Download Chemistry 2 Final Exam Review_MC

Chemistry 2 Final Exam Review for Multiple Choice 2012
You will be provided a solubility chart. You will NEED a pencil (with an eraser) and a calculator. You may bring your periodic table
and an 8.5 inch x 11 inch cheat sheet, HAND-WRITTEN only on both sides of the paper.
Vocabulary (PLUS all of the other vocab that is on your objectives)
Arrehenius Acid and Base
Solvent
Bronsted Acid and Base
Aqueous
Diprotic acid
Calorimeter
Monoprotic acid
Heat Capacity
Triprotic acid
Joule
Amphoteric/amphoterism
Enthalpy
Conjugate Acid
Specific Heat
Conjugate Base
Heat of reaction
Equilibrium
Heat of formation
LeChatlier’s Principle
Hess’s Law
Activation Energy
Heat of Fusion
Catalyst
Heat of Vaporization
Precipitate
Endothermic
Solute
Exothermic
Boyle’s Law
Charles’ Law
Dalton’s Law
Gay-Lussac’s Law
Ideal Gas Law
STP
limiting reactant
excess reactant
theoretical yield
actual yield
percentage yield
Acid Base Review
1. Write the formula for the following acids and state whether they are monoprotic, diprotic, or triprotic.
hydrochloric acid
sulfuric acid
phosphoric acid
2. Name/write formula the following:
HNO2
Nitric acid
HCl
H3PO4
sulfurous acid
hydroselenic acid
3. List 3 properties of acids and list 3 for bases.
3.5 What common substance is amphoteric? Why?
4. Complete and balance the following reactions.
1.
H2S
2.
CO3
3.
H2Te
2-
+
KOH 
+
HSO3 
+
HPO4 
_____________________________________
-
______________________________________
2-
______________________________________
5. In reaction 1 above, is KOH acting as Arrhenius base or Bronsted Lowry Base?
2-
6. In reaction 2 above, is CO3 acting as an: Arrhenius acid, Arrhenius base, Bronsted Lowry Acid, or Bronsted Lowry base?
7. For reactions 2 and 3 write the acid and it’s conjugate base and the base and it’s conjugate acid.
1
Chemistry Final Review 2012
8. Complete the following chart.
[H+]
[OH-]
pH
pOH
acid/base/neutal
-8
1.8 X 10
5.35
+
+
9. The H (or H3O ) concentration of a solution is 1.23 x 10
-10
mol/L. What is the pH?
+
10. The pH of a solution is 6.5. Find the [H ] for this solution.
-
11. What is the pH of a solution if the [OH ] is 4.7 x 10
-11
mol/L?
-
12. What is the [OH ] concentration of a solution if the pH is 3.9?
13. Identify the acid, conj acid, base and conj base in this reaction.
+
-
HCl + H2O  H3O + Cl
14. What salt is formed from the neutralization reaction between hydrochloric acid and magnesium hydroxide?
15. What is transferred between a conjugate acid-base pair?
Thermochemistry
16. From the following enthalpy changes:
H2 + F2 2HF
H= -542.2 kJ
H= -571.6 kJ
2H2 + O2  2H2O
Calculate the value of Hrxn for the rxn: 2F2 + 2H2O  4HF + O2
17. What law did you use to solve this problem?
18. A 22.2 g sample of silver absorbs 65.5 J of heat energy when its temperature is raised from 31.0C to 43.5C . Find the specific
heat of silver.
19. How much heat is required to raise the temperature of 20.0 g of Fe from 26.00C to 72.30C? The specific
J/gC.
heat of iron is 0.447
20. How many joules are required to raise the temperature of 150. g of water from 30.0C to 50.0C? The specific heat of water is
o
4.184 J/g C.
21. What is a calorimeter used for?
21.5 Use the given standard enthalpies of formation to determine the heat of reaction (enthalpy change) of the following reaction:
C3H6O(l) + 4 O2(g) → 3 CO2(g) + 3 H2O(l)
ºf CO2(g) = -393.5 kJ/mole
2
ºf H2O(l) = -285.8 kJ/mole
Hºf C3H6O(l) = -249.5 kJ/mole
Chemistry Final Review 2012
Solubility/Solution
22. Use your solubility rules for the following to determine if the compounds are soluble or insoluble.
Compound
Name/formula
Soluble /Insoluble
CaBr2
Na2SO4
AlPO4
Potassium nitrate
Silver chloride
Magnesium hydroxide
23. Identify the products and predict the precipitate (by circling) for the following reactions. Balance the finished equation.
a.
b.
c.
Ba(NO3)2 (aq) + K2SO4 (aq)
AgNO3 (aq) + NaBr (aq)
FeCl3 (aq) + KOH (aq)
24. Calculate molarity (M) for the following problems:
a.
b.
57 g Al2(SO4)3 in 500. mL
45 g C6H12O6 in 500. mL
25. What mass of sucrose C12H22O11, is needed to make 300. mL of 0.50 M solution?
Gas Laws
26. A gas in a container has a pressure of 150. kPa at 35C. What is the pressure when the temperature is -120.C?
27. A sample of gas (H2) occupies 1200 mL at a pressure of 3200 torrs. If temperature is kept constant,
what would the new volume be at 4600 torrs.
28. A sample of N2 occupies a volume of 0.789 L at 26.0°C. What would the volume be at 40.0°C, if pressure remains the same.
29. Helium gas exerts a pressure of 750.mmHg at 25.0 degrees Celsius. If the volume is held constant, what pressure will it exert a 0
degrees Celsius?
o
30. What is the pressure in atmospheres exerted by 45.5 grams oxygen gas in a 5300 cubic centimeters container at 75.0 C?
31. At a constant pressure, a sample of CO2 gas has a volume of 110. mL at 200. Kelvin. If the temperature is raised to 400. Kelvin,
what would the new volume of CO2 gas be?
Stoichiometry
32. Using the balanced reaction below answer questions a-d:
2 KClO3 (s)  2 KCl (s) + 3 O2 (g)
a. How many moles of KClO3 are used to produce 10. moles of O2?
b. How many grams of O2 are produced if 2.50 g of KClO3 is completely decomposed by heating?
3
Chemistry Final Review 2012
c. What is the percent yield for this reaction if 0.78grams of oxygen was actually produced?
d. How many grams of KCl are produced if 2.50 g of KClO 3 is decomposed?
33. In the following equation, which is the limiting reactant if 2.6 moles of aluminum are reacted with 5.2 moles of HC1? (Balance
rxn first!)
Al + HCl  AlCl3 + H2
34. What mass of BaSO4 can be made from a solution containing 2.84 grams of Na2SO4 when 50.0 grams of BaC12 are added? Write
balanced equation first.
Equilibrium/LeChatlier’s Principle/Collision Theory
35. Why does a higher temperature cause a reaction to go faster?
36. Why does a higher concentration make a reaction go faster?
37. How does a catalyst work?
38. At equilibrium, how do the rate of a forward reaction and rate of the reverse reaction compare?
39. Given: C2H4(g) + H2(g)  C2H6(g)
a. What is the effect of decreasing volume on the contained gases?
b.
If more reactant, C2H4(g) , is added what will be the effect on the reaction?
c.
What change(s) would cause the reaction to shift right?
40. Name the following.
NO
__________________________________
NI3 ______________________________
CuF2 __________________________________
BaI2 _____________________________
SnO2 ___________________________________
CCl4 ______________________________
PCl5 __________________________________
P2O5 ______________________________
41. Write the formulas for the following.
bromine
____________________________
dinitrogen oxide
____________________________
iron (III) permanganate
____________________________
nitrogen dioxide
____________________________
tricarbon octahydride
____________________________
4
Chemistry Final Review 2012