Chapter 3 Terms Answers – Flashcards
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Calcium 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
answer
C
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Calculate 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
answer
B
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Calculate 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
answer
C
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Calculate 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
answer
B
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Aluminum 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
answer
B
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Calculate 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
answer
B
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Magnesium 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
answer
E
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Sodium 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
answer
A
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What 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
answer
B
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Calculate 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
answer
D
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Phosphorus 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
answer
E
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Aluminum 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
answer
D
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Calculate 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
answer
B
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Potassium 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
answer
D
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Sulfur 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
answer
C
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Calculate 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
answer
E
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The 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
answer
C
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Copper(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
answer
B
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Lead(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
answer
C
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Household 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 %
answer
D
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Gadolinium 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
answer
A
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Hydroxylamine 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
answer
B
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Hydroxylamine 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
answer
B
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A 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
answer
E
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A 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
answer
D
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Alkanes 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
answer
B
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Terephthalic 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
answer
c
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Terephthalic 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
answer
e
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Hydroxylamine 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
answer
d
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In 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
answer
C
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Balance 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)
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a
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Balance 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)
answer
b
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Balance 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)
answer
C
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Balance 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)
answer
b
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Balance 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)
answer
d
question
Sulfur 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
answer
c
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Aluminum 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
answer
B
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Ammonia 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
answer
d
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Ammonia, 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
answer
c
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How 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
answer
c
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How 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
answer
a
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Phosphine, 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
answer
d
question
Potassium 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
answer
c
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Aluminum 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
answer
e
question
Lead(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
answer
a
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Aluminum 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
answer
a
question
Aluminum 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.
answer
e
question
Magnesium 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
answer
E
question
Magnesium (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.
answer
D
question
Potassium 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.
answer
A
question
Tetraphosphorus 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%
answer
B
question
What 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%
answer
C
question
Methanol (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%
answer
B
question
A 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
answer
E
question
Sodium 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
answer
C
question
Lithium 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
answer
a
question
Hydrochloric 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
answer
d
question
Sodium 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
answer
A
question
Calculate 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
answer
E
question
When 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
answer
d
question
Calcium 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
answer
d
question
What 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
answer
C
question
What 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.
answer
B
question
How 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
answer
d
question
How 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
answer
E
question
Copper(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
answer
b
question
Propane, 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
answer
A
question
For a sample consisting of 2.50 g of methane, CH4, calculate a. the number of moles of methane present.
answer
0.156
question
For a sample consisting of 2.50 g of methane, CH4, calculate b. the total number of atoms present.
answer
4.69 x 10^23
question
In 0.20 mole of phosphoric acid, H3PO4, a. how many H atoms are there?
answer
3.61 x 10^23
question
In 0.20 mole of phosphoric acid, H3PO4, b. what is the total number of atoms?
answer
9.64 x 10^23
question
In 0.20 mole of phosphoric acid, H3PO4, c. how many moles of O atoms are there?
answer
4.82 x 10^23
question
A 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?
answer
C22H35O2
question
Analysis 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?
answer
PCl3
question
Balance the following equation for the combustion of butane, a hydrocarbon used in gas lighters: C4H10(g) + O2(g) > CO2(g) + H2O(l)
answer
2C4H10(g) + 13O2(g) > 8CO2(g) + 10H2O(l)
question
Balance the equation B2O3(s) + NaOH(aq) > Na3BO3(aq) + H2O(l)
answer
B2O3(s) + 6NaOH(aq) > 2Na3BO3(aq) + 3H2O(l)
question
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)
answer
4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(l)
question
Gaseous methanol (CH4O) reacts with oxygen gas to produce carbon dioxide gas and liquid water. Write a balanced equation for this process.
answer
2CH4O(g) + 3O2(g) > 2CO2(g) + 4H2O(l)
question
Consider 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?
answer
oxygen
question
Consider 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?
answer
2.99
question
Ammonia, 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?
answer
3.52
question
Consider 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.
answer
water
question
Consider 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.
answer
9.50
question
Consider 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.
answer
1.11
question
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, a. what is the maximum amount (mol) of DDT which could be formed?
answer
0.0444
question
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, b. what is the limiting reagent?
answer
Chlorobenzene
question
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?
answer
77.2%
question
You 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?
answer
1.000
question
A 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?
answer
0.961
question
a. 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.
answer
0.00461
question
a. 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?
answer
0.684
question
Aluminum 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?
answer
59.3 ml
question
Aluminum 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?
answer
15.8
question
One mole of O2 has a mass of 16.0 g. (True/False)
answer
false
question
One mole of methane (CH4) contains a total of 3 x 10^24 atoms. (True/False)
answer
true
question
The formula CH3O0.5 is an example of an empirical formula. (True/False)
answer
false
question
In 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)
answer
true
question
In 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)
answer
false
question
In a correctly balanced equation, the number of reactant molecules must equal the number of product molecules. (True/False)
answer
false
question
When 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)
answer
true
