The Big 3
What is the name of these 3 formulas?
P1V1 = P2V2
V1/T1 = V2/T2
V1/n1 = V2/n2
Boyles - P1V1 = P2V2
Charles - V1/T1 = V2/T2
Avogadros - V1/n1 = V2/n2
What is the formula for the ideal gas law?
PV = nRT
What is the formula for freezing point depression and boiling point elevation? [Hint: they are basically the same]
Change in T = kb/f m (Molality)
What is vapor pressure?
The vapor pressure is the pressure exerted by a gas in equilibrium with its liquid phase at a given temperature
Explain the phrase "like disolves like" and what concept does it apply to
A solute will be able to dissolve in solvent if they have the same polarity. This concept is miscibility/solubility.
A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is increased to 60.0 mmHg?
8.20 L
What is the formula for density of a gas?
d = PM/RT
What is the formula for Henry's Law?
Cgas =kH Pgas
What is the normal boiling point?
The temperature at which its equilibrium vapor pressure is equal to 1 atmosphere.
What is the formula for Raoult's law?
Ptotal=x1 P1°+x2 P2°+x3 P3°+⋯
What is the proportionality of the 3 laws?
Boyles - inversely
Charles - directly
Avogadros - directly
The density of a gas is measured at 1.853 g / L at 745.5 mmHg and 23.8 °C. What is its molar mass?
46.01 g/mol
What is the formula for mole fraction and molality
Mole fraction - xb = Molb / (Mola + Molb)
Molality = Moles of Solute / Kilograms of Solvent
Carbon tetrachloride has a vapor pressure of 213 torr at 40.0 °C and 836 torr at 80.0 °C. What s the enthalpy of vaporization in kJ/mol?
31.4 kJ/mole
The normal freezing point of water is 0.00 ̊C and it's freezing point depression constant is 1.86 ̊C/m. If
we make up a 1.00 molal solution of Na2SO4, what is the freezing point of the mixture.
-1.86oC
A container with a volume of 25.47 L holds 1.050 mol of oxygen gas (O2) whose molar mass is 31.9988 g/mol. What is the volume if 7.210 g of oxygen gas is removed from the container, assuming the pressure and temperature remain constant?
20L
At what temperature will 0.654 moles of neon gas occupy 12.30 liters at 1.95 atmospheres?
447 K
What is the Clausius-Clapeyron Equation?
Too hard to type in here so I will write it on the board
Calculate the mass of water (in g) that can be vaporized at its boiling point with 155 kJ of heat (ΔHvap = 40.7 kJ/mol at 100 °C)
68.6 g of H2O
What is the vapor pressure of an aqueous solution that has a solute mole fraction of 0.1000? The vapor pressure of water is 25.756 mmHg at 25 °C.
23.18 mmHg
At one point in history people could measure temperature by looking at the volume of a sample of gas. Suppose a sample in a gas thermometer has a volume of 135mL at 11.0°C. Indicate what temperature would correspond to each of the following volumes: 113 mL, 142, mL, 155 mL , 127mL. (FIRST TO ANSWER CORRECTLY GETS THE CREDIT)
238 K or –35.3 °C; 299 K or 25.7 °C; 326 K or 53.1 °C; 267 K or -5.83 °C
Show how the ideal gas law and density question are related.
rearrange the variables and cancel some units out and you can create the equations from one another
What is the equation for Kinetic Energy OR urms and what are the key concepts about the equation?
KEavg=3/2 kB T or KEavg=1/2 murms^2
urms=√(3RT/M) or urms=√((3/2 kB T)/m)
Draw and label a phase diagram. Label all three phases and the two points
Henry’s law relates the _______ of a sparingly soluble gas in a liquid to the ______ _______ of the gas.
Concentration, Partial Pressure