Chapter 3 Terms

CCalcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its molar mass.

A) 118.15 g/mol

B) 99.15 g/mol

C) 78.07 g/mol

D) 59.08 g/mol

E) 50.01 g/mol

BCalculate the molar mass of tetraphosphorus decaoxide, P4O10, a corrosive substance which can be used as a drying agent.

A) 469.73 g/mol

B) 283.89 g/mol

C) 190.97 g/mol

D) 139.88 g/mol

E) 94.97 g/mol

CCalculate the molar mass of rubidium carbonate, Rb2CO3.

A) 340.43 g/mol

B) 255.00 g/mol

C) 230.94 g/mol

D) 145.47 g/mol

E) 113.48 g/mol

BCalculate the molar mass of (NH4)3AsO4.

A) 417.80 g/mol

B) 193.03 g/mol

C) 165.02 g/mol

D) 156.96 g/mol

E) 108.96 g/mol

BAluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and manufacture of antiperspirants. Calculate its molar mass.

A) 450.06 g/mol

B) 342.15 g/mol

C) 315.15 g/mol

D) 278.02 g/mol

E) 74.98 g/mol

BCalculate the molar mass of Ca(BO2)2·6H2O.

A) 273.87 g/mol

B) 233.79 g/mol

C) 183.79 g/mol

D) 174.89 g/mol

E) 143.71 g/mol

EMagnesium fluoride is used in the ceramics and glass industry. What is the mass of 1.72 mol of magnesium fluoride?

A) 43.3 g

B) 62.3 g

C) 74.5 g

D) 92.9 g

E) 107 g

ASodium bromate is used in a mixture which dissolves gold from its ores. Calculate the
mass in grams of 4.68 mol of sodium bromate.A) 706 g

B) 482 g

C) 383 g

D) 32.2 g

E) 0.0310 g

BWhat is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

A) 4.00 x 10^2 g

B) 25.0 g

C) 17.0 g

D) 4.00 x 10^-2 g

E) 2.50 x 10^-3 g

DCalculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2.

A) 3.28 mol

B) 2.32 mol

C) 0.431 mol

D) 0.305 mol

E) 0.200 mol

EPhosphorus pentachloride, PCl5, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of PCl5.

A) 5.38 mol

B) 3.55 mol

C) 0.583 mol

D) 0.282 mol

E) 0.186 mol

DAluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

A) 2.377 mol

B) 2.146 mol

C) 1.105 mol

D) 0.4660 mol

E) 0.4207 mol

BCalculate the number of oxygen atoms in 29.34 g of sodium sulfate, Na2SO4.

A) 1.244 x 10^23 O atoms

B) 4.976 x 10^23 O atoms

C) 2.409 x 10^24 O atoms

D) 2.915 x 10^24 O atoms

E) 1.166 x 10^25 O atoms

DPotassium dichromate, K2Cr2O7, is used in tanning leather, decorating porcelain and waterproofing fabrics. Calculate the number of chromium atoms in 78.82 g of K2Cr2O7.

A) 9.490 x 10^25 Cr atoms

B) 2.248 x 10^24 Cr atoms

C) 1.124 x 10^24 Cr atoms

D) 3.227 x 10^23 Cr atoms

E) 1.613 x 10^23 Cr atoms

CSulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 x 10^20 molecules of SO3.

A) 6.06 x 10^-4 g

B) 2.91 x 10^-2 g

C) 4.85 x 10^-2 g

D) 20.6 g

E) 1650 g

ECalculate the mass in grams of 8.35 x 10^22 molecules of CBr4.

A) 0.0217 g

B) 0.139 g

C) 7.21 g

D) 12.7 g

E) 46.0 g

CThe number of hydrogen atoms in 0.050 mol of C3H8O3 is

A) 3.0 x 10^22 H atoms

B) 1.2 x 10^23 H atoms

C) 2.4 x 10^23 H atoms

D) 4.8 x 10^23 H atoms

E) none of these choices is correct

BCopper(II) sulfate pentahydrate, CuSO4·5H2O, is used as a fungicide and algicide. Calculate the mass of oxygen in 1.000 mol of CuSO4·5H2O.

A) 249.7 g

B) 144.0 g

C) 96.00 g

D) 80.00 g

E) 64.00 g

CLead(II) nitrate is a poisonous substance which has been used in the manufacture of special explosives and as a sensitizer in photography. Calculate the mass of lead in 139 g of Pb(NO3)2.

A) 107 g

B) 90.8 g

C) 87.0 g

D) 83.4 g

E) 62.6 g

DHousehold sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass?

A) 26.7 %

B) 33.3 %

C) 41.4 %

D) 42.1 %

E) 52.8 %

AGadolinium oxide, a colorless powder which absorbs carbon dioxide from the air, contains 86.76 mass % Gd. Determine its empirical formula.

A) Gd2O3

B) Gd3O2

C) Gd3O4

D) Gd4O3

E) GdO

BHydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O.
Determine its empirical formula.A) HNO

B) H2NO2

C) HN6O16

D) HN16O7

E) H2NO3

BHydroxylamine nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass O. If its molar mass is between 94 and 98 g/mol, what is its molecular formula?

A) NH2O5

B) N2H4O4

C) N3H3O3

D) N4H8O2

E) N2H2O4

EA compound of bromine and fluorine is used to make UF6, which is an important chemical in processing and reprocessing of nuclear fuel. The compound contains 58.37 mass percent bromine. Determine its empirical formula.

A) BrF

B) BrF2

C) Br2F3

D) Br3F

E) BrF3

DA compound containing chromium and silicon contains 73.52 mass percent chromium. Determine its empirical formula.

A) CrSi3

B) Cr2Si3

C) Cr3Si

D) Cr3Si2

E) Cr2S

BAlkanes are compounds of carbon and hydrogen with the general formula CnH2n+2. An alkane component of gasoline has a molar mass of between 125 and 130 g/mol. What is the value of n for this alkane?

A) 4

B) 9

C) 10

D) 13

E) 14

cTerephthalic acid, used in the production of polyester fibers and films, is composed of
carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. What is its empirical
formula?A) C2H3O4

B) c3h4o2

C) C4H3O2

D) C5H12O4

E) c2h2o

eTerephthalic acid, used in the production of polyester fibers and films, is composed of
carbon, hydrogen, and oxygen. When 0.6943 g of terephthalic acid was subjected to
combustion analysis it produced 1.471 g CO2 and 0.226 g H2O. If its molar mass is
between 158 and 167 g/mol, what is its molecular formula?A) c4h6o7

B) c6h8O5

C) c7h12O4

D) C4H3O2

E) C8H6O4

dHydroxylamine hydrochloride is a powerful reducing agent which is used as a polymerization catalyst. It contains 5.80 mass % H, 20.16 mass % N, 23.02 mass % O, and 51.02 mass % Cl. What is its empirical formula?

A) H2N7O8Cl18

B) H2N2O2Cl

C) HN3O4Cl9

D) H4NOCl

E) H4NOCl2

CIn the combustion analysis of 0.1127 g of glucose (C6H12O6), what mass, in grams, of CO2 would be produced?

A) 0.0451 g

B) 0.0825 g

C) 0.1652 g

D) 0.4132 g

E) 1.466 g

aBalance the following equation:

B2O3(s) + HF(l) > BF3(g) + H2O(l)

A) B2O3(s) + 6HF(l) > 2BF3(g) + 3H2O(l)

B) B2O3(s) + H6F6(l) > B2F6(g) + H6O3(l)

C) B2O3(s) + 2HF(l) > 2BF3(g) + H2O(l)

D) B2O3(s) + 3HF(l) > 2BF3(g) + 3H2O(l)

E) B2O3(s) + 6HF(l) > 2BF3(g) + 6H2O(l)

bBalance the following equation:

UO2(s) + HF(l) > UF4(s) + H2O(l)

A) UO2(s) + 2HF(l) > UF4(s) + H2O(l)

B) UO2(s) + 4HF(l) > UF4(s) + 2H2O(l)

C) UO2 (s) + H4F4(l) > UF4 (s) + H4O2(l)

D) UO2(s) + 4HF(l) > UF4(s) + 4H2O(l)

E) UO2(s) + 8HF(l) > 2UF4(s) + 4H2O(l)

CBalance the following equation for the combustion of benzene:

C6H6(l) + O2(g) > H2O(g) + CO2(g)

A) C6H6(l) + 9O2(g) > 3H2O(g) + 6CO2(g)

B) C6H6(l) + 9O2(g) > 6H2O(g) + 6CO2(g)

C) 2C6H6(l) + 15O2(g) > 6H2O(g) + 12CO2(g)

D) C6H6(l) + 15O2(g) > 3H2O(g) + 6CO2(g)

E) 2C6H6(l) + 9O2(g) > 6H2O(g) + 12CO2(g)

bBalance the following equation:

c8h18o3(l) + O2(g) > H2O(g) + CO2(g)

A) C8H18O3(l) + 8O2(g) > 9H2O(g) + 8CO2(g)

B) C8H18O3(l) + 11O2(g) > 9H2O(g) + 8CO2(g)

C) 2C8H18O3(l) + 22O2(g) > 9H2O(g) + 16CO2(g)

D) C8H18O3(l) + 13O2(g) > 18H2O(g) + 8CO2(g)

E) 2C8H18O3(l) + 17O2(g) > 18H2O(g) + 16CO2(g)

dBalance the following equation:

Ca3(PO4)2(s) + SiO2(s) + C(s) > CaSiO3(s) + CO(g) + P4(s)

A) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) > 3CaSiO3(s) + 8CO(g) + P4(s)

B) Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) > 3CaSiO3(s) + 14CO(g) + P4(s)

C) Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) > 3CaSiO3(s) + 8CO(g) + 2P4(s)

D) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) > 6CaSiO3(s) + 10CO(g) + P4(s)

E) 2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) > 6CaSiO3(s) + 10CO(g) + 4P4(s)

cSulfur dioxide reacts with chlorine to produce thionyl chloride (used as a drying agent for inorganic halides) and dichlorine oxide (used as a bleach for wood, pulp and textiles).

SO2(g) + 2Cl2(g) > SOCl2(g) + Cl2O(g)

If 0.400 mol of Cl2 reacts with excess SO2, how many moles of Cl2O are formed?

A) 0.800 mol

B) 0.400 mol

C) 0.200 mol

D) 0.100 mol

E) 0.0500 mol

BAluminum will react with bromine to form aluminum bromide (used as an acid catalyst in
organic synthesis).Al(s) + Br2(l) > Al2Br6(s) [unbalanced]

How many moles of Al are needed to form 2.43 mol of Al2Br6?

A) 7.29 mol

B) 4.86 mol

C) 2.43 mol

D) 1.62 mol

E) 1.22 mol

dAmmonia will react with fluorine to produce dinitrogen tetrafluoride and hydrogen
fluoride (used in production of aluminum, in uranium processing, and in frosting of light
bulbs).2NH3(g) + 5F2(g) > N2F4(g) + 6HF(g)

How many moles of NH3 are needed to react completely with 13.6 mol of F2?

A) 34.0 mol

B) 27.2 mol

C) 6.80 mol

D) 5.44 mol

E) 2.27 mol

cAmmonia, an important source of fixed nitrogen that can be metabolized by plants, is produced using the Haber process in which nitrogen and hydrogen combine.

N2(g) + 3H2(g) > 2NH3(g)

How many grams of nitrogen are needed to produce 325 grams of ammonia?

A) 1070 g

B) 535 g

C) 267 g

D) 178 g

E) 108 g

cHow many grams of sodium fluoride (used in water fluoridation and manufacture of insecticides) are needed to form 485 g of sulfur tetrafluoride?

3SCl2(l) + 4NaF(s) > SF4(g) + S2Cl2(l) + 4NaCl(s)

A) 1940 g

B) 1510 g

C) 754 g

D) 205 g

E) 51.3 g

aHow many grams of oxygen are needed to react completely with 200.0 g of ammonia,
NH3?4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g)

A) 469.7 g

B) 300.6 g

C) 250.0 g

D) 3.406 g

E) 2.180 g

dPhosphine, an extremely poisonous and highly reactive gas, will react with oxygen to form tetraphosphorus decaoxide and water.

PH3(g) + O2(g) P4O10(s) + H2O(g) [unbalanced]

Calculate the mass of P4O10(s) formed when 225 g of PH3 reacts with excess oxygen.

A) 1880 g

B) 940. g

C) 900. g

D) 470 g

E) 56.3 g

cPotassium chlorate (used in fireworks, flares and safety matches) forms oxygen and potassium chloride when heated.

KClO3(s) > KCl(s) + O2(g) [unbalanced]

How many grams of oxygen are formed when 26.4 g of potassium chlorate is heated?

A) 223 g

B) 99.1 g

C) 10.3 g

D) 6.86 g

E) 4.60 g

eAluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl3.

What mass of chlorine gas is needed to react completely with 163 g of aluminum?

A) 214 g

B) 245 g

C) 321 g

D) 489 g

E) 643 g

aLead(II) sulfide was once used in glazing earthenware. It will also react with hydrogen
peroxide to form lead(II) sulfate and water. How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II) sulfide?A) 151 g

B) 123 g

C) 50.3 g

D) 37.7 g

E) 9.41 g

aAluminum oxide (used as an adsorbent or a catalyst for organic reactions) forms when
aluminum reacts with oxygen.4Al(s) + 3O2(g) > 2Al2O3(s)

A mixture of 82.49 g of aluminum ( M = 26.98 g/mol) and 117.65 g of oxygen ( M = 32.00 g/mol) is allowed to react. What mass of aluminum oxide ( = 101.96 g/mol) can be formed?

A) 155.8 g

B) 200.2 g

C) 249.9 g

D) 311.7 g

E) 374.9 g

eAluminum reacts with oxygen to produce aluminum oxide which can be used as an
adsorbent, desiccant or catalyst for organic reactions.4Al(s) + 3O2(g) > 2Al2O3(s)

A mixture of 82.49 g of aluminum ( M = 26.98 g/mol) and 117.65 g of oxygen ( M = 32.00 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

A) Oxygen is the limiting reactant; 19.81 g of aluminum remain.

B) Oxygen is the limiting reactant; 35.16 g of aluminum remain.

C) Aluminum is the limiting reactant; 16.70 g of oxygen remain.

D) Aluminum is the limiting reactant; 35.16 g of oxygen remain.

E) Aluminum is the limiting reactant; 44.24 g of oxygen remain.

EMagnesium reacts with iron(III) chloride to form magnesium chloride (which can be used in fireproofing wood and in disinfectants) and iron.

3Mg(s) + 2FeCl3(s) > 3MgCl2(s) + 2Fe(s)

A mixture of 41.0 g of magnesium ( M = 24.31 g/mol) and 175 g of iron(III) chloride ( M = 162.2 g/mol) is allowed to react. What mass of magnesium chloride = 95.21 g/mol) is formed?

A) 68.5 g MgCl2

B) 77.0 g MgCl2

C) 71.4 g MgCl2

D) 107 g MgCl2

E) 154 g MgCl2

DMagnesium (used in the manufacture of light alloys) reacts with iron(III) chloride to form magnesium chloride and iron.

3Mg(s) + 2FeCl3(s) > 3MgCl2(s) + 2Fe(s)

A mixture of 41.0 g of magnesium ( M = 24.31 g/mol) and 175 g of iron(III) chloride (
M = 162.2 g/mol) is allowed to react. Identify the limiting reactant and determine the mass of the excess reactant present in the vessel when the reaction is complete.

A) Limiting reactant is Mg; 67 g of FeCl3 remain.

B) Limiting reactant is Mg; 134 g of FeCl3 remain.

C) Limiting reactant is Mg; 104 g of FeCl3 remain.

D) Limiting reactant is FeCl3; 2 g of Mg remain.

E) Limiting reactant is FeCl3; 87 g of Mg remain.

APotassium chloride is used as a substitute for sodium chloride for individuals with high blood pressure. Identify the limiting reactant and determine the mass of the excess reactant remaining when 7.00 g of chlorine gas reacts with 5.00 g of potassium to form potassium chloride.

A) Potassium is the limiting reactant; 2.47 g of chlorine remain.

B) Potassium is the limiting reactant; 7.23 g of chlorine remain.

C) Chlorine is the limiting reactant; 4.64 g of potassium remain.

D) Chlorine is the limiting reactant; 2.70 g of potassium remain.

E) No limiting reagent: the reactants are present in the correct stoichiometric ratio.

BTetraphosphorus hexaoxide ( M = 219.9 g/mol) is formed by the reaction of phosphorus with oxygen gas.

P4(s) + 3O2(g) > P4O6(s)

If a mixture of 75.3 g of phosphorus and 38.7 g of oxygen produce 43.3 g of P4O6, what is the percent yield for the reaction?

A) 57.5%

B) 48.8%

C) 38.0%

D) 32.4%

E) 16.3%

CWhat is the percent yield for the reaction

PCl3(g) + Cl2(g) > PCl5(g)

If 119.3 g of PCl5 ( M = 208.2 g/mol) are formed when 61.3 g of Cl2 ( M = 70.91 g/mol) react with excess PCl3?

A) 195%

B) 85.0%

C) 66.3%

D) 51.4%

E) 43.7%

BMethanol (CH4O) is converted to bromomethane (CH3Br) as follows:

CH4O + HBr > CH3Br + H2O

If 12.23 g of bromomethane are produced when 5.00 g of methanol is reacted with excess HBr, what is the percentage yield?

A) 40.9%

B) 82.6%

C) 100.%

D) 121%

E) 245%

EA 0.150 M sodium chloride solution is referred to as a physiological saline solution because it has the same concentration of salts as normal human blood. Calculate the mass of solute needed to prepare 275.0 mL of a physiological saline solution.

A) 41.3 g

B) 31.9 g

C) 16.1 g

D) 8.77 g

E) 2.41 g

CSodium chlorate is used as an oxidizer in the manufacture of dyes, explosives and matches. Calculate the mass of solute needed to prepare 1.575 L of 0.00250 M NaClO3 ( M = 106.45 g/mol).

A) 419 g

B) 169 g

C) 0.419 g

D) 0.169 g

E) 0.00394 g

aLithium hydroxide is used in alkaline batteries. Calculate the molarity of a solution prepared by dissolving 1.495 moles of LiOH in enough water to give a final volume of 750. mL.

A) 1.99 M

B) 1.50 M

C) 1.12 M

D) 0.502 M

E) 0.00199 M

dHydrochloric acid is widely used as a laboratory reagent, in refining ore for the production of tin and tantalum, and as a catalyst in organic reactions. Calculate the
number of moles of HCl in 62.85 mL of 0.453 M hydrochloric acid.A) 28.5 mol

B) 1.04 mol

C) 0.139 mol

D) 0.0285 mol

E) 0.00721 mol

ASodium hydroxide, also known as caustic soda, is used to neutralize acids and to treat cellulose in making of cellophane. Calculate the number of moles of solute in 1.875 L of 1.356 M NaOH solution.

A) 2.543 mol

B) 1.383 mol

C) 0.7232 mol

D) 0.3932 mol

E) 0.001383 mol

ECalculate the molarity of a 23.55-mL solution which contains 28.24 mg of sodium sulfate (used in dyeing and printing textiles, = 139.04 g/mol).

A) 8.625 M

B) 1.199 M

C) 0.8339 M

D) 0.2031 M

E) 0.008625 M

dWhen 2.61 g of solid Na2CO3 is dissolved in sufficient water to make 250 mL of solution,
the concentration of Na2CO3 is:A) 0.0246 M

B) 10.4 M

C) 0.205 M

D) 0.0985 M

E) 0.141 M

dCalcium chloride is used to melt ice and snow on roads and sidewalks and to remove water from organic liquids. Calculate the molarity of a solution prepared by diluting 165
mL of 0.688 M calcium chloride to 925.0 mL.A) 3.86 M

B) 0.743 M

C) 0.222 M

D) 0.123 M

E) 0.114 M

CWhat will be the final volume of a solution prepared by diluting 25 mL of 8.25 M sodium
hydroxide to a concentration of 2.40 M?A) 330 mL

B) 210 mL

C) 86 mL

D) 60 mL

E) 7.3 mL

BWhat volume, in L, of 10.0 M HCl is needed to make 2.00 L of 2.00 M HCl solution by dilution with water?

A) 0.800 L

B) 0.400 L

C) 0.200 L

D) 0.100 L

E) None of these choices is correct.

dHow many mL of concentrated nitric acid (HNO3, 16.0 M) should be diluted with water in order to make 2.00 L of 2.00 M solution?

A) 32.0 mL

B) 62.5 mL

C) 125 mL

D) 250. mL

E) 500. mL

EHow many milliliters of 1.58 M HCl are needed to react completely with 23.2 g of

NaHCO3 ( M = 84.02 g/mol)?

HCl(aq) + NaHCO3(s) > NaCl(s) + H2O(l) + CO2(g)

A) 638 mL

B) 572 mL

C) 536 mL

D) 276 mL

E) 175 mL

bCopper(II) sulfide, CuS, is used in the development of aniline black dye in textile printing. What is the maximum mass of CuS which can be formed when 38.0 mL of 0.500 M CuCl2 are mixed with 42.0 mL of 0.600 M (NH4)2S? Aqueous ammonium
chloride is the other product.A) 2.41 g

B) 1.82 g

C) 1.21 g

D) 0.909 g

E) 0.044 g

APropane, C3H8, is commonly provided as a bottled gas for use as a fuel. In 0.200 mol of propane,

A) what is the mass of propane?

C) 1.20 x 10^23 C3H8 molecules

B) 7.21 g

D) 9.64 x 10^23 H atoms

0.156For a sample consisting of 2.50 g of methane, CH4, calculate

a. the number of moles of methane present.

4.69 x 10^23For a sample consisting of 2.50 g of methane, CH4, calculate

b. the total number of atoms present.

3.61 x 10^23In 0.20 mole of phosphoric acid, H3PO4,

a. how many H atoms are there?

9.64 x 10^23In 0.20 mole of phosphoric acid, H3PO4,

b. what is the total number of atoms?

4.82 x 10^23In 0.20 mole of phosphoric acid, H3PO4,

c. how many moles of O atoms are there?

C22H35O2A compound consisting of C, H and O only, has a molar mass of 331.5 g/mol. Combustion of 0.1000 g of this compound caused a 0.2921 g increase in the mass of the CO2 absorber and a 0.0951 g increase in the mass of the H2O absorber. What is the
empirical formula of the compound?
PCl3Analysis of a white solid produced in a reaction between chlorine and phosphorus showed that it contained 77.44% chlorine and 22.56% phosphorus. What is its empirical formula?
2C4H10(g) + 13O2(g) > 8CO2(g) + 10H2O(l)Balance the following equation for the combustion of butane, a hydrocarbon used in gas
lighters:C4H10(g) + O2(g) > CO2(g) + H2O(l)
B2O3(s) + 6NaOH(aq) > 2Na3BO3(aq) + 3H2O(l)Balance the equation
B2O3(s) + NaOH(aq) > Na3BO3(aq) + H2O(l)
4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(l)Balance the following equation for partial oxidation of ammonia, an important reaction in the production of nitric acid:

NH3(g) + O2(g) > NO(g) + H2O(l)

2CH4O(g) + 3O2(g) > 2CO2(g) + 4H2O(l)Gaseous methanol (CH4O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.
oxygenConsider the balanced equation for the combustion of propane, C3H8

C3H8(g) + 5O2(g) > 3CO2(g) + 4H2O(l)

If propane reacts with oxygen as above,

a. what is the limiting reagent in a mixture containing 5.00 g of C3H8 and 10.0 g of O2?

2.99Consider the balanced equation for the combustion of propane, C3H8

C3H8(g) + 5O2(g) > 3CO2(g) + 4H2O(l)

If propane reacts with oxygen as above,

b. what mass of CO2 is formed when 1.00 g of C3H8 reacts completely?

3.52Ammonia, NH3 , is produced industrially from nitrogen and hydrogen as follows:

N2(g) + 3H2(g) > 2NH3(g)

What mass, of which starting material, will remain when 30.0 g of N2 and 10.0 g of H2
react until the limiting reagent is completely consumed?

waterConsider the balanced equation:

Al2S3(s) + 6H2O(l) 2Al(OH)3(s) + 3H2S(g)

If 15.0g of aluminum sulfide and 10.0g of water are allowed to react as above, and
assuming a complete reaction,

a. by calculation, find out which is the limiting reagent.

9.50Consider the balanced equation:

Al2S3(s) + 6H2O(l) 2Al(OH)3(s) + 3H2S(g)

If 15.0g of aluminum sulfide and 10.0g of water are allowed to react as above, and
assuming a complete reaction,

b. calculate the maximum mass of H2S which can be formed from these reagents.

1.11Consider the balanced equation:

Al2S3(s) + 6H2O(l) > 2Al(OH)3(s) + 3H2S(g)

If 15.0g of aluminum sulfide and 10.0g of water are allowed to react as above, and
assuming a complete reaction,

c. calculate the mass of excess reagent remaining after the reaction is complete.

0.044479. The insecticide DDT was formerly in widespread use, but now it is severely restricted

owing to its adverse environmental effects. It is prepared as follows:

C2HCl3O + C6H5Cl > C14H9Cl5 + H2O
chloral chlorobenzene DDT

If 10.00 g of chloral were reacted with 10.00 g of chlorobenzene,

a. what is the maximum amount (mol) of DDT which could be formed?

Chlorobenzene79. The insecticide DDT was formerly in widespread use, but now it is severely restricted

owing to its adverse environmental effects. It is prepared as follows:

C2HCl3O + C6H5Cl > C14H9Cl5 + H2O
chloral chlorobenzene DDT

If 10.00 g of chloral were reacted with 10.00 g of chlorobenzene,

b. what is the limiting reagent?

77.2%79. The insecticide DDT was formerly in widespread use, but now it is severely restricted

owing to its adverse environmental effects. It is prepared as follows:

C2HCl3O + C6H5Cl > C14H9Cl5 + H2O
chloral chlorobenzene DDT

If 10.00 g of chloral were reacted with 10.00 g of chlorobenzene,

c. what is the % yield, if 12.15 g of DDT is produced?

1.000You are provided with a 250 mL volumetric flask, deionized water and solid NaOH. How
much NaOH should be weighed out in order to make 250. mL of 0.100 M solution?
0.961A solution of methanol (CH4O) in water has a concentration of 0.200 M. What mass of
methanol, in grams, is present in 0.150 liters of this solution?
0.00461a. A solution of common salt, NaCl, in water has a concentration of 0.0921 M. Calculate
the number of moles of HCl contained in 50.0 mL of this solution.
0.684a. A solution of common salt, NaCl, in water has a concentration of 0.0921 M. Calculate
the number of moles of HCl contained in 50.0 mL of this solution.b. If, instead, an NaCl solution is prepared by dissolving 10.0 g of solid NaCl in enough
water to make 250. mL of solution, what is the molarity?
59.3 mlAluminum metal dissolved in hydrochloric acid as follows:

2Al(s) + 6HCl(aq) > 2AlCl3(aq) + 3H2(g)

a. What is the minimum volume of 6.0 M HCl(aq) needed to completely dissolve 3.20 g of aluminum in this reaction?

15.8Aluminum metal dissolved in hydrochloric acid as follows:

2Al(s) + 6HCl(aq) > 2AlCl3(aq) + 3H2(g)

b. What mass of AlCl3 would be produced by complete reaction of 3.20 g of aluminum?

falseOne mole of O2 has a mass of 16.0 g.

(True/False)

trueOne mole of methane (CH4) contains a total of 3 x 10^24 atoms.

(True/False)

falseThe formula CH3O0.5 is an example of an empirical formula.

(True/False)

trueIn combustion analysis, the carbon and hydrogen contents of a substance are determined from the CO2 and H2O, respectively, which are collected in the absorbers.

(True/False)

falseIn combustion analysis, the oxygen content of a substance is equal to the total oxygen in the CO2 and H2O collected in the absorbers.

(True/False)

falseIn a correctly balanced equation, the number of reactant molecules must equal the number of product molecules.

(True/False)

trueWhen a solution is diluted with water, the ratio of the initial to final volumes of solution is equal to the ratio of final to initial molarities.

(True/False)