Name_________________
Second Semester Final Exam
Multiple Choice: Please mark the answer to the multiple choice questions on your bubble sheet.
1) The molar mass of magnesium cyanide, Mg(CN)2, is approximately
A) 50.3 g
B) 64.3 g
C) 76.3 g
D) 100.6 g
2) The total number of atoms in (NH4)3BO3 is
A) 12
B) 17
C) 19
3) What is the mass in grams of 5.90 mol C8H18?
A) 0.0512 g
B) 389 g
C) 673 g
D) 19.4 g
4) How many atoms are there in 1 mole of helium?
5)
6)
7)
8)
A) 6.02 x 1023 atoms
B) 22.4 atoms
C) 4.0 atoms
D) 0.0821 atoms
The percent composition of silver (Ag) in AgNO3 is
A) 0.625 %
B) 1.57 %
C) 62.5 %
D) 157 %
E) 169.9 %
Which of the following is an empirical formula?
A) C2H4
B) C2H6
C) CH4
D) C3H6
Which of the following could be a molecular formula for the empirical formula CH2
A) C3H6
B) C6H3
C) CH
D) CH4
What is the coefficient in front of the O2 when the following reaction is correctly balanced?
____C3H8 + ____ O2  _____CO2 + _____ H2O
A) 1
B) 2
C) 3
D) 4
E) 5
9) What are the correct coefficients that would balance the following chemical reaction?
______P4 + _____O2  _____P2O5
A) 1, 5, 2
B) 1, 3, 2
C) 2, 5, 2
D) 2, 10, 5
E) 1, 5, 4
10) Which of the following is true about the chemical reaction: 2 H2 + O2  2 H2O
A) The mass of the products is more than the mass of the reactants.
B) The “” means equals.
C) There are two molecules of H2 for every one molecule of O2.
D) The reactants are on the right side of the arrow and the products are on the left side.
11) Identify the type of chemical reaction: C3H8 + O2  CO2 + H2O
A) composition
B) decomposition C) single replacement
D) double replacement
E) combustion
D) double replacement
E) combustion
12) Identify the type of chemical reaction: Mg + Cl2  MgCl2
A) composition
B) decomposition C) single replacement
13) Identify the type of chemical reaction: HCl + O2  H2O + Cl2
A) composition
B) decomposition C) single replacement
14) Given the following equation:
D) double replacement
E) combustion
N2 + 3 H2  2 NH3
How many moles of NH3 can be produced by reacting 15 moles of H2 with an excess of N2?
A) 22.5 moles
B) 15 moles
15) Given the following equation:
C) 10 moles D) 2 moles
E) 1 mole
2 H2O  2 H2 + O2
How many grams of O2 are produced from the decomposition of 90 grams of H2O?
A) 32 g
B) 45 g
C) 80 g
D) 160 g
E) 180 g
16) Given the following equation: 2 H2O  2 H2 + O2
How many liters of O2 will be produced from 9.0 g of H2O decomposing?
A) 4.5 L
B) 5.6 L
C) 8.0 L
D) 11.2 L
E) 22.4 L
17) Which of the following statements about limiting reactants is true?
A) Limiting reactants will always be solids.
B) Limiting reactants are left over when a reaction is complete.
C) The limiting reactant will have the greatest mass of starting material.
D) The limiting reactant will be used up before any other substance.
18) Given the following equation: 4 Fe + 3 O2  2 Fe2O3
What is the limiting reactant when 12.0 moles of Fe and 10.0 moles O2 react?
A) Fe
B) O2
C) Fe2O3
D) Both Fe and O2
19) A reaction is carried out according to the following equation 2 KBr  2 K + Br2
What is the % yield of the reaction if only 8.0 grams of Br2 were actually formed, but 12.0 grams of Br2
were theoretically supposed to form?
A) 1.5 %
B) 4%
C) 20%
D) 25%
E) 67%
20) Convert the pressure 35.0 inches of mercury into millimeters of mercury.
A) 0.0015 mm Hg
B) 1.378 mm Hg
C) 889.0 mm Hg
D) 7,955,872 mm Hg
21) Convert the pressure 0.0504 atmospheres into kilopascals.
A) 4.98 x 10-4 kPa
B) 1.51 kPa
C) 5.10 kPa
D) 38.3 kPa
22) Where is there more air pressure?
A) Above sea level
B) At sea level
C) Below sea level
23) If the temperature of a liquid decreases, the vapor pressure of the liquid will:
A) Increase
B) Decrease
C) Stay the same
24) According to the graph, at what pressure will Ethanol have a boiling point of 60 ⁰ C?
A) 17 kPa
B) 52 kPa
C) 63 kPa
D) 102 kPa
25) A solid substance has a definite
particle arrangement, melts over a
small range of temperatures, and
does not get gooey when heated.
This substance is most likely:
A) Amorphous
B) Crystalline
C) Deposition
D) Sublimation
26) When a gas turns into a liquid, the phase change is called:
A) Condensation
B) Evaporation
C) Freezing
D) Melting
27) What is the triple point of a substance?
A) The three states of matter exist at equilibrium at the same time.
B) The hottest temperature that a liquid can exist.
C) The hottest temperature that a solid can exist.
D) Only one state of matter is changing into another.
28) Using the phase diagram, at a pressure of 1 atmosphere and a temperature of 50 ⁰ C, water is in what
phase?
A) Ice
B) Water
C) Vapor
D) Triple point
29) When a solid turns straight into a gas, the phase change is
called:
A) Melting
B) Freezing
C) Sublimation
D) Deposition
30) The relationship between pressure and temperature is:
A) Inverse
B) Direct
C) Equal
D) Not related
31) A balloon with a volume of 2.50 liters has the temperature doubled while the pressure stays the same.
What is the new volume of the balloon?
A) 2.25 L
B) 2.50 L
C) 5.00 L
D) 7.50 L
32) How much space will one mole of oxygen take up at STP?
A) 22.4 L
B) 24.2 L
C) 44.8 L
D) 48.4 L
33) At what conditions do real gases behave most like ideal gases?
A) High temperature and high pressure
B) High temperature and low pressure
C) Low temperature and low pressure
D) Low temperature and high pressure
34) What is the volume of a balloon that contains 1.93 moles at a pressure of 100 kPa and a temperature of
20 ⁰C?
A) 3.21 L
B) 47.0 L
C) 293 L
D) 386 L
35) A container has hydrogen, oxygen, and an unknown gas in it. The total pressure of the container is the
standard pressure in kPa. If the hydrogen and oxygen BOTH have a partial pressure of 40.5 kPa, what is
the partial pressure of the unknown gas?
A) 20.3 kPa
B) 60.8 kPa
C) 679.0 kPa
D) 719.5 kPa
36) Which of the following is a solution?
A) pure water
B) magnesium metal
C) air
D) diamond
37) Which of the following is a solvent in coffee?
A) Sugar
B) Water
C) Caffeine
D) Cream
38) Which of the following will not mix with water?
A) polar solutes
B) nonpolar solutes
C) ionic salts
39) Alcohol and water completely mix together. Which sentence describes this solution?
A) Alcohol and water are miscible.
B) Alcohol and water are immiscible.
C) Alcohol and water are saturated.
D) Alcohol and water are electrolytes.
40) A solution contains as much solute as possible. What kind of solution is this?
A) Saturated solution
B) Unsaturated solution
C) Supersaturated solution
D) Aqueous solution
41) How does increasing the temperature of a solution affect the solubility of a solid?
A) The solubility increases as the temperature increases.
B) The solubility decreases as the temperature increases.
C) The solubility stays the same as the temperature increases.
42) Which solution is more concentrated?
43) If I dilute 500 mL of 2.0 M sodium acetate solution to a new total volume of 1750 mL, what will the
concentration of this solution be?
A) 1.75 M
B) 0.57 M
C) 1,750,000 M
D) 2252 M
44) Find the concentration of a solution that contains 2 moles of sugar dissolved in 0.5 L of solution.
A) 1 M
B) 1.5 M
C) 2.5 M
D) 4 M
45) What is the difference between a strong acid and a weak acid?
A) Strong acids only react with strong bases.
B) Strong acids contain hydride ions and weak acids do not.
C) Strong acids dissociate completely in solution.
D) Strong acids change the color of solutions.
46) Find the pH of a 0.00001 M solution of HCl
A) 0.000001
B) 1
C) 5
D) 7
47) If a solution has a pH of 4 what kind of solution is it?
A) Acidic
B) Basic
C) Neutral
D) Alkaline
48) Which of the following are the products of a neutralization reaction?
A) Water and salt
B) Water and oxygen
C) Acid and base
D) H+ and OH49) A student is doing a titration to find the molarity of 150 mL of an unknown acid. The student uses 47
mL of a 0.10 M standard solution of NaOH. What was the concentration of the unknown acid?
A) 0.03 M
B) 31.9 M
C) 705 M
D) 197.1 M
50) What is an indicator used for?
A) When an indicator changes colors you can find the concentration of the solution.
B) An indicator changes an acid into a base.
C) An indicator will change color depending on the pH of a solution
D) When an indicator changes color the solution is always neutral.
51) What is a common example of an acid?
A) Baking soda
B) Drain cleaner
C) Antacid tablets (Tums, Rolaids)
D) Vinegar
Formulas
1 mole = 6.02 x 1023 molecules = 22.4 L at STP = molar mass
% = part/whole x100
% yield = actual yield/theoretical yield x 100
1000mL = 1L
__________________________________________________________________
PV = nRT
Standard Pressure = 101.3 kPa = 1 atmosphere (atm) = 760 mm Hg = 29.92 inches Hg
°C= K-273
K=°C+273
P1V1 = P2V2
Tk1
Tk2
PT=P1+P2+P3…..
PV=nRT
Ideal Gas Law Constants:
R = 8.31 (kPa)(L)/(mole)(K) R = 0.0821 (atm.)(L)/(mole)(K)
pH = − (log [H+])
[H+] = 10−pH
Molarity = moles of solute /liters of solution
M1V1 = M2V2
Grams of solute= M x L x molar mass