Second Semester ACADEMIC Final Exam Review
Complete the following questions and make sure you go through your notes! This is not ALL that you need to remember but a guideline to help you study!
LS 4
Chemical reactions
Balance the following reactions:
1) __ C + __ H2 à __ C3H8
2) __ NH3 + __ O2 à__ NO + __ H2O
3) __ NaI + __ Pb(SO4)2 à __ PbI4 + __ Na2SO4
For the following reactions, indicate whether the following are examples of composition, decomposition, combustion, single replacement, or double replacement.
4) Na3PO4 + 3 KOH à 3 NaOH + K3PO4 ______
5) C6H12 + 9 O2 à 6 CO2 + 6 H2O ______
6) Pb + FeSO4 à PbSO4 + Fe ______
7) CaO à Ca + O2 ______
8) P4 + 3 O2 à 2 P2O3 ______
For the following reactants, predict the products and balance the equation.
9) ____ Al + ____ S à
10) ____ Ba3N2 à
11) ____ C6H14 + ____ O2 à
LS 5
Thermodynamics
12) What is an exothermic reaction? Which direction does the heat flow?
13) What is an endothermic reaction? Which direction does the heat flow?
14) How much heat will be released when 4.0 moles of sulfur reacts with excess O2 according to the following equation? 2 S + 3 O2 → 2 SO3 ΔH = –791.4 kJ
15) Draw a reaction profile for an endothermic reaction then label activation energy, ΔH, reactants, and products.
16) In the lab, Ms. Segal gets a beaker filled with 55 mL of water. She heats up a 30 gram piece of unknown metal and drops the metal into the water. The water has an initial temperature of 25 °C and it changes to 39 °C. The specific heat of water is 4.186 J/g °C?
A) How much heat is transferred to the water?
B) What is the specific heat of the metal if the metal had an initial temperature of 97 °C?
17) Mr. Reid takes 15.00 g of ice at -10.0˚C and heats it up to water vapor at 150.0˚C.
a. Draw the heating curve for the above reaction.
T (˚C)
Time (seconds)
b. Label the region of the graph where ice is melting and boiling.
c. When heat is added to water that is boiling at 100 ˚C, what happens to the temp. of the water? Why?
Kinetics
18) What are the four factors that can change the rate of a chemical reaction?
19) How does a catalyst speed up a reaction?
20) A reaction is third order with respect to A and first order with respect to B and C.
a. Write a rate law for the above reaction.
b. What is the overall order of the reaction? ______
c. If the concentration of A and B double while C stays the same, what happens to the original rate of the reaction?
Equilibrium
21) What does it mean for a reaction to be at equilibrium?
22) What will happen to the system using Le Chatelier’s principle?
2 SO2(g) + O2(g) ↔ 2 SO3(g) + energy
a. SO2 is added ______
b. SO3 is removed ______
c. The volume is decreased. ______
d. The temperature is decreased. ______
23) Given the following equation answer the questions below:
4 H2(g) + Fe3O4(g) ↔ 3 Fe(s) + 4 H2O(g)
a) Write the equilibrium expression for this reaction.
b) The concentration of each reactant at equilibrium is 0.5 M. The concentration for the products at equilibrium is 2.0 M. Calculate the Keq for the reaction.
LS 6
Chemical Quantities 1 mole = 6.02 x 1023 atoms or molecules = 22.4 L of gas at STP = Molar Mass
Make sure you show your work and label all your units!
24) Count the total number of atoms in the following compounds:
a) Ca(OH)2_____ b) HC2H3O2_____ c) Al(H2PO4)3 _____
25) Determine the formula mass of the following compounds:
a) SO3_____
b) Ca(OH)2_____
c) C12H22O11 ______
26) Convert 58g of CO2 to moles.
27) Determine the percent composition by mass of each element in Na2O.
Stoichiometry
28) Given the following equation: 2 KClO3 à 2 KCl + 3 O2
How many moles of O2 can be produced by letting 45 moles of KClO3 decompose?
29) Given the following equation: Cu + 2 AgNO3 à Cu(NO3)2 + 2 Ag
How many grams of Cu are needed to react with 11.22 grams of AgNO3?
30) Given the following equation:2 KClO3 à 2 KCl + 3 O2
How many Liters of O2 will be produced from 5.00 g of KClO3?
31) Given the following equation: 2 Fe + 6 HCl à 2 FeCl3 +3 H2
A) What is the limiting reactant when 120 moles of Fe and 145 moles HCl react?
B)Why?
32) A reaction is carried out according to the following equation:
2 KClO3 à 2 KCl + 3 O2
Calculate the percent yield of KCl if 5.0 grams of KCl was theoretically supposed to form and after running the experiment 4.7 grams of KCl were actually formed in lab.
LS 7
States of Matter
Gas pressure conversions: (1 atm = 760 mm Hg = 101.3 kPa = 14.7 lbs/in2 = 29.92 in Hg)
32) 400 mm Hg = ______kPa
33) 120 kPa = ______atm
34) Where is there more air pressure in a building?
A) The first floor B) The third floor C) The fifth floor
35) If the temperature of a liquid increases, the vapor pressure of the liquid will:
A) Increase B) Decrease C) Stay the same
36) What is the boiling point of water on top of a mountain where the pressure is 40 kPa?
37) Define the Triple Point of a substance.
38) Using the phase diagram, at a temperature of 75°C and a pressure of 0.006 atm, water is in what phase?
39) Tell if the following are either an Amorphous solid (A) or a Crystalline solid (C).
a. Salt ______b. Sugar ______c. Glass ______
d. Plastic ______e. Wax ______
f. Gets gooey when heated ______
g. Definite particle arrangement ______
40) Name the following phase changes…
a. Solid to liquid: ______b. liquid to gas: ______
c. Solid to gas: ______d. gas to liquid: ______
41) Why do liquids boil?
42) How can you get water to boil at a temperature lower than 100 ⁰ C?
Gas Laws
43) Define a direct relationship:
Define an inverse relationship:
44) Is the relationship between temperature and pressure a(n) direct or inverse relationship?
45) A balloon is filled with 3 liters of gas. The pressure is cut in half. What is the new volume?
46) What does STP mean?
47) How much space will one mole of hydrogen take up at STP?
48) At which conditions do real gases behave most like ideal gases?
49) How many moles of helium are in a balloon with a pressure of 5 atm, a volume of 17 liters and at a temperature of 47 degrees Celsius?
50) A container has oxygen, helium, and nitrogen in it. The total pressure is 500 mm Hg. If the helium and nitrogen have a partial pressure of 200 mm Hg EACH, what is the partial pressure of the oxygen?
51) A sample of air contains 44.0 kPa nitrogen and 12.4 kPa oxygen in a 500 mL bottle has a temperature of 26 ⁰ C.
A) How many moles of the nitrogen are in the bottle?
B) How many moles of the oxygen are in the bottle?
52) My best friend’s birthday is in the middle winter and she loves snow. She is having a party outside in order to celebrate. She loves balloons so I blow up a balloon with 0.50 grams of helium in a 22 ˚C room and the atmospheric pressure is 0.97 atm.
A) What is the volume of the balloon in liters?
B) I take the balloon outside in the cold (5 ˚C) and the balloon shrinks. What will the new volume of the balloon be when I give my friend her balloon?
LS 8
Solutions
53) What is meant by the term solution?
54) What is the difference between solute and solvent?
55) If you mix together water, grease, sugar, and Br2…which solutes will dissolve in which solvents? WHY?
56) What is the difference between a saturated, unsaturated, and supersaturated solution?
57) How does temperature affect the solubility of a solid dissolved in a liquid?
58) What is the difference between a concentrated solution and a dilute solution?
59) If I dilute 250 mL of 0.10 M LiC2H3O2 solution to a new total volume of 750 mL, what will the concentration of this solution be?
60) How many grams would I need to make 500 mL of a 1.5 molar KOH solution.
61) Find the concentration of a solution that contains 5 moles of sugar in 2.489 L of solution
62) How many liters of concentrated sulfuric acid would I need to make 1.5 liters of a 3.0 M sulfuric acid solution if I have 18 M sulfuric acid in the stock room.
Acids and Bases
63) What is the difference between a strong acid and a weak acid?
64) Find the pH of a 0.0001 M solution of HCl.
65) If a solution has a pH of 11.0 what kind of solution is it? Acid, base, or neutral?
66) What are the two products of a neutralization reaction?
67) A student is doing a titration to find the molarity of 200 mL of an unknown acid. The student uses 55 mL of a 2.3 M standard solution of NaOH. What was the concentration of the unknown acid?
68) What is an indicator?
69) What is the purpose of a titration?
70) What are some common examples of an acid?
71) What are some common examples of a base?
Final Exam Equation Sheet
1 mol = 6.02 x 1023 molecules = 22.4 L (STP) = Molar Mass in grams
1 atm = 760 mm Hg = 101.3 kPa = 14.7 psi = 29.92 in Hg
% yield = actual yield/theoretical yield x 100
______
pH = − (log [H+]) [H+] = 10−pH
grams = Molarity x Liters x Molar Mass
Molarity = moles of solute /liters of solution
M1V1 = M2V2
q = mc∆T
Keq= [products]x/[reactants]y
PV = nRT R = 0.0821 atm L / K mol
P1V1/TK1 = P2V2/TK2 PT = P1 + P2 + P3… ______
K = °C + 273