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CHM1
Exam 16
Name ____________________________
Multiple Choice
1. A student determined a sample to have a mass of 0.0120 g. How many significant
figures are in the mass of this sample?
(1) 2
(2) 3
2.
(3) 4
(4) 5
The diagram below represents a portion of a 100 milliliter graduated cylinder.
What is the reading of the meniscus?
(1) 35.0 mL
(2) 36.0 mL
(3) 44.0 mL
(4) 45.0 mL
3. If an ideal gas is placed in a cylinder whose volume is 2.0 L at 1.0 atmospheres of
pressure, what will the pressure of the gas be if the volume is reduced to 1.0 L?
(1) 1.0 atm
(2) 2.0 atm
(3) 0.50 atm
(4) 15 atm
4. If a gas is placed in a seal container and the gas is heat, what happens to the pressure
of the gas?
(1) The pressure increases.
(2) The pressure decreases.
(3) The pressure remains the same?
CHM1
Exam 16
5. How many neutrons are in an atom of carbon–13?
(1) 5
(2) 6
(3) 7
(4) 13
6. What is the ground state electron configuration of a sulfur atom?
(1) 1s22s22p63s23p6
(2) 1s22s22p63s23p4
(3) 1s22s22p63s43p2
(4) 1s22s22p63s63p2
7. Elements in the same group of the Periodic Table have
(1)
(2)
(3)
(4)
The same number of valence electrons and similar chemistry.
The same number of valence electrons, but different chemistry.
Different numbers of valence electrons and similar chemistry.
Different numbers of valence electrons, and different chemistry.
8. A neutral phosphorus atom has how many valence electrons?
(1) 2
(2) 3
(3) 5
(4) 8
9. A metal is
(1)
(2)
(3)
(4)
malleable and conducts electricity.
brittle and conducts electricity.
malleable and does not conduct electricity.
brittle and does not conduct electricity.
10. Which of the following is an anion?
(1) Fluorine, F2
(2) Chloride, Cl-
(3) Copper, Cu
(4) Ammonium, NH4+
11. What is the atomic symbol for carbon
(1) C
(2) Ca
(3) Co
(4) Cu
12. What is the formula of carbon tetrafluoride?
(1) CF
(2) CF2
(3) C4F
(4) CF4
CHM1
13.
Exam 16
Given the reaction:
Pb(NO3)2 (aq) + Na2CrO4 (aq) 
PbCrO4 (s) + 2 NaNO3 (aq)
What is the total number of moles of NaNO3 formed when 2 moles of Na2CrO4 react
completely with excess lead (II) nitrate?
(1) 1 mole
(2) 2 moles
(3) 3 moles
(4) 4 moles
14. Which equation represents a double replacement reaction?
(1) 2 Na + 2 H2O  2 NaOH + H2
(2) CaCO3  CaO + CO2
(3) LiOH + HCl  LiCl + H2O
(4) CH4 + 2 O2  CO2 + 2 H2O
15. For the following balanced chemical reaction, what is the sum of the stoichiometric
coefficients?
CH4 (g) + 2 O2 (g)  CO2 (g) + 2 H2O (g)
(1) 1
(2) 2
(3) 4
(4) 6
16. What is the formula of ammonium sulfate?
(1) NH4SO3
(2) (NH4)2SO3
(3) NH4SO4
(4) (NH4)2SO4
17. How many grams of NaCl (molar mass = 58.5 g/mole) must be dissolved in 200. mL
of an aqueous solution to prepare a 0.100 M solution?
(1) 58.5 g
(2) 1170 g
(3) 1.17 g
(4) 0.585 g
18. What is the formula of ethanoic acid, which is more commonly known as acetic acid?
(1) HC2H3O2
(2) H2C2H3O2
(3) HC2O4
(4) H2C2O4
CHM1
Exam 16
19. Based on the following reaction
2 N2 (g) + 5 O2 (g)  2 N2O5 (g)
How many gram of N2O5 could theoretically be formed by reacting 10.0 g of elemental
nitrogen with 12.0 g of elemental oxygen?
(1) 27.1 g
(2) 11.3 g
(3) 38.5 g
(4) 16.2 g
20. Which structural formula represents an alcohol?
21.
(1)
(3)
(2)
(4)
Which of these formulas contains the most polar bond?
(1) H-Br
(2) H-Cl
22.
(3) H-F
(4) H-I
The nucleus of an atom of K-42 contains
(1) 19 protons and 23 neutrons
(2) 19 protons and 42 neutrons
(3) 20 protons and 19 neutrons
(4) 23 protons and 19 neutrons
CHM1
23.
Exam 16
A diagram of a chemical cell and an equation are shown below.
When the switch is closed, the electrons will flow from
(1) the Pb (s) to the Cu (s)
(2) the Cu (s) to the Pb (s)
(3) the Pb2+ (aq) to the Pb (s)
(4) the Cu2+ (aq) to the Cu (s)
24. Shown below are the reduction potentials for four half-reactions under standard
conditions.
Reduction half reactions
Ag+ + e- ---> Ag
Pb2+ + 2 e- ---> Pb
Cr3+ + 3 e- ---> Cr
Mg2+ + 2 e- ---> Mg
Reduction potentials
+0.80
-0.13
-0.74
-2.37
Which metal is most easily oxidized?
(1) Ag
(2) Pb
(3) Cr
(4) Mg
25. Given the reaction:
6 CO2 + 6 H2O  C6H12O6 + 6 O2
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
(1) 2.5
(2) 6.0
(3) 12
(4) 15
26. Which compound contains ionic bonds?
(1) N2
(2) NO2
(3) CaO
(4) CO2
CHM1
27.
Exam 16
Which graph shows the pressure-temperature relationship expected for an ideal
gas?
(1)
(2)
(3)
(4)
28.
Given the equation:
2 C2H2 (g) + 5 O2 (g)  4 CO2 (g) + 2 H2O (g)
How many moles of oxygen are required to react completely with 1.0 moles of C2H2?
(1) 2.5
(2) 2.0
29.
(3) 5.0
(4) 10
In the reaction 23993Np  23994Pu + X, what does X represent
(1) a neutron
(2) a proton
(3) an alpha particle
(4) a beta particle
30. The half-life of a radioactive substance is 2.5 minutes. What fraction of the original
radioactive substance remains after 10 minutes?
(1) 1/2 (3) 1/4
(2) 1/8 (4) 1/16
31. A student performed a titration in which she neutralized 16.4 milliliters of a HCl
solution by adding 12.7 milliliters of a 0.620 M KOH solution. What was the
molarity of the HCl solution?
(1) 0.168 M
(2) 0.480 M
(3) 0.620 M
(4) 0.801 M
CHM1
Exam 16
32. What is the pH of a 0.001 M HNO3 solution?
(1) 1
(2) 2
(3) 3
(4) 11
33. What is the pH of pure water?
(1) 0
(2) 1
(3) 7
(4) 14
34. Standard temperature and pressure are equal to
(1) 0°C and 50.6 kPa
(2) 32°C and 50.6 kPa
(3) 0°C and 101.3 kPa
(4) 32°C and 101.3 kPa
CHM1
Answers
1. 2
2. 1
3. 2
4. 1
5. 3
6. 2
7. 1
8. 3
9. 1
10. 2
11. 1
12. 4
13. 4
14. 3
15. 4
16. 4
17. 3
18. 1
19. 4
20. 2
21. 3
22. 1
23. 1
24. 4
25. 4
26. 3
27. 4
28. 1
29. 4
30. 4
31. 2
32. 3
33. 3
34. 3
Exam 16