Name: ______Period:______Date:______
CP Chemistry Final Exam Study Guide
The CP Chemistry Final Exam will consist of 90 multiple choice questions and 3 open ended questions. The chapters and topics covered on the exam are listed below:
Chapter 8
Writing and balancing equations including all the proper symbols
5 different types of reactions
Predicting products
Chapter 9
Stoichiometry à molar ratios and problem solving
Limiting reactants à definition and calculations
Percent Yield
Chapter 10
Kinetic Molecular Theory of Gases
Chapter 11
Gas Laws à definition and calculations (Dalton’s, Boyle’s, Charles’, Gay-Lussac’s, Combined, Avogadro’s, Ideal, Graham’s)
Chapter 12
Definitions à solute, solvent
Types of mixtures (solution, colloid, suspension)
Molarity and Molality à definition and calculations
Solubility à factors affecting, rate and equilbrium
Chapter 13
Colligative properties
Chapter 14
Definitions of Acid and Basesà Arrhenius, Bronsted-Lowry and Lewis
Strong and Weak Acids/Bases
Chapter 15
pH and pOH scales and calculations
Chapter 16
Specific Heat à definition and calculations
Enthalpy
Hess’s Law
Entropy à definition only
Chapter 17
Factors affect reaction rate
Chapter 18
Chemical equilibrium
Directions: Define each of the following terms:
· Precipitate –
· Coefficient –
· Limiting Reactant –
· Percentage Yield –
· Theoretical Yield –
· Barometer –
· Diffusion –
· Effusion –
· Electrolyte –
· Colligative Properties –
· Alloy –
· Temperature –
· Heat –
· Entropy –
· Activation Energy –
· Effervescence –
Directions: Explain what happens during each of the following types of reactions, and write the general equation for each:
· Synthesis Reaction –
· Decomposition Reaction –
· Single-Displacement Reaction –
· Double-Displacement Reaction –
· Combustion Reaction –
Directions: Answer the following questions in the space provided.
1. What are the main observations that usually indicate that a chemical reaction has occurred?
2. Write both a word equation and a formula equation to represent the reaction that produces sodium hydroxide from sodium oxide and water.
3. Balance the following equations:
a. Fe2O4 + Al → Al2O3 + Fe
b. CaO + H2O → Ca(OH)2
c. Al + CuSO4 → Al2(SO4)3 + Cu
4. Answer the following questions using the activity series:
a. Name two elements that aluminum would be able to replace in a single-displacement reaction.
b. Name two elements that aluminum would NOT be able to replace in a single displacement reaction.
c. Predict the products that would form when aluminum is dropped into a solution of CuCl2.
d. Predict the products that would form when aluminum is dropped into a solution of HCl.
e. Predict the products that would form when aluminum is dropped into water.
5. Each of the four types of reaction stoichiometry problems requires using what type of conversion factor?
6. What are the units of molar mass?.
7. In the equation 2KClO3 → 2KCl + 3O2,
a. What is the mole ratio of KClO3 to oxygen?
b. how many moles of oxygen are produced when 5.0 mol of KClO3 decompose completely?
8. What happens when the limiting reactant in a chemical reaction is completely used?
9. Convert the pressure 0.90 atm to mm Hg.
10. What is STP?
11. A mixture of four gases exerts a total pressure of 500 mm Hg. Gases A and B each exert 150 mm Hg. Gas C exerts 90 mm Hg. What pressure is exerted by gas D?
12. Which mixture contains visible particles that settle out unless the mixture is stirred?
13. In which type of mixture do the particles scatter light, giving rise to the Tyndall effect?
14. What factors increase the rate of dissolution when dissolving a solid in a liquid?
15. What is the difference between a saturated solution and an unsaturated solution?
16. Write the equation for the dissociation of AlBr3. How many moles of ions will be produced from the dissociation of 1 mol of AlBr3?
17. Explain what a binary acid is, and give an example.
18. What is an amphoteric species?
19. At 25oC, what are the pH values for acidic, neutral, and basic solutions?
20. What are the units of energy?
21. What are the units of specific heat?
22. If a piece of copper is heated from 20.0oC to 80.0oC, what is the value of ∆T?
23. How is ∆H calculated for a chemical reaction? What type of chemical reaction would have a negative value for ∆H?
24. In general, how does the entropy of a solid compare with that of a liquid?
25. In order for molecules to react, they must collide. What are the two conditions required for a collision to be effective?
26. Explain what happens when a chemical reaction is at equilibrium.
EXTENDED RESPONSE QUESTIONS
Three of these extended response questions will be on your final exam. The numbers will be changed, but other than that these are the exact questions you will have to answer.
Chapter 8
1) Consider the following reactants: Al (s) + ZnCl2 (aq). Use the activity series to predict the outcome and products of the reaction, if any, and write a balanced equation.
Chapter 9
2) Consider the following reaction: P4 + 6Cl2 → 4PCl3. Identify the limiting reactant if 75.0 g of P4 reacts with 315 g of chlorine, and how much PCl3 will be formed in the reaction (the theoretical yield).
Chapter 11
3) Calculate the approximate volume of a 0.400 mol sample of gas at 20.0oC and a pressure of 1.25 atm.
4) Chlorine is produced by the reaction 2HCl (g) → H2 (g) + Cl2 (g). How many grams of HCl must be used to produce 10.0L of chlorine gas at STP?
Chapter 16
5) Determine the enthalpy change for the net reaction:
2C (s) + 2 H2O (g) → CH4 (g) + CO2 (g) ΔH =
from the following standard enthalpies of reaction:
C (s) + H2O (g) → CO (g) + H2 (g) ΔHo = 131.3 kJ
CO (g) + H2O (g) → CO2 (g) + H2 (g) ΔHo = -41.2 kJ
CH4 (g) + H2O (g) → 3H2 (g) + CO (g) ΔHo = 206.1 kJ
Chapter 12
6) How many grams of magnesium chloride would be needed to make 25.0ml of a 3.0M aqueous solution?