Heating and Cooling Curves
This type of curve is an endothermic process.
Heating curve
This is the Ideal Gas formula.
PV=nRT
What is the common formula for Dalton's Law of Partial Pressure?
Ptotal = P1 + P2 + P3...
This is the value for the R constant (with the correct units!)
0.08206 or 0.0821 L.atm/mol.K
How many liters are in 4.5 moles of carbon dioxide at STP?
101 L
How much energy would be required for 3.4 moles of Hydrogen to change from a liquid to a gas. ΔHvap: 0.499 kJ/mol.
Answer in kJ.
1.70 kJ
This equation explains how pressure and volume are related to one another.
P1V1 = P2V2
A container contains the following gases: 3.4 atm of hydrogen, 6.2 atm of oxygen, and 2.33 atm of carbon. What is the total pressure in the container?
11.9 atm
This equation is the foundation of Avogadro's Law.
V1/n1 = V2/n2
How many moles are in 3.5 L of hydrogen gas at standard conditions?
0.156 moles
How much energy would be required for 8.6 grams of Helium to change from a liquid to a gas? ΔHvap: 0.083 kJ/mol.
Answer in kJ.
0.178 kJ
The pressure of hydrogen changes from 3.4 atm to 8.7 atm. If the final temperature is 124K, what is the original temperature?
48.6 K
The total pressure of a container is 8.33 torr. The following are the gases and their appropriate partial pressures: 2.3 torr hydrogen, 3.9 torr nitrogen, and an unknown pressure of helium. What is the pressure of helium?
2.13 torr
The volume of oxygen changes from 3.4 L to 2.1 L. If the original number of moles was 5.9, what is the new number of moles?
3.64 moles
What is the volume (in L) of 45.7 grams of carbon dioxide at STP?
23.3 L
How much energy would be required for liquid water to revert back to it's solid state? Mass of the sample is 34.29 grams. Answer in kJ.
ΔHvap: 40.7 kJ/mol
ΔHfus: 6.01 kJ/mol
11.4 kJ
R = 0.08206 L.atm/mol.K
A 5.4 mol sample of oxygen occupies a 12.9 L container and is found to have a pressure of 6.98 atm. What is the temperature of oxygen?
203 K
Hydrogen: 9.8 atm
Helium: 8.77 atm
Argon: 10.2 atm
Oxygen: 5.78 atm
Chlorine: 9.88 atm
Nitrogen: Unknown (find value)
Total Pressure: 53.83 atm
9.47 atm
DOUBLE JEOPARDY
R = 0.08206 L.atm/mol.K
A sample of nitrogen gas has the following values: 120K, 13.4 L, and 4.3 atm. What is the mass of the sample?
164 g
6 CO2 + 6 H2O → C6H12O6 + 6 O2
Find the volume of carbon dioxide produced at STP when 14.3 grams of oxygen gas reacts.
10.0 L
DOUBLE JEOPARDY
How much energy would be required for 56.3 g of water at 33°C to increase to 121°C? Answer in kJ.
Tb: 100°C
ΔHvap: 40.7 kJ/mol
c(liquid): 4.184 J/g°C
c(gas): 0.002 J/g°C
143 kJ
The pressure of a substance changes from 4.6 atm to 6.3 atm. At the same time, the temperature changes from 201K to 250K. If the original volume of the substance is 8.5 L, what is the new volume?
7.72 L
DOUBLE JEOPARDY
A gaseous mixture inside a container is found to have a pressure of 89.65 mmHg. The mixture contains 4 gases: helium, hydrogen, oxygen, and nitrogen. Nitrogen has a partial pressure of 43.2 mmHg. Hydrogen has a partial pressure of 10.09 mmHg. Helium has a partial pressure double that of the hydrogen sample. What is the partial pressure of oxygen?
16.18 mmHg
The pressure of a substance changes from 8.6 atm to 12.3 atm. At the same time, the volume changes from 9.8 L to 5.43 L. If the new temperature is 134K, what is the original temperature?
169K
DOUBLE JEOPARDY
6 CO2 + 6 H2O → C6H12O6 + 6 O2
How many grams of glucose would be required for 121 L of oxygen at STP to react completely?
162 L