Name:____________________
Date:_______________
Honors Chemistry Review for Final 2014
Chapter 10
1. Draw the Lewis Dot Structure and determine the molecular geometry of the
following molecules:
a. NF3
b. CCl4
c. H2S
d. CO2
e. CH3OH
2. Draw the Lewis Dot Structure of the following molecule, including any resonance
and bond polarity arrows:
CH3CH2CO2-
Chapter 11
3. Which IMFs are present in a sample of the following molecules?
a. NF3
b. CCl4
c. H2S
d. CO2
e. CH3OH
f. CH3CH2CO2-
4. What type of interaction occurs between NF3 and CCl4?
5. Which of the substances from Question 3 would have the lowest boiling point?
Highest boiling point? Explain.
6. An insulated beaker contains 100 g of water at 24.6°C. A 90-g piece of a metal is
heated to 100°C and placed in the water. The temperature of the water rises until
it plateaus at 29.2°C. Calculate the specific heat of the metal. (The specific heat of
water is 4.184 J/g⋅ K.)
Chapter 12
7. If you have 500 mL of a 0.8 M solution of MgCl2, how many moles of MgCl2 do
you have? How many moles of Cl- do you have?
8. How many grams of KNO3 do I need to make 250 mL of a 6M solution?
9. Use the following balanced equation to solve.
2NH4Cl(aq) + Ca(OH)2(aq) → CaCl2(aq) + 2NH3(g) + 2H2O(l)
How many grams of calcium chloride will be made when 750 mL of a 0.5 M
ammonium chloride solution react?
10. Calculate the molality and boiling point of a solution made of 48 grams of
CH3OH dissolved in 200 grams of water.
Name:____________________
Date:_______________
Honors Chemistry Review for Final 2014 – Part II
Chapter 13
1. What volume will 100 grams of CO2 occupy at STP?
2. Based on the following equation, what volume of SO2(g) will be produced if 15
grams of CS2(l) react at 1.5 atm and 40°C?
CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)
Chapter 14
3. Write the K expression for the following reaction:
CS2(l) + 3O2(g) → CO2(g) + 2SO2(g)
4. If the equilibrium concentration of NO2(g) is 3.4 x 10-3 M at 25°C, what is the
equilibrium concentration of N2O4(g)?
2 NO2 (g) ⇔ N2O4 (g)
K = 6.7 at 25°C
5. Assuming the reaction in Question 4 is endothermic, which way will the
equilibrium shift if we apply the following stresses?
a. Cool the reaction vessel
b. Add a catalyst
c. Decrease the volume of the container
d. Remove N2O4(g)
Chapter 15
6. If the pH of a solution is 4.5, what is the concentration of hydroxide?
7. Calculate the pH of a 0.002 M solution of Ca(OH)2.
8. What is the conjugate acid of HSO4-?
9. What is the conjugate base of HCO3-?
10. If you have the following equilibrium established from a buffer made of acetic
acid and sodium acetate, what will happen to the concentration of acetate if base
were added to the solution?
CH3COOH  H+ + CH3COO-
Chapter 16
11. The molar enthalpy of the combustion of methanol, CH3OH, is -726 kJ/mole.
How much heat is released if 50 grams of methanol burn?
12. Predict the sign of ΔG for the following reaction:
Heat + AB(g)  A(s) + B(g)
Chapter 17
13. Identify the oxidizing agent in the following reaction:
Zn(s) + CuCl(aq)  ZnCl(aq) + Cu(s)