Dalton's Law
Phase Diagram
Ideal Gas Laws
Combined Gas Laws
Stoichiometry
100
How do you find the total pressure of a mixture of gasses?
Add the partial pressures of each gas
100
The phase from gas to liquid is _______, and the phase from liquid to gas is _________.
Condensation, Vaporization/Evaporation
100
The three properties of a gas that we can measure are......
Pressure, Temperature, and Volume.
100
Convert 785 mL to L
0.785 L
100
1 mol = ____ L
22.4 L
200
Find the total pressure for a mixture containing two gasses with partial pressures of 3 atm and 9 atm
12 atm
200
At the critical point, _______ cannot exist.
liquid
200
1 atm = ______kPa
101.3 kPa
200
What formula do we use for combined gas laws?
P1V1/T1 = P2V2/T2
200
The standard temperature and pressure (STP) is....
Temperature: 0ºC, 273 K
Pressure: 1 atm, 760 torr/mmHg, 101.3 kPa
Volume: 22.4 L
300
Find the total pressure for a mixture that contains four gasses with partial pressures of 3.00 kPa, 4.50 kPa, 3.09 kPa, and 1.60 kPa.
3.00 kPa + 4.50 kPa + 3.09 kPa, 1.60 kPa =
12.19 kPa
300
The phase from solid to gas is __________, and the phase from gas to solid is _____________.
Sublimation, Deposition
300
Convert 30oC to Kelvin (K)
303 K
300
How many moles of CaCO3 would be needed to completely react with 0.563 moles of 2HCl?
CaCO3 + 2HCl 🡪 CO2 + CaCl2 + H2O
0.563 mol HCl x 1 mol CaCO3 / 2 mol HCl
= 0.282 mol CaCO3
300
What is the volume of 3.00 moles of carbon dioxide gas (CO2) at Standard Temperature, & Pressure (STP)?
67.2 L
400
If the partial pressures of three gasses in a tank are 25 atm, 10 atm, and 15 atm, what is the total pressure inside of the tank?
25 atm + 10 atm + 15 atm =
50 atm
400
If this substance was at 1.25atm at -100oC, what phase change would occur if the temperature increased to 300oC
Melting
400
How many moles of oxygen will occupy a volume of 2.0 L at 1.5 atm and 20oC?
n = 0.12
(1.5)(2.0) = n(0.0821)(293)
400
At 20oC and 1.5 atm pressure, a gas fills 3.0 L. What is its pressure at 25oC and 3.5 L?
1.28 atm
(1.5)(3.0)/293 = P(3.5)/298
400
How many grams of Cl2 are needed to completely react with 112 grams of 2KBr?
Cl2 + 2KBr 🡪 Br2 + 2KCl
33.4g Cl2
112 KBr x 1 mol x 1 mol x 70.9g / 119g x 2 mol x 1 mol
500
If the total pressure of four gasses is 100 atm, and the the partial pressures of three gasses are 20 atm, 60 atm, and 10 atm, what is the partial pressure of the fourth gas?
10 atm
20 + 60 + 10 + 10 = 100
500
What is the freezing and boiling point of this diagram?
Freezing: 100oC
Boiling: 350oC
500
At what temperature will 0.80 moles of Ne occupy 10.00 liters (L) at 1.27 atmospheres (atm)?
(1.27)(10.00) = (0.80)(0.0821)T
T = 181.43 K
500
The volume of a gas at STP is 680 mL. What will the volume be if the pressure rises to 1.5 atm and 40 oC?
(1)(680)/273 = (1.5)V/313K
V = 519.76mL or 0.52 L
500
If 30.0 grams of Zn are used in the reaction, how many moles of H2 can be produced?
Zn + 2HCl 🡪 H2 + ZnCl2
0.47 mol