1. HONORS CHEMISTRY
SEMESTER 2
FINAL REVIEW
TEACHER VERSION

2. A hot piece of steel is added to 100. 0 g of water at 21. 0 oC
A hot piece of steel is added to g of water at 21.0 oC. The specific heat of water is J/g oC. How much heat was transferred, if the final temperature is 26.0 oC?
Q = (100g)(4.184)(26-21oC)
= 2092 J
= 2090 J

3. 2. A metal sample has a mass of 800.0g
and a specific heat of 0.42 cal/goC. If the
sample gives off 110 cal of heat, what is
its change in temperature?
∆T = Q/(mCp)
= (110 cal)/(800.0 g)(0.42 cal/goC)
= 0.33 oC

4. 3. Water boils at 100 oC. What is the temperature in K?
K = oC + 273 =
= 373 K

5. 4. Is the following reaction
exothermic or endothermic?
H2O(s) + heat → H2O(l)
Endothermic

6. 5. 68 oF is equivalent to how many oC?
T(oC) = 5/9[T(oF) – 32]
= 20 oC

7. 6.
-50 oC is equivalent to what temperature in K?
T(K) = T(oC) + 273 =
= 223 K

8. 7. If a sample of chloroform is initially at 32oC, what is its final temperature if 225.0g of chloroform absorbs 725 Joules of heat, and the specific heat of chloroform is 0.96 J/(goC)?
Q = mc∆T
725J = (225.0g)(0.96 J/goC)(Tf-32oC)
3.4 = (Tf-32oC)
Tf = 35.4oC

9. 8. When a substance changes from a solid to a
gas, the phase change is called
a) Melting
b) Sublimation
c) Evaporation
d) Condensation

10. 9. When ammonium nitrate is dissolved, the
temperature of the water goes down. Heat
is absorbed by the reaction. Which of the
statements is the most accurate.
a) the reaction is endothermic.
b) the reaction is exothermic.
c) both a and b
d) neither a or b

11. 10. Which of the following is named incorrectly?
a) Sn3(PO4)2 tin(II) phosphate
b) Fe(OH)3 iron(III) hydroxide
c) Fe(HCO3)2 iron (II) bicarbonate
d) N2O4 nitrogen tetroxide
e) none of the above
DINITROGEN TETROXIDE

12. 11. A chemical reaction is a process in which
a) phases change between reactants and products.
chemical and physical properties remain unchanged.
the law of conservation of matter (mass) applies.
heat is generated.
all of the above

13. 12. What is the physical state of methanol (CH3OH) in
the following reaction:
CH3OH (l) O2 (g)  CO2 (g) H2O (l)
a) Gas
b) Liquid
c) Solid
d) Aqueous

14. 13. What scientist is associated with the direct
relationship between temperature and volume?
a) Arrhenius
b) Boyle
c) Charles
d) Avogadro

15. 14. Avogadro's number represents
a) the number of atoms in a mole of zinc
b) the number of molecules in a mole of
nitrogen gas
c) the number of eggs in a mole of eggs
d) all of the above
e) none of the above

16. 15. What is the molar mass of bromine gas?
a) g/mol
b) g/mol
c) g/mol
d) there is not enough information provided to answer
e) none of the above
BROMINE IS A DIATOMIC MOLECULE

17. 16. Convert 290. g of water to moles:
a) moles
b) moles
c) moles
d) moles

18. 17 How many molecules are in 9.0g of H2O?
a) molecules
b) x 1023 molecules
c) x 1023 molecules
d) x 1023 molecules
e) x 1023 molecules

19. 18. How many molecules are in 5.7 moles of KCl?
a) 3.4 x 1024 molecules
b) 2.4 x 1023 molecules
c) 425 g
d) 2.9 x 1024 molecules
e) 5.1 x 1023 molecules

20. 19. Two moles of silicon contains how many atoms?
a) atoms
b) x 1024 atoms
c) x 1023 atoms
d) x 1023 atoms
e) none of the above

21. 20. Consider the following reaction
CrCl3(s) + KCl(s) + 2H2SO4(l) → KCr(SO4)2(s) + 4HCl(g)
green white colorless purple colorless
solid solid liquid solid gas
When reaction is done, a wet purple solid containing
solid green specks remains. Which substance is the
limiting reactant?
a. CrCl3
b. KCl (nothing remained of this reactant in the product)
c. H2SO4
d. KCr(SO4)2
e. none of the above

22. 21. Calculate the number of moles of carbon dioxide
that can be produced in the atmosphere, when
124. grams of carbon reacts with
excess oxygen.
C (s) + O2 (g) → CO2 (g)
a) moles
b) moles
c) moles
d) moles
e) moles

23. 22. The reactant that gets completely
consumed in a reaction process, while
some of the other reactants are left over
is called
a) the excess reactant
b) the limiting reactant
c) the short reactant
d) the abundant reactant

24. 23. Consider the reaction, H2(g) + F2(g) → 2HF(g)
In which picture of the reactants is H2(g) ( )
the limiting reactant?
None of
these
a b c d e
The limiting reactant is completely used
up during the reaction, so nothing should remain
of it as a product.

25. 24. How many grams of silver (I) iodide are produced
when silver reacts with 12.7 grams of aluminum
iodide in the following equation?
Silver + Aluminum iodide  Silver (I) iodide + Aluminum
a) g
b) g
c) g
d) g
e) none of the above

26. 25. Given 12.8 grams of HBr and 8.2 grams of KOH,
what is the maximum number of grams of H2O
that can be formed during the reaction
KOH + HBr  KBr + H2O?
a) 28. grams
b) 23. grams
c) 2.8 grams
d) 2.6 grams (can’t form more than the least)

27. 26. What percentage by mass of ammonium chloride
is hydrogen?
a) 11 %
b) 88 %
c) 7.5 %
d) 6.7 %

28. 27. Which one of the following molecular
formulas is also an empirical formula?
a) C2H6
b) C3H8
c) H2O2
d) K2P4O6
e) C4H4
The empirical is the lowest reduced ratio between
The atoms in the formula.

29. 28. Convert 9120 mmHg of pressure to atm:
a) 140 atm
b) 2.9 atm
c) atm
d) atm
e) none of these

30. 29. In an experiment pressure and volume are compared
by placing increasing force on a syringe. The data is
graphed. Which statement is most accurate?
a) The pressure decreases with increasing force.
b) The volume decreases with increasing force.
c) The pressure increases with increasing force.
d) The volume increases with increasing force.
e) Both b & c

31. 30. When using the ideal gas law, temperature is
expressed in
a) Kelvin
b) degrees F
c) degrees C
d) none of the above
e) any of the above

32. 31. Which statement best describes the
relationship between volume and pressure?
a) they are inversely related
b) as pressure increases, volume increases
c) they are directly related
d) none of the above
Pressure ↑ Volume ↓
Pressure ↓ Volume ↑

33. 32. If a gas has a pressure of 2.40 atm and a volume
of 480. mL, what will the volume be if the pressure
is changed to 10.0 atm?
a) 115 mL
b) 210 mL
c) mL
d) mL
e) none of the above
(2.40atm)(480mL) = (10.0atm)V2
V2 = (2.4 x 480)/10
V2 = 115 mL

34. 33. If a gas has a temperature of 273 K and a pressure
of 5.00 atm in a rigid container, when the
temperature is raised what should happen to the
pressure?
a) it should decrease
b) it should stay the same
c) it should increase
d) it should become 0 atm

35. 34. If a gas has a pressure of 4.6 atm, a volume of 2.5 L,
and the temperature is 100 K, how many moles of
gas are there?
a) 4.0 moles
b) 1.4 moles
c) 4.8 moles
d) 2.8 moles
(4.6atm)(2.5L) = n( )(100K)
n = (4.6atm x 2.5L)/( x 100K)
n = 1.4 mol

36. 35. Which of the following is an example of a solution
a) oil + water
b) Pb + water
c) NaI + water
d) water
e) all of the above
A solution is a homogenous mixture. You need
a solution that you can’t see the parts of the
mixture. NaI is a salt and will dissolve in water.

37. 37. In a solution the substance dissolving the solid is
called the:
a) solid
b) solvent
c) solute
d) precipitate

38. 39. What is the molarity (M) of a solution of
nitric acid, if 4.2 moles are added to 3.9
liters of solution?
a) 3.4 M
b) 1.1 M
c) 24 M
d) M
e) M

39. 40. What is the concentration of NaOH in a
solution prepared be dissolving 12.4 g of
NaOH in enough water to give 190. mL
of solution?
a) M
b) x 10-3 M
c) M
d) M
e) none of these

40. 41. How many mL of 12.0 M HCl solution are required
to make 2.25 L of a 1.50 M solution of HCl?
a) mL
b) 281 mL
c) mL
d) mL
e) none of these
(X mL)(12.0M) = (2250 mL)(1.50M)
X mL = (2250 mL x 1.5M)/12.0M
X mL = 281 mL
BE CAREFUL WITH THE UNITS!

41. 42. If 25 mL of 0.050 molar sodium fluoride solution
is measured and enough water is added to
make 35 mL of solution. What is the molarity
of the new solution?
a) 35 M
b) M
c) M
d) M
e) none of these
(25mL)(0.05M) = (35mL)(X M)
X M = (25 x 0.05)/35
X M = M

42. 43. What mass of AgCl is formed when 47.8 mL
of M NaCl is treated with an excess of
aqueous silver nitrate?
a) g
b) g
c) g
d) g
e) none of these

43. 44. Which is a property of acids?
a) tastes sour
b) reacts with metals
c) can burn skin
d) has a pH below 7
e) all of the above

44. 45. A solution that has more H+ than OH- ions is:
a) basic and turns litmus paper red
b) acidic and turns litmus paper blue
c) acidic and turns litmus paper red
d) basic and turns litmus paper blue

45. 46. When you reach the neutralization point of a
laboratory titration, it is often indicated by:
a) an increase in the density of the solution
b) an absence of cations and anions in the
solution
c) equal numbers of cations and anions in the
d) an increase in the conductivity of the solution
e) a change in the color of the indicator

46. 47. Bases are identified as bases because they:
a) have more OH- ions than H+ ions
b) have more H+ ions than OH- ions
c) are neutral
d) have a pH between 0-7

47. 48. Water would best be described as
a) neutral
b) acidic
c) having the same number of OH- and H+ ions
d) alkaline
e) both a and c

48. 49. Which of the following is most likely an acid?
a) KOH
b) HCl
c) NaOH
d) C8H18
e) none of these

49. 50. Which of the following is most likely a base?
a) H2SO4
b) NaCl
c) NaOH
d) C4H10
e) none of these

50. 51. Cars emit nitrogen oxides, which can react with
water in the air to form nitric acid. What reagent
can remove nitric acid from the air?
a) HNO3
b) NO2
c) Mg(OH)2
d) CO2

51. 52. How many moles of Mg(OH)2 are required to
neutralize 200. L of 2.00 M HNO3(aq)?
Mg(OH)2(s) + 2HNO3(aq) → Ca(NO3)2(aq) + 6H2O(l)
a) moles
b) moles
c) moles
d) moles
e) none of these

52. 53. What volume of 0.235 M NaOH is required
to neutralize 37.4 mL of M HBr?
a) mL
b) mL
c) mL
d) mL
e) mL
Ratio between the acid and the base is 1:1.
For this situation, use MaVa=MbVb
(X mL)(0.235M) = (0.150M)(37.4mL)
X mL = (0.150 x 37.4)/0.235
X mL = 23.9 mL

53. 54. What is the pH of a 0.067 M solution of nitric
acid (HNO3 a strong acid)? a)
b) 1.5 c) d)
e) none of these
pH = -log(0.067) = 1.17

54. 55. If the pH of canned soda was measured with
a pH probe and determined to be What
is the hydrogen ion [H+]concentration?
a) M
b) x 10-4 M
c) M
d) M
e) x 10-3 M
[H+] = =

55. 56. Which one of the following acids contains
three hydrogen atoms per molecule?
a) nitric acid HNO3
b) phosphoric acid H3PO4
c) hydrofluoric acid HF
d) sulfuric acid H2SO4
e) hydrochloric acid HCl

56. 57. The net ionic reaction for the reaction between aqueous lead nitrate and aqueous potassium iodide is
a. Pb(NO3)2(aq) + KI(aq) → PbI2(s) + KNO3(aq)
b. Pb2+(aq) + NO3-(aq) + K+(aq) + I-(aq) → Pb2+(aq) + I-(aq) + K+(aq) + NO3-(aq)
c. Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + I-(aq) → PbI2(s) + 2K+(aq) + 2NO3-(aq)
d. Pb2+(aq) + 2I-(aq) → PbI2(s)
e. none of these

57. 58. What is the correct balanced complete ionic equation for the reaction of lead (II) nitrate with potassium chloride?
a.Pb(NO3)2(aq) + KCl(aq) → PbCl2(s) + KNO3(aq)
b. Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq) → Pb2+(aq) + 2Cl-(aq) +2 K+(aq) + 2NO3-(aq)
c. Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq) → Pb2+(aq) + 2Cl-(aq) + 2KNO3(s)
d. Pb2+(aq) + 2NO3-(aq) + K+(aq) + Cl-(aq) → PbCl2(s) + K+(aq) + NO3-(aq)
e. Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq) → PbCl2(s) + 2 K+(aq) + 2NO3-(aq)