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CHM 114 Practice Final Exam 76 Questions (Solutions) Arizona State University

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CHM 114

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Arizona State University

CHM 114 Practice Final Exam 76 Questions (Solutions) Arizona State University CHM 114 Practice Final Exam 76 Questions (Solutions) Arizona State University Chapter 1 (Fundamentals of Matter & Measurement) 1. What type of matter does the microscopic diagram below describe? A. Pure element B...

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CHM 114 Practice Final Exam 76 Questions (Solutions) Arizona State Universi
Chapter 1 (Fundamentals of Matter & Measurement)

1. What type of matter does the microscopic diagram below describe?

A compound consists of two or more
different elements. Three molecules
represent a compound such as H2S. The
other two molecules represent an
element such as N2.

Therefore, the diagram represents a
mixture of an element and a
A. Pure element compound.
B. Pure compound
C. Mixture of an element and a compound
D. Mixture of elements
E. Mixture of compounds

2. The measurement 12.5109 m can also be written with different units without the use of exponents as
12.5 .

A. km 1 nm = 10-9 m,
B. mm so 12.5 nm is equal to 12.5109 m
C. Mm
D. m
E. nm

3. The flow rate for a gas was determined to be 22.4 liters per second (L/s). What is the flow rate in units
of gallons per minute (gal/min)? (1 gallon = 3.7854 liters)

A. 1.41 gal/min
B. 5.92 gal/min 22.4 L
s
× 60 s × 1 gal =355 gal
min
C. 10.1 gal/min 1 min 3.7854 L
D. 355 gal/min
E. 5090 gal/min

Chapter 2 (Atoms, Isotopes, Ions, Molecular & Ionic Compounds, Nomenclature)

4. What is the symbol for an isotope that has 21 protons and 24 neutrons?

45 Sc
A. 21
Atomic number = 21 protons, which is the atomic
B. 24
21 Sc number for scandium, Sc.
C. 45
24 Cr The mass number = 45, which is the sum of the
D. 21
Cr number of protons (21) and neutrons (24) in this
24
specific isotope.
45 Sc
E. 69
45 Rh The isotope symbol is 21
therefore:

P. Marks 2024

,5. A specific metal with a 2+ charge (M2+) has 28 electrons. What is the identity of the metal?

A. Fe A metal with a 2+ charge has two fewer negatively-
B. Ni charged electrons than positively-charged protons.
C. Zn With 28 electrons, the nucleus must have 30 protons and
D. Ca an atomic number of 30, which corresponds to zinc, Zn.
E. K

6. Which of the following is composed of discrete molecular units?

A. MgCl2 Molecular compounds usually exist as individual molecules, so they exist as discrete
(separate) molecular units. Molecular compounds are composed of atoms of
B. TiO2
nonmetal elements. The only molecular compound listed is methanol, CH3OH.
C. AgNO3
(The others are ionic compounds.)
D. CH3OH
This is in contrast to ionic compounds which do not exist as molecules, but instead
E. NaOH exist as extended crystalline lattices of cations and anions. The formula for an ionic
compound represents the ratio of ions.

7. What is the formula for sodium carbonate?
A. NaCO3 This is an ionic compound, so it’s composed of ions.
B. Na(CO3)2 Sodium ion = Na+
C. Na2CO3 Carbonate ion = CO32-
D. Na2CO2 In compounds, charges sum to zero so the ratio of ions
E. NaHCO3 must be 2:1, so we write the formula as Na 2CO3.

8. The compound NO2 is named .
A. nitrogen oxide This is a molecular compound, because it’s composed of
B. nitrogen dioxide nonmetal atoms.
C. nitrogen(IV) oxide Molecular compounds are named using Greek prefixes.
D. nitrite NO2 is named nitrogen dioxide.
E. nitrate

9. Identify the formula that correctly matches the
name. Remember to classify compound as ionic or molecular
A. sodium nitrate, NaNO2 before naming. The Roman numeral indicates the metal ion
charge for metals that can form ions with different charges.
B. chromium(I) oxide, CrO
C. copper(II) sulfate, CuSO4 The correct name and formula is copper(II) sulfate, CuSO4.
D. sulfur dioxide, S2O The correct formulas for the others are:
E. aluminum chloride, AlCl2 A. NaNO3 B. Cr2O D. SO2 E. AlCl3

Chapter 3 (Moles, Compound Composition, Non-aqueous Reactions, Stoichiometry)

10. After the following equation is properly balanced, what is the coefficient in front of O2?

C6H14(l) + O2(g)  CO2(g) + H2O(g)
A. 2
B. 6
C. 7 C6H14(l)+ 19/2O2(g)6CO2(g)+ 7H2O(g)
D. 14
Multiply through by 2:
E. 19
P. Marks 2024
2C6H14(l)+19O2(g)12CO2(g)+ 14H2O(g)

, 11. Which sample contains the greatest number of molecules?
Grams MM Moles Avogadro's
A. 10.0 g F2 # Molecules  1 mol  6.022×1023molecules

B. 20.0 g F2  
X g 22 or Cl    
g   1 mol
  number of
 
molecules
C. 10.0 g Cl2 F
This shows us that the sample with the greater number of molecules has
the
D. 20.0 g Cl2 greater mass and a substance with smaller molar mass.
E. This all contain the same number of molecules

12. Determine the total number of ions in 0.010 mol Mg(NO3)2.

A. 3 ions Moles Avogadro's # # formula units #ions/
   # ions
for mula uni t
B. 7 ions  6.022×1023 formula unit
 s  3 ions 
C. 6.01021 ions 0.010 mol Mg(NO3 )2   1 mol
   1 formula
D. 1.81022 ions = 1.8×1022 ions unit 
E. 4.11022 ions

13. How many grams of NaOH are in 0.10 mol NaOH?
A. 4.0 grams
B. 40 grams Moles xMM
C. 400 grams Grams
D. 6.641023 grams  
0.10 mol NaOH   40.00
 g   4.0 g
 1 mol
E. 6.01022 grams NaOH 

14. The balanced equation for the detonation of nitroglycerin is shown below. If 0.36 mol of C3H5O9N3
react, how many moles of H2O should form?

4C3H5O9N3(l)  12CO2(g) + 6N2(g) + O2(g) + 10H2O(g)

A. 3.6 B. 0.36 C. 36 D. 0.90 E. 0.14
Moles C H O N xmole ratio Moles
3 5 9 3 2
H O  10 mol H O 

0.36 mol C H O N
3 5 9 3  2
 4 mol 3C5 H O
 0.90 mol H2O
9 3 
N 

15. A piece of pure calcium metal is allowed to sit out on a lab bench, exposed to the oxygen in the air for a
few hours. It gains a mass of 0.12 g due the following reaction:

2Ca(s) + O2(g)  2CaO(s)

What mass of calcium metal has reacted to form calcium oxide?

A. 0.30 grams Ca The gain in mass (0.12 g) is equal to mass of O2 gas reacting. Because it’s
B. 0.15 grams Ca a gas it was not weighed initially. The rest is stoichiometry:
C. 0.60 grams Ca
D. 0.12 grams Ca Grams MM Moles mol ratio Moles MM Grams
E. 0.24 grams Ca
 0.12 g 2

 32.00
 1 mol
  2 mol Ca   40.08 g
g O  Ca 1 mol O  1 mol
O2 Ca
  2   2   
P. Marks 2024 O
 0.30 g Ca
reacted

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