature decreases.
T1: 432 K
T2: 404.2 K
V2: 7.58 L
Wanted: V1
Correct answer is 8.10 L
What is 25oC in Kelvin?
25+273 = 298K
What is the constant R?
8.31
A gas has a pressure of 0.875 atm at 35.0 °C(35+273=308K). What is the pressure at 545K?
The Law used is...
What is 1.56 atm?
Lussac’s Law
P1: 644 kPa
P2: 57.2 kPa
V1: 98.8 L
T1: 345 K
T2: 575 K
Correct answer is 1850 L
A gas has a volume of 300mL at 150oC. It is heated until it's volume is 600 mL. What is the new temperature of the gas if the pressure remains constant?
V1/T1=V2/T2
300mL/423K = 600mL/T2
T2 = 846K (or 800K in sf)
Double Jeopardy!
A gas has a volume of 3.5L at STP. How many moles of gas is this?
*STP=Pressure 1atm, temperature=273K
PV=nRT
(1)(3.5L)=(n)(.0821)(273K)
n = 0.16 mol
A gas with a pressure of 735 mmHg and a volume of 4L is allowed to expand to a volume of 12L. What is the pressure of the gas when the volume reaches 12L if the temperature remains constant?
P1V1=P2V2
(735mmHg)(4L) = (P2)(12L)
P2 = 245mmHg
Double Jeopardy!
P: 425.1 kPa
n: 2.83 mol
T: 394 K
Wanted: V in liters
Correct answer is 21.8 L
Boyle’s law, stated mathematically is P1V1 = P2V2. According to this law, what is the relationship between pressure and volume?
As the pressure increases, the volume decreases.
A sample of nitrogen is kept at a constant temperature of 300K. If the initial pressure is 4atm and the volume is 1.85L, what is the new volume if the pressure is changed to 1.6atm?
4.63L
A gas will increase in pressure inside a sealed container when heated. Which of the following is the best explanation for this in terms of kinetic molecular theory?
The particles gain more energy and therefore move faster, causing more collisions with the walls of the container.
P1: 531.56 kPa
P2: 253.37 kPa
V1: 18.6 L
T1: 429.99 K
T2: 539 K
Find V2
Correct answer is 48.9 L