CHEM 1310 EXAM 4
1. The formula for calcium phosphate is
2. The correct name for NH4NO3 is
A) hydrogen nitrogen oxide.
B) ammonium nitrate.
ammonium nitrogen trioxide.
Dissolve unknown substance in water
React unknown with known substance to form a precipitate
Filter and dry precipitate
Use chemical formula and mass of precipitate to determine amount of unknown
A summary of terminology for oxidation-reduction
or shift of
X loses electron(s)
Y gains electron(s)
X is oxidized
Y is reduced
X is the reducing agent
Y is the oxidizing agent
X increases its
Classify each of the following reactions.
Ca2+ + CO32NH3 + H+
Zn + 2HCl
Ca + F2
ZnCl2 + H2
Redox (H2 Displacement)
The concentration of a solution is the amount of solute
4.6 Lithium fluoride (LiF) is a strong electrolyte.
What species are present in LiF(aq)?
4.10 Identify each of the following substances as a
strong electrolyte, weak electrolyte, or nonelectrolyte:
4.14 Explain why
Apparatus for Studying the Relationship Between
Pressure and Volume of a Gas
As P (h) increases
P x V = constant
P1 x V1 = P2 x V2
Constant amount of gas
A sample of chlorine gas occupies a volume of 9
Chem 1310 Exam 3 Notes
Ionic compounds, strong acids, and strong bases (metal hydroxides) are strong
electrolytes (completely broken up into ions of the compound). Weak acids and weak
bases are weak electrolytes. Molecular substances other than acids or b
EXAM 3 CHEM 1310 WS09 Key
1. (p. 87) How many grams of sodium fluoride (used in water fluoridation and manufacture of
insecticides) are needed to form 485 g of sulfur tetrafluoride?
3SCl2(l) + 4NaF(s) SF4(g) + S2Cl2(l) + 4NaCl(s)
a. 1940 g
Name: _ Student #: _ (please print legibly!) Word Problem: If 15.8 g of solid barium hydroxide are disolved in 200 mL of 0.250 M phosphoric acid, a precipitate of barium phosphate forms. What is the mass of the filtered, dried precipitate? (20 points, you
Properties of Acids
Have a sour taste. Vinegar owes its taste to acetic acid. Citrus
fruits contain citric acid.
Cause color changes in plant dyes.
React with certain metals to produce hydrogen gas.
2HCl (aq) + Mg (s)
MgCl2 (aq) + H2 (g)
React with carbon
Name: _ Date: _ 1. The diameter of an atom is approximately 1 10 8 cm. What is this diameter when expressed in nanometers? A) 1 10 19 nm B) 1 10 15 nm C) 1 101 nm D) 1 10 10 nm E) 1 10 1 nm
2. How many milliliters is 0.005 L? A) 0.5 mL B) 5 mL C) 0.50 mL
Note: The following are MINIMUM sets of questions that will expose you to the
principles you are expected to master. I would recommend you do EVERY problem you
can get your hands on, especially those involving topics that give you difficulty!
3 FS12 (HEM
MUL T!PLE CHO
ij n ~ JI'~ rnative th
1) The c orrect name c
~ D m O_
est Completes t he
lor KzS is
l ".fJ ota ssium sulfide
E) dl'p t .
B) potassium sulfate
E xam3FSI2CHEM1310 White
Name_ _ _ _ _
MULTIPLE CHOICE. Choose the one alternative t hat b est c ompletes the statement o r a nswers t he q uestion.
1) W hat is the concentration (M) o f a NaCI solution prepared by dissolving 9.3 g o f NaCl i n suff
E xam3FSI2CHEM131O Yellow
N ame_ _ _ _ _ _ _ _ _ _ _
M ULTIPLE C HOICE. C hoose t he o ne a lternative t hat b est c ompletes t he s tatement o r a nswers t he q uestion.
1) C alculate the concentration (M) o f s odium ions in a s olution m ade b
Name: _ Date: _ 1. What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical reaction? V2O5(s) + 5Ca(l) 2V(l) + 5CaO(s) A) 5.6 g B) 40.0 g C) 20.3 g
D) 22.4 g E)
Exam 2 FS12 CHEM 1310 VERSION BLUE
Name _ _ _ _ _ _ _ _
MULTIPLE CHOICE. Choose the one alternative t hat best completes t he s tatement o r answers
the q uestion.
1) H ow m any liters o f w ine can be held in a w ine b arrel whose capacity is 26.0 gal
EXAM 2 FS12 CHEM 1310 VERSION GREEN
NAME: _ _ _ _ _ _ _ _ _
MULTIPLE CHOICE. Choose t he o ne alternative t hat best completes t he s tatement o r answers
t he q uestion.
1) A sample o f CH 2F2 with a mass o f 19 g contains atoms o f F.
E xam 2 FS12 C HEM 1310 VERSION WHITE
N ame_ _ _ _ _ _ _ _ _ _ _ _
MULTIPLE C HOICE. C hoose t he o ne a lternative t hat b est c ompletes t he s tatement o r a nswers t he q uestion.
1) The m ass % o f H i n m ethane (CH4) is _ _ _- '
E xam 2 FS12 C HEM 1310 VERSION Yellow
N ame _ _ _ _ _ _ _ _ _ _ _ _ _
MUL TIPLE C HOICE. C hoose t he o ne a lternative t hat b est c ompletes t he s tatement o r a nswers t he q uestion.
1) C alculate the percent ~nitrogen i n P tCI2(NH3)2.
Name: _ Date: _ 1. How many atoms are in 4.39 g of CO2? A) 6.01 1022 atoms B) 1.16 1026 atoms C) 6.04 1024 atoms
D) 1.81 1025 atoms E) 1.80 1023 atoms
2. What is the theoretical yield of vanadium, in moles, that can be produced by the reaction of 2.0 mole
Partial Credit Question EXAM 2 1400
You must show work to receive partial credit.
Part A (15 points)
1.00 grams silver nitrate reacts with 1.2 grams sodium sulfate to produce silver sulfate and
Step 1: Write a balance
Log into Blackboard
Go to CHEM 1310
Click on any assignment:
Click on the Launch button on the far right. This will take you to the McGraw Hill Connect site.
When you are there, enter in the code that was part of your package from the bookstor
Density (d) Calculations
m = PM
m is the mass of the gas in g
M is the molar mass of the gas
Molar Mass (M) of a Gaseous Substance
d is the density of the gas in g/L
A 2.10-L vessel contains 4.65 g of a gas at 1.00 atm and 27.0 0C. What
Daltons Law of Partial Pressures
V and T are constant
Ptotal = P1 + P2
Consider a case in which two gases, A and B, are in a container of volume V.
nA is the number of moles of A
nB is the number of moles of B
PT = PA + PB
Learning Objectives for Chapter 5
1. Explain how gases differ from liquids and solids
2. Understand how a barometer works and interconvert units of pressure
3. Describe Boyle's, Charles's, and Avogadro's laws, understand how they relate to the
ideal gas l
Exam 2 CHEM 1310 F811 Ver. 2 1400 Blue Name
1) One million argon atoms is _mol of argon atoms.
A) 1.0 X 10‘6 B) 6.0 X 1023 C) 1.0 X 10'6 ® 1.7 X 10'18 E) 3
2) There are , molecules of methane in 0.123 mol of methane (CH4).
A) 5 7.40 X 1022 C) 2.46 x 10'2