Chemistry Semester 2 Review for Summer School 2014-15
Directions: Answer the following multiple choice questions on the bubble sheet provided.
1) What is the formula of sodium nitride?
A) NaN
B) Na2N
C) Na3N
D) NaN3
E) Na2N3
2) What is the formula of aluminum oxide?
A) AlO
B) Al2O
C) Al3O
D) AlO3
E) Al2O3
3) What is the formula for potassium sulfide?
A) KS
B) K2S
C) KS2
D) K2S2
4) Which of the following compounds has the formula KNO 2?
A) potassium nitrate
B) potassium nitride
C) potassium nitrite
D) potassium nitrogen oxide
5) What is the name of the ionic compound formed from strontium and phosphorus?
A) strontium phosphorus B) strontium phosphoride C) strontium phosphate D) strontium phosphide E) strontide phosphate
6) Which of these elements does not exist as a diatomic molecule?
A) Ne
B) F
C) H
D) I
7) The shape of the carbon tetrachloride molecule is called _____.
A) tetrahedral
B) square
C) four-cornered
D) planar
8) Which of the following covalent bonds is the most polar?
A) C-C
B) C-H
C) C-Cl
D) C-Br
E) C-S
9) If you rewrite the following word equation as a balanced chemical equation, what is the coefficient and symbol for fluorine?
nitrogen trifluoride → nitrogen + fluorine
A) 3F
B) 6F2
C) F3
D) 6F
E) 3F2
10) Aluminum chloride and bubbles of hydrogen gas are produced when metallic aluminum is placed in hydrochloric acid. What
is the balanced equation for this reaction?
A) H + AlCl → Al + HCl
D) Al + 2HCl → AlCl2 + H2
B) 2Al + 6HCl → 2AlCl3 + 3H2
E) H2 + AlCl3 → Al + 2HCl
C) Al + HCl3 → AlCl3 + H
11) Chemical equations must be balanced to satisfy the _____.
A) law of definite proportions
C) law of conservation of mass
B) law of multiple proportions
D) principle of Avogadro
12) Symbols used in equations, together with the explanations of the symbols, are shown below. Which set is correct?
A) (g), grams B) (l), liters C) (aq), dissolved in water D) (p), solid product E) (s), stuff
13) In the chemical equation, H2O2(aq) → H2O(l) + O2(g), the H2O2 is a _____.
A) product
B) reactant
C) solid
D) gas
14) Which of the following is the correct equation for the reaction that takes place when solid phosphorus combines with oxygen
gas to form diphosphorus pentoxide?
A) P(s) + O2(g) → PO2(g)
D) P2O5 → P2(s) + O2(g)
E) P2(s) + O5(g) → P2O5(g)
B) P(s) + O(g) → P5O2(g)
C) P(s) + O2(g) → P2O5
15) In every balanced chemical equation, each side of the equation has the same number of _____.
A) atoms
B) molecules
C) moles
D) coefficients E) subscripts
16) When potassium hydroxide and barium chloride react, potassium chloride and barium hydroxide are formed. The balanced
equation for this reaction is _____.
A) KH + BaCl → KCl + BaH
C) 2KOH + BaCl2 → 2KCl + Ba(OH)2
E) 2KOH + 2BaCl2 → 2KCl2 + 2Ba(OH)2
B) KOH + BaCl → KCl + BaOH D) KOH + BaCl2 → KCl2 + BaOH
17) Write a balanced equation for the synthesis reaction that takes place when iron(III) oxide is formed from its constituent
elements.
A) Fe2 + O3 → Fe2O3
C) 4Fe + 3O2 → 2Fe2O3
E) Fe + O3 → FeO3
B) 2Fe + 3O → Fe2O3
D) 3Fe + O → Fe3O
18) Write a balanced equation to represent the decomposition of lead(IV) oxide.
A) PbO2 → Pb + 2O
C) Pb2O → 2Pb + O
E) 2PbO → 2Pb + O2
B) PbO2 → Pb + O2
D) PbO → Pb + O2
19) What is the balanced chemical equation for the single replacement that takes place between bromine and sodium iodide?
A) Br2 + NaI → NaBr2 + I
C) Br-2 + 2NaI → 2NaBr + 2IE) Br + NaI2 → NaBr + I2
B) Br2 + 2NaI → 2NaBr + I2
D) Br + NaI2 → NaBrI2
20) What are the correct formulas and coefficients for the products of this double-replacement reaction?
RbOH + H3PO4 →
A) Rb(PO4)3 + H2O B) RbPO4 + 2H2O C) Rb3PO4 + 3H2O D) H3Rb + PO4OH E) 3RbH + H2OPO4
21) The equation 2C3H7OH + 9O2 → 6CO2 (g) + 8H2O (g) is an example of which type of reaction? →
A) combustion
B) single-replacement
C) double-replacement
D) decomposition
22) In order to predict whether or not a single-replacement reaction takes place, we need to consult a chart which shows the __.
A) periodic table
D) ionic charges of representative elements
B) activity series of metals
E) formulas and names of common metal ions having an ionic charge greater than 1.
C) common polyatomic ions
23) Use the activity series of metals to write a balanced chemical equation for the following single replacement reaction:
Ag(s) + KNO3(aq) →
A) Ag(s) + KNO3(aq) → AgNO3 + K
D) Ag(s) + KNO3(aq) → Ag + K + NO3
B) Ag(s) + KNO3(aq) → AgK + NO3
E) No reaction takes place because silver is less reactive than potassium.
C) Ag(s) + KNO3(aq) → AgKNO3
24) A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of
the products of this reaction would be _____.
A) Co(OH)3
B) Co(OH)2
C) LiCo3
D) LiCl3
E) Cl3OH
25) How do you know the following reaction occurs and is not a "No Reaction"?
Ni(NO3)2(aq) + K2S(aq) → NiS(s) + 2KNO3(aq)
A) A gas is formed.
D) Ionic compounds are products.
B) A solid precipitate is formed.
E) Heat is required.
C) Ionic compounds are reactants..
26) A double-replacement reaction takes place when aqueous Na2CO3 reacts with aqueous Sn(NO3)2. You would expect one of
the products of this reaction to be _____.
A) NaNO3
B) NaSn
C) Sn(CO3)2
D) CNO3
27) In a combustion reaction, one of the reactants is _____.
A) hydrogen
B) nitrogen
C) oxygen
D) a metal
28) What is the molar mass of chromic sulfate, Cr2(SO4)3?
A) 148.1 g
B) 200.0 g
C) 288.0 g
29) What is the molar mass of (NH4)2CO3?
A) 144 g
B) 138 g
C) 96 g
E) a binary ionic compound
D) 344.2 g
D) 78 g
E) 43 g
E) 392.2 g
30) What is the volume, in liters, of 0.500 mol of C3H8 gas at STP?
A) 0.0335 L
B) 11.2 L
C) 16.8 L
D) 22.4 L
E) 5.60 L
31) What is the number of moles in 500 L of He gas at STP?
A) 0.05 mol
B) 0.2 mol
C) 20 mol
D) 90 mol
E) 10 000 mol
32) How many liters of oxygen at STP are required to react completely with 3.6 liters of hydrogen At STP to form water?
2H2(g) + O2(g) → 2H2O(g)
A) 1.8 L
B) 3.6 L
C) 2.0 L
D) 2.4 L
33) How many liters of NH3 are needed to react completely with 30.0 L of NO (at STP)?
4NH3(g) + 6NO(g) → 5N2(g) + 6H2O(g)
A) 5.0 L
B) 20.0 L
C) 7.5 L
D) 120.0 L
E) 180.0 L
34) How many liters of chlorine gas, at STP, can be produced when 0.98 L of HCl react with excess O 2?
4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(g)
A) 0.98 L
B) 0.49 L
C) 3.9 L
D) 2.0 L
E) 0.25 L
35) Iron(III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe2O3 are formed when 16.7 g of
Fe reacts completely with oxygen?
4Fe(s) + 3O2(g) → 2Fe2O3(s)
A) 12.0 g
B) 23.9 g
C) 47.8 g
D) 95.6 g
E) 267 g
36) Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate
would be formed if 250 g H2SO4 completely reacted with aluminum?
2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
A) 0.85 g
B) 290 g
C) 450 g
D) 870 g
E) 2600 g
37) Which statement is true if 12 mol CO and 12 mol Fe2O3 are allowed to react?
3CO(g) + Fe2O3(s) → 2Fe(s) + 3CO2(g)
A) The limiting reagent is CO and 8.0 mol Fe will be formed. D) The limiting reagent is Fe 2O3 and 36 mol CO2 will be formed.
B) The limiting reagent is CO and 3.0 mol CO2 will be formed. E) The limiting reagent is Fe and 18 mol CO 2 will be formed.
C) The limiting reagent is Fe2O3 and 24 mol Fe will be formed.
38) What is the maximum number of grams of PH3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to
form PH3?
P4(g) + 6H2(g) → 4PH3(g)
A) 0.43 g
B) 6.8 g
C) 270 g
D) 45 g
E) 99 g
39) Metallic copper is formed when aluminum reacts with copper(II) sulfate. How many grams of metallic copper can be obtained
when 54.0 g of Al reacts with 319 g of CuSO4?
2Al + 3CuSO4 → Al2(SO4)3 + 3Cu
A) 21.2
g B) 127 g
C) 162 g
D) 381 g E) 957 g
40) The reactant present in the smallest amount is _____ the limiting reactant.
A) always
B) sometimes
C) never
41) When an equation is used to calculate the amount of product that will form during a reaction, then the value obtained is called
the _____.
A) actual yield
B) percent yield
C) theoretical yield
D) minimum yield
E) percent composition
42) Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO 3)2 is
heated to give 5.5 actual grams of PbO?
2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g)
A) 18%
B) 44%
C) 56%
D) 67%
E) 82%
43) Hydrogen gas is produced when zinc reacts with hydrochloric acid. If the actual yield of this reaction is 85%, how many
grams of zinc are needed to produce 112 L of H 2 at STP?
Zn(s) + 2HCl(aq) → ZnCl2(s) + H2(g)
A) 2.2 g
B) 95 g
C) 180 g
D) 280 g
E) 380 g
44) In a particular reaction between copper metal and silver nitrate, 12.7 g Cu produced 38.1 g Ag. What is the percent yield of
silver in this reaction?
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
A) 29.4%
B) 56.7%
C) 77.3%
D) 88.2%
E) 176%
45) What is the number of moles of solute in 250 mL of a 0.4M solution?
A) 0.1 mol
B) 0.16 mol
C) 0.62 mol
D) 1.6 mol
E) 1 mol
46) Increasing the volume of a given amount of gas at constant temperature causes the pressure to decrease because _____.
A) the molecules are striking a larger area with the same force
C) the molecules are moving more slowly
B) there are fewer molecules
D) there are more molecules
47) What happens to the temperature of a gas when it is put under increased pressure?
A) The temperature increases.
B) The temperature does not change.
C) The temperature increases.
48) What happens to the pressure of a gas inside a container if the temperature of the gas is lowered?
A) The pressure increases.
B) The pressure does not change.
C) The pressure decreases.
49) Which of these changes would NOT cause an increase in the pressure of a gaseous system?
A) The container is made larger.
C) The temperature is increased.
B) Additional amounts of the same gas are added to the container.
D) Another gas is added to the container.
50) A gas occupies a volume of 0.7 L at 10.1 kPa. What volume will the gas occupy at 101 kPa?
A) 7 L
B) 4 L
C) 0.7 L
D) 0.07 L
51) A beaker containing 80 grams of lead (II) nitrate, in 100 grams of water has a
temperature of 30 °C. Approximately how many grams of the salt are
undissolved, on the bottom of the beaker?
A) 80 grams
B) 66 grams
C) 14 grams
D) 20 grams
52) When 50 rams of potassium chloride, is dissolved in 100 grams of water at
50°C, the solution can be correctly described as:
A) Saturated
B) Supersaturated
C) Unsaturated
53) Which salt is LEAST soluble at 50 °C?
A)
KNO3
B) Ce2(SO4)3
C) K2Cr2O7
D) KClO3
54) At approximately what temperature does the solubility of sodium chloride,
NaCl, match the solubility of potassium dichromate, K2Cr2O7?
A) 60°C
B) 30°C
C) 50°C
D) 83°C
55) When 20 grams of potassium chlorate, KCLO3, is dissolved in 100 grams of water at 80°C, the solution can be correctly
described as:
A) Supersaturated
B) Saturated
C) Unsaturated
Note: The final exam may include other topics, so please remember
to look over your review sheet and refer to your notes and text for
additional practice questions.