Gas Law Concepts
Each of the flasks in contains the same number of gas molecules at the same volume
In which would the pressure be lowest?
https://docs.google.com/document/d/152oXevv4KMcCBcDOhA6wBIAxa16cvJtAkv-gKk6jWx4/edit
Flask 2
If a nitrogen gas occupies has a volume of 600. mL at a pressure of 1.00 atm. What volume
will the gas occupy at a pressure of 1.50 atm, assuming the temperature remains constant?
400. mL
P1V1=P2V2
A gas is at 27oC and the temperature is doubled. What is the new temperature in Celsius?
327oC
Standard temperature is _________ oC and standard pressure is _________ torr or_________ atm.
0 , 760 , 1
Which of these gases is LEAST ideal
CO2, NH3, H2, He
NH3
the hydrogen bonding causes more IMF's
(H2 is most ideal)
Each of the above flasks contains the same number of molecules at the same temperature.
In which container is the pressure highest?
https://docs.google.com/document/d/1451gYjpKtQzXjY0n6Q5K9KzWKj-pQMj4E63gEPWEtpg/edit
Flask 1
In a closed container at 1.00 atmosphere, the temperature of a sample of gas is raised from 400. K to 500. K. What is the new pressure after the container heats up?
1.25 atm
Temperature is the measure of...
average kinetic energy
____________ is caused by the force of gas particles hitting the walls of the container.
Pressure
Which of these gases is MOST ideal
H2, N2, F2, Cl2
H2
(Cl2 is least ideal with more LDF)
Helium and Argon are at the same temperature. Helium has ______ average kinetic energy as argon
a) the same
b) a higher
c) a lower
a
At constant pressure and 25 °C a sample of gas occupies 9.00 liters. At what temperature in Celsius will the gas occupy 4.50liters?
-124oC
How would the Maxwell Boltzmann distribution change with an increase of temperature. Be specific
https://images.deepai.org/django-summernote/2019-04-26/ba959845-f889-445a-9d7b-12314b2ee434.png
The graph would shift right AND have a lower peak
A mixture of unknown gases, A and B have partial pressure of PA = 0.35 atm and PB = 0.45 atm. If the gas mixture is at 256 K in a 1.1 L container how many total moles of gas are present?
.042 moles
Need to use PV=nRT
Which of these conditions is MOST ideal for a gas
a) 500 K, 1 atm
b) 50 K, 100 atm
c) 500 K, 100 atm
d) 50 K, 1 atm
a
1) Which gas law keeps pressure constant while comparing volume and temperature?
2) Which gas law keeps temperature constant while comparing pressure and volume?
1) Charles'
2) Boyle's
GAY-LUSSAC'S keeps volume constant
If 35.0 g nitrogen is placed into a container at STP, what is the volume of the gas?
28.0 L
The following Maxwell Boltzmann Distribution shows neon at 300 K. How would the graph of Oxygen at 300 K compare? Be specific
https://images.deepai.org/django-summernote/2019-04-26/ba959845-f889-445a-9d7b-12314b2ee434.png
Oxygen is O2 so the more massive gas would shift left AND have a higher peak
A mixture of 4.5% H2, 76% O2, and 19.5% N2 has a total pressure of 2.3 atm. What is the partial pressure of each of the gases?
0.10 atm H2 , 1.7 atm O2 , 0.45 atm N2
Which of these conditions is LEAST ideal for a gas
a) 500 K, 1 atm
b) 50 K, 100 atm
c) 500 K, 100 atm
d) 50 K, 1 atm
b
A gas has a pressure of 500. mmHg. If you double the volume and triple the temperature of a gas, what is the new pressure?
750 mmHg
If I have 0.40 moles of a gas at a pressure of 560 torr and a volume of 12 liters, what is the temperature in Celsius?
-4oC (sig figs are REALLY weird here...sorry)
The following Maxwell Boltzmann Distribution shows Argon at 500 K. How would the graph of Krypton at 500 K compare?
https://myalevels.co.uk/wp-content/uploads/2018/04/mbgraph.png
Same - This graph shows Kinetic Energy as the x-axis. Since same temperature, they will have the same average kinetic energy
A 2.5 L sample at 273 K contains 0.006 mol H2, 0.0024 mol O2, and 0.0002 mol CH4. What is the partial pressure in mmHg of O2?
16 mmHg
Use PV=nRT
Name THREE of the assumptions for ideal gasses.
(Here are 4)
Molecules are in constant rapid random straight line motion
When particles collide no energy is lost in the elastic collision
The individual particles have no volume
There are no attractive forces between particles