Chapter 10 Review
1. If a gas has a pressure of 865 mmHg, what is that pressure in kPa? (760 mmHg = 101.325 kPa) (Pressure conversion)
2. If you have a mass of 49 kg and are on Jupiter, where the acceleration due to gravity is 24.79 m/s2. What is your force in Newtons? (Force calculation)
3. While on Jupiter, you decide to stand on one foot. Your foot has an area of 0.15 m x 0.35 m. Calculate the amount of pressure exerted. (Pressure = F/A)
4. A sample of Argon has a volume of 3.8 L at 2.5 atm. What is the pressure if the gas is allowed to expand to 6.1 L? (Boyle’s Law)
5. A gas occupies 73 mL at 5.0°C. What will the temperature be (in °C) when the gas occupies 175 mL, assuming there is no change in pressure? (Charles’ Law)
6. How many moles of a gas are present if it occupies 7.5 L at 25°C at a pressure of 1.6 atm? (Ideal Gas Law)
7. A sample of a gas has a mass of 3.15 g and occupies 50.0 mL at STP. Find the molecular mass of the gas. (Molecular mass)
8. Find the density of Hydrogen fluoride gas at 1.26 atm and 22°C. (Density)
9. A gaseous mixture of Br2, O2 and H2 has a total pressure of 2.0 atm and contains 5.0 g of each gas. Find the partial pressure of each gas in the mixture. (Partial Pressure)
Chapter 11 Review
1. Since dispersion forces are the only forces present in the following compounds, which compound has the lowest boiling point? (Dispersion forces and boiling point)
GeF4 GeBr4 GeCl4
2. What type(s) of intermolecular forces are in the following? (Identifying IM forces)
a. Ne
b. CH3OH
c. NaCl
3. Place the following IM forces in order of lowest boiling point to highest. (Properties of IM forces)
H-bonding Ionic Dipole-dipole Dispersion
4. Using the graph below, what is the pressure and temperature at the triple point?
5. If this material was at a pressure of 30 atm and a temperature of 50°C, what state of matter would it be in?
6. If that same material in #5 was heated to 400°C at a constant pressure, what phase change would happen? (#4-6 – Phase diagram)
Chapter 13 Review
1. The Henry’s Law constant for Argon in water at 35°C is 6.2 x 10-4 M/atm. If the pressure is 795 mmHg, calculate the solubility of Argon. (Henry’s Law)
2. A solution is prepared by adding 7.14 grams of glucose, C6H12O6, to 100.0 grams of water. The final volume of the solution was 103.0 mL. Calculate the following. (Molarity, molality, mass % and mole fraction)
a. Molarity
b. Molality
c. Mass %
d. Mole fraction
3. What is the freezing point of a solution that contains 25.0 g of ethylene glycol (C2H6O2) in 275 g of chloroform? What is the boiling point? (Collig. Properties)
4. Using the solubility curve below, at 40°C, 50 g of KNO3 are dissolved in 100 g of water. Is this solution saturated or unsaturated?
5. If at 50°C, 80 g of KNO3 are completely dissolved in 100 g of water (and it’s saturated), how many grams of KNO3 would completely dissolve in 350 g of water?
6. A saturated solution of NH4Cl is formed in 100 g of water at 90°C. If that solution is cooled to 40°C, how many grams of precipitate are formed? (#4-6 – Solubility Curve)
Chapter 14 Review
1. Given the balanced equation H2 + Cl2 à 2 HCl and the following data, calculate the average rate for every 2 second interval. (Average rate)
Time (s) [Cl2] Average Rate (M/s)
0.0 1.5
2.0 0.9
4.0 0.6
6.0 0.4
2. Using the balanced equation and the following data, find the rate law.
2 NO + 2 H2 à N2 + 2 H2O
Trial [NO] [H2] Initial Rate (M/min)
1 1.5 1.0 0.55
2 1.5 2.0 1.1
3 4.5 1.0 4.95
3. Using the data above and your answer to #2, calculate the rate constant.
4. If the concentration of NO was 3.0 M and the concentration of H2 was 1.5 M, what would the reaction rate be?
5. What is the overall order of the reaction? (#2-5 – Rate laws)
6. The rate law for a first-order reaction can be written as:
2 NOCl à 2 NO + Cl2 Rate = k[NOCl] where k = 1.2 s-1
a. Determine the half-life of this reaction.
b. Calculate [NOCl] at t = 3.5 s if [NOCl]0 = 6.0 M. (Half-lives, concentrations)
7. The rate constant of a given reaction is 4.2 x 10-2 at 50°C. The activation energy is 15.5 kJ/mol. Calculate the value of the rate constant at 100°C.
8. A particular reaction has an activation energy of 25 kJ and an overall enthalpy change of 10 kJ. Sketch an energy profile for the reaction and label Ea and ∆E. What type of reaction is this (endo or exo)? What is the activation energy for the reverse reaction?