Chemistry Semester 2 ReviewSummer School 2014-15 (2nd Review Guide)
Naming
1) Which of these elements does not exist as a diatomic molecule?
A) Ne B) FC) H D) I
2) What is the formula of aluminum oxide?
A) AlO B) Al2O C) Al3O D) AlO3E) Al2O3
3) Which of the following compounds has the formula KNO2?
A) potassium nitrate B) potassium nitride C) potassium nitrite D) potassium nitrogen oxide
4) 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
Reactions
5) What are the missing coefficients for the equation? Al2(SO4)3(aq) + KOH(aq) → Al(OH)3(aq) + K2SO4(aq)
A) 1,3,2,3 B) 2,12,4,6 C) 4,6,2,3 D) 1,6,2,3 E) 2,3,1,1
6) If you rewrite the following word equation as a balanced chemical equation, what is the coefficient and symbol for oxygen?
dicarbon hexahydride + oxygen → water + carbon dioxide
A) 7 OB) 3.5O2C) 4O3D) 14 O E) 7O2
7) 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 + 3H2E) H2 + AlCl3 → Al + 2HCl
C) Al + HCl3 → AlCl3 + H
8) 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
9) 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
10) In the chemical equation, H2O2(aq) → H2O(l) + O2(g), the H2O2 is a _____.
A) product B) reactant C) solid D) gas
11) 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
12) 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
13) 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)2E) 2KOH + 2BaCl2 → 2KCl2 + 2Ba(OH)2
B) KOH + BaCl → KCl + BaOH D) KOH + BaCl2 → KCl2 + BaOH
14) Write a balanced equation for the synthesis reaction that takes place when iron(III) oxide is formed from its constituent elements.
A) Fe2 + O3 → Fe2O3C) 4Fe + 3O2 → 2Fe2O3E) Fe + O3 → FeO3
B) 2Fe + 3O → Fe2O3D) 3Fe + O → Fe3O
15) 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 + O2D) PbO → Pb + O2
16) What is the balanced chemical equation for the single replacement that takes place between bromine and sodium iodide?
A) Br2 + NaI → NaBr2 + I C) Br2 + 2NaI → 2NaBr + 2I-E) Br + NaI2 → NaBr + I2
B) Br2 + 2NaI → 2NaBr + I2D) Br + NaI2 → NaBrI2
17) 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
18) 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
19) 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
20) 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 + NO3E) No reaction takes place because silver is less reactive than potassium.
C) Ag(s) + KNO3(aq) → AgKNO3
21) 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)3B) Co(OH)2C) LiCo3D) LiCl3E) Cl3OH
22) 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..
23) 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) 6F2C) F3D) 6F E) 3F2
24) 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) NaNO3B) NaSn C) Sn(CO3)2D) CNO3
25) In a combustion reaction, one of the reactants is _____.
A) hydrogen B) nitrogen C) oxygen D) a metal E) a binary ionic compound
Moles
26) All of the following are equal to Avogadro's number (6.02 x 1023) EXCEPT _____.
A) the number of molecules of nitrogen in 1 mol N2D) the number of molecules of carbon monoxide in 1 mol CO
B) the number of atoms of gold in 1 mol Au E) the number of atoms of bromine in 1 mol Br2
C) the number of formula units (molecules) of sodium phosphate in 1 mol Na3PO4
27) 94) How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?
A) 5 x (6.02 x 1023) B) 5 C) 35 D) 35 x (6.02 x 1023)
28) What is the molar mass of chromium(III) sulfate, Cr2(SO4)3?
A) 148.1 g B) 200.0 g C) 288.0 g D) 344.2 g E) 392.2 g
29) What is the molar mass of (NH4)2CO3?
A) 144 g B) 138 g C) 96 g D) 78 g E) 43 g
30) How many moles of tungsten atoms are there in 4.8 x 1025 atoms of tungsten?
A) 8.0 moles B) 8.0 x 101 moles C) 8.0 x 102 moles D) 1.3 x 10-2 moles E) 1.3 x 10-1 moles
31) How many atoms are there in 5.70 mol of hafnium?
A) 6.02 x 1023 atoms B) 1.06 x 1022 atoms C) 3.43 x 1023 atoms D) 1.06 x 1023 atoms E) 3.43 x 1024 atoms
32) How many ammonium ions, NH4+, are there in 5.0 mol (NH4)2S?
A) 3.4 x 102B) 3.0 x 1024C) 6.0 x 1024D) 1.5 x 1025E) 6.0 x 1025
33) How many bromide ions are there in 1.5 moles of MgBr2?
A) 5.0 x 10-24 ions B) 3.0 ions C) 2.8 x 102 ions D) 9.0 x 1023 ions E) 1.8 x 1024 ions
34) What is the number of moles in 15.0 g AsH3?
A) 0.19 B) 0.44 C) 2.3 D) 5.2 E) 1200
35) The chemical formula of aspirin is C9H8O4. What is the mass of 0.40 mol of aspirin?
A) 45 g B) 10.8 g C) 160 g D) 72 g \
36) How many moles are present in 3.58 x 1022 atoms of tungsten?
A) 0.0594 molesB) 3.50 moles C) 5.94 x 1044 molesD) 5.40 x 1055 moles
Stoich
37) Determine the percent composition of magnesium in magnesium chloride:
A) 25.5%B) 40.7%C) 50.0%D) 68.6%
38) In the reaction 2 CO + O2 → 2 CO2, what is the ratio of moles of oxygen used to moles of CO2 produced?
A) 1:1 B) 2:1 C) 1:2 D) 2:2
39) How many moles of Al are needed to react completely with 1.2 mol of FeO? 2Al + 3FeO → 3Fe + Al2O3
A) 1.2 mol B) 0.8 mol C) 1.6 mol D) 2.4 mol E) 4.8 mol
40) How many moles of glucose, C6H12O6, can be "burned" biologically when 10.0 mol of oxygen is available?
C6H12O6 + 6O2 → 6CO2 + 6H2O
A) 0.938 mol B) 1.67 mol C) 53.3 mol D) 60.0 mol E) 301 mol
41) How many moles of H3PO4 are produced when 71.0 g P4O10 reacts completely to form H3PO4?
P4O10 + 6H2O → 4H3PO4
A) 0.063 5 mol B) 1.00 mol C) 4.00 mol D) 16.0 mol E) 98.0 mol
42) How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water.)
Be + 2H2O → Be(OH)2 + H2
A) 4.00 g B) 36.0 g C) 162 g D) 324 g E) 648 g
43) When two substances react to form products, the reactant which is left over is called the _____.
A) determining reagent B) limiting reagent C) excess reagent D) catalytic reagent E) reactive reagen
44) 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
45) 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
46) 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
47) 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
48) How many liters of chlorine gas, at STP, can be produced when 0.98 L of HCl react with excess O2?
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
49) 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
50) 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
51) When two substances react to form products, the reactant which is used up is called the _____.
A) determining reagent B) limiting reagent C) excess reagent D) catalytic reagent E) reactive reagent
52) 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 Fe2O3 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 CO2 will be formed.
C) The limiting reagent is Fe2O3 and 24 mol Fe will be formed.
53) 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
54) Metallic copper is formed when aluminum reacts with copper(II) sulfate in this limiting problem. 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
55) The reactant present in the smallest amount is _____ the limiting reactant.
A) always B) sometimes C) never
56) 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
57) Lead nitrate can be decomposed by heating. What is the percent yield of the decomposition reaction if 9.9 g Pb(NO3)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%
58) 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 H2 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
59) 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%
GASES
60) Which of the following is NOT one of the assumptions of kinetic theory?
A) Gases consist of hard spherical particles. D) Only small attractive and repulsive forces exists between gas particles.
B) Particles in a gas are assumed to have an insignificant volume. E) none of the above
C) All gas particles move in constant random motion.
61) Decreasing the volume of a given amount of gas at constant temperature causes the pressure to increase because
A) once there are fewer molecules C) the molecules are moving faster
B) the molecules are striking a smaller area with the same force D) there are more molecules
62) According to Dalton’s Law, the total pressure in the system is equal to:
A) the product of the partial pressuresC) the difference of the partial pressures
B) the sum of the partial pressuresD) the sum of the partial temperatures
63) If the volume of a container holding a gas is reduced, what will happen to the pressure within the container?
A) The pressure will increase. B) The pressure will not change. C) The pressure will decrease.
64) A mixture of four gases exerts a total pressure of 860 mm Hg. Gases A and B each exert 220 mm Hg.Gas C exerts 110 mm Hg. What pressure is exerted by gas D?
A. 165 mm HgB. 530 mm HgC. 310 mm Hg D. 860 mm Hg
65) Why does an aerosol can become cooler when gas is released?
A) because the propellant expands C) because the product expands within the can
B) because the propellant contracts D) because the volume of the can decreases
66) If a capped syringe is plunged into cold water, in which direction will the syringe piston slide?
A) in B) outC) No sliding will occur.
67) If a capped syringe is heated, in which direction will the syringe plunger move?
A) out B) in C) The plunger will not move.
68) Boyle's law states that _____.
A) the volume of a gas varies inversely with pressure C) the temperature of a gas varies inversely with pressure
B) the volume of a gas varies directly with pressure D) the temperature of a gas varies directly with pressure
69) Charles' law states that _____.
A) the pressure of a gas is inversely proportional to its temperature in kelvins
B) the volume of a gas is directly proportional to its temperature in kelvins
C) the pressure of a gas is directly proportional to its temperature in kelvins
D) the volume of a gas is inversely proportional to its temperature in kelvins
70) Why does the pressure inside a container of gas increase if more gas is added to the container?
A) because there is a corresponding increase in the number of particles striking an area of the wall of the container per unit time
B) because there is a corresponding increase in the temperature
C) because there is a corresponding decrease in volume
D) because there is a corresponding increase in the force of the collisions between the particles and the walls of the container
71) Why does air leave a tire when the tire valve is opened?
A) because the pressure outside the tire is lower than the pressure inside the tire
B) because the pressure outside the tire is greater than the pressure inside the tire
C) because the temperature is higher outside the tire than inside the tire
D) because there are more gas particles outside the tire than inside the tire
72) 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 moleculesD) there are more molecules
73) 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.
74) 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.
75) 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.
76) Standard pressure is exactly
A) 1 atmB) 101.325 atmC) 273 atmD) 760 atm
77) Convert the pressure 0.840 atm to mmHg.
A) 365 mmHgB) 437 mmHgC) 638 mmHgD) 780 mmHg
78) 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
79) A sample of gas occupies 40.0 mL at -123oC. What volume does the sample occupy at 27oC?
A) 182 mL B) 8.80 mL C) 80.0 mL D) 20.0 mL
80) At 710. mmHg a sample of nitrogen gas occupies 625 mL. What volume does the gas occupy if the temperature remains constant and the pressure increases to 760. mmHg?
A) 135 mLB) 584 mLC) 600 mLD) 609 mL
81) At what temperature in °C will 250.0 mL sample of gas originally at 25°C have a volume of 350.0 mL?
A) 35.0°CB) 144°CC) 212 °CD) 417°C
82) The combined gas law relates which of these?
A) pressure and volume only C) volume and temperature only
B) temperature and pressure only D) temperature, pressure, and volume
Molarity
83) 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
84) How many mL of 3M HCl are needed to make 300 mL of 0.1M HCl?
A) 10 mL B) 100 mL C) 90 mL D) 9 mL E) 30 mL
85) In which of the following is the solution concentration expressed in terms of molarity?
A) 10 g of solute/1000 g of solution C) 10 mL of solute/1 L of solution E) 10 mol of solute/1 kg of solution
B) 10 g of solute/1000 mL of solution D) 10 mol of solute/1 L of solution
Liquids-Solids & IM Forces
86) Which of the following covalent bonds is the most polar?
A) C-C B) C-H C) C-Cl D) C-BrE) C-S
87) Which of the following compounds has the strongest intermolecular forces?
A) CBr4B) CO C) I2D) NH3
88) The bonds between the hydrogen and oxygen atoms between different water molecules are _____.
A) hydrogen bonds B) ionic bonds C) nonpolar covalent bonds D) polar covalent bonds
Specific heat
89) How much heat does it take to warm 16.0 g of pure water from 90.0oC to 100.0oC? (specific heat of water= 4.18 J/g oC)
A) 66.9 joules B) 669 joules C) 160 joules D) 16.0 joules
90) How much heat does it take to vaporize 36.0 g of pure water? (heat of vaporization water= 2260 J/g)
A) 62.8 JB) 81400 JC) 8140000 JD) 5530000 j
Solutions SOLUBILITY
91) What is the term for the dissolving medium in a solution?
A) solvent B) solute C) solvator D) emulsifier
92) What occurs in solvation?
A) Solute ions separate from solvent molecules. C) Solvent molecules bind covalently to solute molecules.
B) Solvent molecules surround solute ions. D) Ionic compounds are formed.
93) What is the maximum amount of KNO3 that can dissolve in 150 g of water at 60oC?
A) 27.5 g B) 55 g C) 110 g D) 165 g (go ahead, look on a solubility table below)
94) Which of the following factors increase the solubility of a gas dissolved in a solvent?
A) high pressure and high temperature C) low pressure and high temperature
B) high pressure and low temperatureD) low pressure and low temperature
95) Which of the following operations usually makes a substance dissolve faster in a solvent?
A) agitation B) raising the temperature C) crushing the substance to a powderD) all of the above
96) Which of the following is true of the colligative properties?
A) the boiling point of a solution is lower than the pure solvent
B) the freezing point of a pure solvent is lower than that of a solution
C) the boiling point of a pure solvent is higher than that of the solution
D) the freezing point of a solution is lower than that of a pure solvent
97) How does solubility generally vary as the temperature increases?
A) solubility decreases B) solubility increases C) solubility remains the same
98) What is the maximum amount of KClO3 that can dissolve in 200 g of water at 20oC?
A) 10 g B) 20 g C) 34 g D) 68 g (go ahead, look on a solubility table)
99) Which of the following factors both affect the solubility of a particular substance?
A) temperature and the nature of solute and solvent C) particle size and degree of mixing
B) temperature and degree of mixing D) particle size and temperature
100) Increasing the temperature of a solution will generally _____.
A) increase the rate at which a solute dissolves C) both A. and B.
B) increase the amount of solute that dissolves D) neither A. nor B.
CP SEMESTER 2 REVIEW ANSWERS 2011-12
1) Answer: A
2) Answer: E
3) Answer: C
4) Answer: D
5) Answer: D
6) Answer: E
7) Answer: B
8) Answer: C
9) Answer: C
10) Answer: B
11) Answer: C
12) Answer: A
13) Answer: C
14) Answer: C
15) Answer: B
16) Answer: B
17) Answer: C
18) Answer: A
19) Answer: B
20) Answer: E
21) Answer: A
22) Answer: B
23) Answer: E
24) Answer: A
25) Answer: C
26) Answer: E
27) Answer: C
28) Answer: E
29) Answer: C
30) Answer: B
31) Answer: E
32) Answer: C
33) Answer: E
34) Answer: A
35) Answer: D
36) Answer: A
37) Answer: A
38) Answer: C
39) Answer: B
40) Answer: B
41) Answer: B
42) Answer: C
43) Answer: C
44) Answer: B
45) Answer: C
46) Answer: A
47) Answer: B
48) Answer: B
49) Answer: B
50) Answer: B
51) Answer: B
52) Answer: A
53) Answer: B
54) Answer: B
55) Answer: B
56) Answer: C
57) Answer: E
58) Answer: D
59) Answer: D
60) Answer: D
61) Answer: B
62) Answer: B
63) Answer: A
64) Answer: C
65) Answer: A
66) Answer: A
67) Answer: A
68) Answer: A
69) Answer: B
70) Answer: A
71) Answer: A
72) Answer: C
73) Answer: A
74) Answer: C
75) Answer: A
76) Answer: A
77) Answer: C
78) Answer: D
79) Answer: C
80) Answer: B
81) Answer: B
82) Answer: D
83) Answer: A
84) Answer: A
85) Answer: D
86) Answer: C
87) Answer: D
88) Answer: A
89) Answer: B
90) Answer: B
91) Answer: A
92) Answer: B
93) Answer: C
94) Answer: B
95) Answer: D
96) Answer: D
97) Answer: B
98) Answer: B
99) Answer: A
100) Answer: C