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General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions

Without doing detailed calculations, explain which of these compounds produces the greatest mass of CO2 when 1.00 mol of the compound is burned in an excess of oxygen:CH4, C2H5OH, C10H8, C6H5OH.
Without doing detailed calculations, explain which of these compounds produces the greatest mass of H2O when 1.00 g of the compound is burned in an excess of oxygen: CH4, C2H5OH, C10H8, C6H5OH.
Indicate the oxidation state of S in (a) SO32-;(b) S2O32-;(c) S2O82-;(d) HSO4-;(e) S4O62-.
Indicate the oxidation state of the underlined element in (a) CH4;(b) SF4;(c) Na2O2;(d) C2H3O2-;(e) FeO42-.
Liquid ethyl mercaptan, C2H6S, has a density of 0.84 g/mL. Assuming that the combustion of this compound produces only CO2, H2O, and SO2, what masses of each of these three products would be produced in the combustion of 3.15 mL of ethyl mercaptan?
Chromium forms three principal oxides. Write appropriate formulas for these compounds in which the oxidation states of Cr are +3, +4, and +6, respectively.
Nitrogen forms five oxides in which its oxidation states are +1, +2, +3, +4, and +5, respectively. Write appropriate formulas for these compounds.
In many of its compounds, oxygen has an oxidation state of -2. However, there are exceptions. What is the oxidation state of oxygen in each of the following compounds? (a) OF2; (b) O2F2; (c) CsO2; (d) BaO2.
Hydrogen and oxygen usually have oxidation states of +1 and -2, respectively, in their compounds. The following cases serve to remind us that there are exceptions. What are the oxidation states of the atoms in each of the following compounds? (a) MgH2;(b) CsO3; (c) HOF; (d) NaAlH4.
Name these compounds: (a) SrO; (b) ZnS; (c) K2CrO4;(d) Cs2SO4;(e) Cr2O3;(f) Fe2(SO4)3;(g) Mg(HCO3)2;(h) (NH4)2HPO4; (i) Ca(HSO3)2;(j) Cu(OH)2; (k) HNO3;(l) KClO4;(m) HBrO3; (n) H3PO3.
Assign suitable names to the compounds (a) ICl(b) ClF3 (c) SiF4 (d) PF5 (e) NO2 (f) S4N4.
Anhydrous CuSO4 can be used to dry liquids in which it is insoluble. The CuSO4 is converted to CuSO4·5 H2O, which can be filtered off from the liquid. What is the minimum mass of anhydrous CuSO4 needed to remove 12.6 g H2O from a tankful of gasoline?
Anhydrous sodium sulfate, Na2SO4 absorbs water vapor and is converted to the decahydrate, Na2SO4 · 10 H2O. How much would the mass of 36.15 g of anhydrous Na2SO4 increase if converted completely to the decahydrate?
A certain hydrate is found to have the composition 20.3% Cu, 8.95% Si, 36.3% F, and 34.5% H2O by mass. What is the empirical formula of this hydrate?
Which of the following names is most appropriate for the molecule with the structure shown below? (a) Butyl alcohol; (b) Butan-2 ol; (c) Butan-1-ol; (d) Isopentyl alcohol. НННН ТТТТ H-C-с-с-с-н | | Н НО Н Н
An 8.129 g sample of MgSO4 · x H2O is heated until all the water of hydration is driven off. The resulting anhydrous compound, MgSO4 weighs 3.967 g. What is the formula of the hydrate?
Which of the following structures are isomers? (a) CH3-CH-CH₂-OH CH₂ CH3 (b) CH3-CH-CH₂-CH₂-OH T CH3 CH₂ (c) CH3 CH₂-CH-CH₂-OH (d) CH,—CH–CH,—0–CH, L CH3 (e) CH3-CH-CH₂-CH-CH₂ I OH T CH3
Which of the following names is most appropriate for the molecule CH3(CH2)2COOH? (a) Dimethyleneacetic acid; (b) Propanoic acid; (c) Butanoic acid;(d) Oxobutylalcohol.
Which of the following structures are isomers? (a) CH3-CH-CH₂-Cl CH₂-CH3 (b) CH3 CH-CH₂-CH3 T CH₂CI (c) CH3-CH-CHCICH3 T CH3 (d) CH3-CH-CH₂-CH-CH3 T CI CH3
Give the name, condensed structural formula, and molecular mass of the molecule whose ball-and-stick model is shown. Refer to the color scheme in Figure 3-3.Figure 3-3 (a) (c) (b) (d)
Write the condensed structural formulas for the organic compounds:(a) Heptane (b) Propanoic acid(c) 2 methylpentan-1-ol (d) Fluoroethane.
Give the name, condensed structural formula, and molecular mass of the molecule whose ball-and-stick model is shown. Refer to the color scheme in Figure 3-3. Figure 3-3 (a) (c) (b) (d)
Write the condensed structural formulas for the organic compounds:(a) Octane (b) Heptanoic acid(c) Hexan-3-ol (d) 2-chlorobutane.
The mineral spodumene has the empirical formula LiAlSi2O6. Given that the percentage of lithium-6 atoms in naturally occuring lithium is 7.40%, how many lithium-6 atoms are present in a 518 g sample of spodumene?
A particular type of brass contains Cu, Sn, Pb, and Zn. A 1.1713 g sample is treated in such a way as to convert the Sn to 0.245 g SnO2, the Pb to 0.115 g PbSO4, and the Zn to 0.246 g Zn2P2O7. What is the mass percent of each element in the sample?
A brand of lunchmeat contains 0.12% by mass of sodium benzoate, C6H5COONa. How many mg of Na does a person ingest by eating 3.50 oz of this meat?
The important natural sources of boron compounds are the minerals kernite, Na2B4O7 · 4 H2O and borax, Na2B4O7 · 10 H2O. How much additional mass of mineral must be processed per kilogram of boron obtained if the mineral is borax rather than kernite?
Is it possible to have a sample of S8 that weighs 1.00 x 10-23 g? What is the smallest possible mass that a sample of S8 can have? Express your answer to the second question in appropriate SI units so that your answer has a numerical value greater than 1. (See Table 1.2 for a list of SI
To deposit exactly one mole of Ag from an aqueous solution containing Ag+ requires a quantity of electricity known as one faraday (F). The electrodeposition requires that each Ag+ ion gain one electron to become an Ag atom. Use appropriate physical constants listed on the inside back cover to
By analysis, a compound was found to contain 26.58 % K and 35.45 % Cr by mass; the remainder was oxygen. What is the oxidation state of chromium in this compound? What is the name of the compound?
In 2013, the IUPAC recommended that the atomic masses of 12 elements be expressed as an atomic mass interval rather as a single invariant value. (See Section 2-5 and Table 2.2.) For example, the IUPAC recommends that the atomic mass of Cl be given as [35.446, 35.457]. Consequently, the results of
What is the molecular formula of a hydrocarbon containing n carbon atoms and only one double bond? Can such a hydrocarbon yield a greater mass of H2O than CO2 when burned in an excess of oxygen?
A hydrocarbon mixture consists of 60.0% by mass of C3H8 and 40.0% of CxHy. When 10.0 g of this mixture is burned, 29.0 g CO2 and 18.8 g H2O are the only products. What is the formula of the unknown hydrocarbon?
A 0.732 g mixture of methane,CH4 , and ethane, C2H6, is burned, yielding 2.064 g CO2. What is the percent composition of this mixture(a) By mass;(b) On a mole basis?
The density of a mixture of H2SO4 and water is 1.78 g/mL. The percent composition of the mixture is to be determined by converting H2SO4 to (NH4)2SO4. If 32.0 mL of the mixture gives 65.2 g (NH4)2SO4, then what is the percent composition of the mixture?
In the year 2000, the Guinness Book of World Records called ethyl mercaptan,C2H6S , the smelliest substance known. The average person can detect its presence in air at levels as low as 9 x 10-4 μmol/m3. Express the limit of detectability of ethyl mercaptan in parts per billion (ppb). (Note: 1 ppb
Dry air is essentially a mixture of the following entities: ,N2, O2 , Ar, and CO2. The composition of dry air, in mole percent, is 78.08% N2, 20.95% O2, 0.93% Ar, and 0.04% CO2. (a) What is the mass, in grams, of a sample of air that contains exactly one mole of the entities? (b) Dry air also
A public water supply was found to contain 0.8 part per billion (ppb) by mass of chloroform, CHCl3. (a) How many CHCl3 molecules would be present in a 350 mL glass of this water? (b) If the CHCl3 in part (a) could be isolated, would this quantity be detectable on an ordinary analytical balance
A sample of the compound MSO4 weighing 0.1131 g reacts with barium chloride and yields 0.2193 g BaSO4. What must be the atomic mass of the metal M?
The metal M forms the sulfate M2(SO4)3. A 0.738 g sample of this sulfate is converted to 1.511 g BaSO4. What is the atomic mass of M?
A 0.622 g sample of a metal oxide with the formula M2O3 is converted to 0.685 g of the sulfide, MS. What is the atomic mass of the metal M?
MgCl2 often occurs in table salt (NaCl) and is responsible for caking of the salt. A 0.5200 g sample of table salt is found to contain 61.10% Cl, by mass. What is the % MgCl2 in the sample? Why is the precision of this calculation so poor?
When 2.750 g of the oxide of lead Pb3O4 is strongly heated, it decomposes and produces 0.0640 g of oxygen gas and 2.686 g of a second oxide of lead. What is the empirical formula of this second oxide?
A 1.013 g sample of ZnSO4 · x H2O is dissolved in water and the sulfate ion precipitated as BaSO4. The mass of pure, dry BaSO4 obtained is 0.8223 g. What is the formula of the zinc sulfate hydrate?
The iodide ion in a 1.552 g sample of the ionic compound MI is removed through precipitation. The precipitate is found to contain 1.186 g I. What is the element M?
An oxoacid with the formula HxEyOz has a formula mass of 178 u, has 13 atoms in its formula unit, contains 34.80% by mass, and 15.38% by number of atoms, of the element E. What is the element E, and what is the formula of this oxoacid?
The insecticide dieldrin contains carbon, hydrogen, oxygen, and chlorine. When burned in an excess of oxygen, a 1.510 g sample yields 2.094 g CO2 and 0.286 g H2O. The compound has a molecular mass of 381 u and has half as many chlorine atoms as carbon atoms. What is the molecular formula of
A thoroughly dried 1.271 g sample of Na2SO4 is exposed to the atmosphere and found to gain 0.387 g in mass. What is the percent, by mass, of Na2SO4 · 10 H2O in the resulting mixture of anhydrous Na2SO4 and the decahydrate?
The atomic mass of Bi is to be determined by converting the compound Bi(C6H5)3 to Bi2O3. If 5.610 g of Bi(C6H5)3 yields 2.969 g Bi2O3, what is the atomic mass of Bi?
A piece of gold (Au) foil measuring 0.25 mm X 15 mm X 15 mm is treated with fluorine gas. The treatment converts all the gold in the foil to 1.400 g of a gold fluoride. What is the formula and name of the fluoride? The density of gold is 19.3 g/cm3.
In an experiment, 244 mL of chlorine gas (Cl2, d = 2.898 g/L) combines with iodine to give 1.553 g of a binary compound. In a separate experiment, the molar mass of the compound is found to be about 467 g/mol. What is the molecular formula of this compound?
Which answer is correct? One mole of liquid bromine, Br2,(a) Has a mass of 79.9 g; (b) Contains 6.022 x 1023 Br atoms; (c) Contains the same number of atoms as in 12.01 g H2O; (d) Has twice the mass of 0.500 mole of gaseous Cl2.
Three of the following formulas might be either an empirical or a molecular formula. The formula that must be a molecular formula is (a) N2O;(b) N2H4;(c) NaCl; (d) NH3.
The compound C7H7NO2 contains (a) 17 atoms per mole; (b) Equal percents by mass of C and H; (c) About twice the percent by mass of O as of N; (d) About twice the percent by mass of N as of H.
Iron is present in red blood cells and acts to carry oxygen to the organs. Without oxygen, these organs will die. There are about 2.6 x 1013 red blood cells in the blood of an adult human, and the blood contains a total of 2.9 g of iron. How many atoms are there in each blood cell?
XF3 consists of 65% F by mass. The atomic mass of the element X must be (a) 8 u; (b) 11u; (c) 31 u; (d) 35 u.
The oxidation state of I in the ion H4IO6- is (a) -1;(b) +1;(c) +7;(d) +8.
The oxidation state of Mn in MgMnO4 is (a) +2;(b) +7; (c) +6; (d) +4; (e) +3.
The name of which compound ends with –ate?(a) HIO4; (b) Na2SO3; (c) KClO2;(d) HFO;(e) NO2.
The name of Sr(HCO3)2 is (a) Strontium oxalate;(b) Strontium carbonate; (c) Sodium bicarbonate;(d) Strontium bicarbonate; (e) None of these.
Which compound has a molar mass of 51.79 g mol-1?(a) NaCl; (b) KF; (c) MgS; (d) Li3P; (e) None of these.
The greatest number of N atoms is found in (a) 50.0 g N2O;(b) 17.0 g NH3; (c) 150 mL of liquid pyridine, C5H5N (d = 0.983 g/mL);(d) 1.0 mol N2.
When combustion is carried out in an excess of oxygen, the quantity producing the greatest mass of both CO2 and H2O is (a) 0.50 mol C10H8;(b) 1.25 mol CH4;(c) 0.500 mol C2H5OH; (d) 1.00 mol C6H5OH.
Calculate the total number of (a) Atoms in one molecule of trinitrotoluene (TNT), CH3C6H2(NO2)3;(b) Atoms in 0.00102 mol CH3(CH2)4CH2OH;(c) F atoms in 12.15 mol C2HBrClF3.
(A) Sorbitol, used as a sweetener in some sugar-free foods, has a molecular mass of 182 u and a mass percent composition of 39.56% C, 7.74% H, and 52.70% O. What are the empirical and molecular formulas of sorbitol?(B) The chlorine-containing narcotic drug pentaerythritol chloral has 21.51% C,
Vitamin C is essential for the prevention of scurvy. Combustion of a 0.2000 g sample of this carbon–hydrogen–oxygen compound yields 0.2998 g CO2 and 0.0819 g H2O. What are the percent composition and the empirical formula of vitamin C?
A nitrogen–hydrogen compound with molar mass 32 g/mol has N in a higher oxidation state than in NH3. What is a plausible formula for that compound?
Determine the mass, in grams, of(a) 7.34 mol NO2;(b) 4.220 x 1025 O2 molecules;(c) 15.5 mol CuSO4.5 H2O;(d) 2.25 x 1024 molecules of C2H4(OH)2.
Explain each term as it applies to the element nitrogen:(a) Atomic mass; (b) Molecular mass; (c) Molar mass.
Explain the important distinctions between each pair of terms: (a) Molecular mass and molar mass;(b) Empirical and molecular formulas; (c) Systematic and trivial, or common, name; (d) Hydroxyl and carboxyl functional group.
Placing a 0.725 g copper strip in the presence of iodine vapor produced a yellowish-white coating on the metal strip. The mass of the copper strip and coating was 0.733 g. The coating was removed by rinsing the coated metal strip in a potassium thiocyanate (KSCN) solution, yielding a clean copper
Briefly describe each of the following ideas or methods:(a) Mole of a compound; (b) Structural formula;(c) Oxidation state; (d) Carbon–hydrogen–oxygen determination by combustion analysis.
Some substances that are only very slightly soluble in water will spread over the surface of water to produce a film that is called a monolayer because it is only one molecule thick. A practical use of this phenomenon is to cover ponds to reduce the loss of water by evaporation. Stearic acid forms
In your own words, define or explain the following terms or symbols: (a) Formula unit; (b) P4; (c) Molecular compound; (d) Binary compound; (e) Hydrate.
A hydrate of copper(II) sulfate, when heated, goes through the succession of changes suggested by the photograph. In this photograph, (a) Is the original fully hydrated copper(II) sulfate; (b) Is the product obtained by heating the original hydrate to 140 °C; (c) Is the product obtained by
All-purpose fertilizers contain the essential elements nitrogen, phosphorus, and potassium. A typical fertilizer carries numbers on its label, such as "5-10-5". These numbers represent the % N, % P2O5 and % K2O, respectively. The N is contained in the form of a nitrogen compound, such as (NH4)2SO4,
How many moles of CO2 are produced in the combustion of 2.72 mol of triethylene glycol,C6H14O4, in an excess of O2?
(A) How many moles of O2 are produced from the decomposition of 1.76 moles of potassium chlorate?2 KClO3(s) → 2 KCl(s) + 3 O2(g)(B) How many moles of Ag are produced in the decomposition of 1.00 kg of silver oxide?2 Ag2O(s) → 4 Ag(s) + O2(g)
Balance the following equations by inspection.(a) SO2Cl2 + HI → H2S + H2O + HCl + I2(b) FeTiO3 + H2SO4 + H2O → FeSO4 · 7 H2O + TiOSO4(c) Fe3O4 + HCl + Cl2 → FeCl3 + H2O + O2(d) C6H5CH2SSCH2C6H5 + O2 → CO2 + SO2 + H2O.
Without doing detailed calculations, and assuming that the volumes of solutions and water are additive, indicate the molarity of the final solution obtained as a result of(a) Adding 200.0 mL of water to 100.0 mL of 0.150 M NaCl(b) Evaporating 50.0 mL water from 250.0 mL of 0.800 M C12H22O11(c)
Write balanced equations based on the information given.(a) Solid magnesium + oxygen gas → solid magnesium oxide(b) Nitrogen monoxide gas + oxygen gas → nitrogen dioxide gas(c) Gaseous ethane(C2H6) + oxygen gas → carbon dioxide gas + liquid water(d) Aqueous silver sulfate + aqueous barium
An alloy used in aircraft structures consists of 93.7% Al and 6.3% Cu by mass. The alloy has a density of 2.85 g/cm3. A 0.691 cm3 piece of the alloy reacts with an excess of HCl(aq). If we assume that all the Al but none of the Cu reacts with HCl(aq), what is the mass of H2 obtained?
Which statements are correct for the reaction 2 H2S + SO2 → 3 S + 2 H2O? Explain your reasoning.(a) 3 mol S is produced per mole of H2S consumed.(b) 3 g S is produced for every gram of SO2 consumed.(c) 1 mol H2O is produced per mole of H2S consumed.(d) Two-thirds of the S produced comes from
Balance the following equations by inspection.(a) PbO + NH3 → Pb + N2 + H2O(b) FeSO4 → Fe2O3 + SO2 + O2(c) S2Cl2 + NH3 → N4S4 + NH4Cl + S8(d) C3H7CHOHCH(C2H5)CH2OH + O2 → CO2 + H2O.
What mass of CO2 is formed in the reaction of 4.16 g triethylene glycol, C6H14O4 with an excess of O2?
Without performing detailed calculations, determine which reaction produces the maximum quantity of O2(g) per gram of reactant. 2 N₂(g) + 4 H₂O(l) + O₂(g) (a) 2 NH4NO3(s) A (b) 2 Ag₂O(s) → 4 Ag(s) + O₂(g) A (c) 2 HgO(s) 2 Hg(l) + O₂(g) A (d) 2 Pb(NO3)2(s) 2 PbO(s) + 4 NO₂(g) +
(A) How many grams of magnesium nitride, Mg3N2, are produced by the reaction of 3.82 g Mg with an excess of N2?(B) How many grams of H2 are required to produce 1.00 kg methanol, CH3OH, by the reaction CO + 2 H2 → CH3OH?
What mass of O2 is consumed in the complete combustion of 6.86 g of triethylene glycol, C6H14O4?
Suppose that the reaction of 1.0 mol NH3(g) and 1.0 mol O2(g) is carried to completion, producing NO(g) and H2O(l) as the only products. Which, if any, of the following statements is correct about this reaction? (a) 1.0 mol NO(g) is produced; (b) 4.0 mol NO(g) is produced; (c) 1.5 mol H2O(l) is
(A) What volume of the aluminum-copper alloy described in Example 4-5 must be dissolved in an excess of HCl(aq) to produce 1.00 g H2?(B) Afresh sample of the aluminum-copper alloy described in Example 4-5 yielded 1.31 g H2. How many grams of copper were present in the sample?Example 4-5An alloy
Suppose that each of these reactions has a 90% yield. CH4(g) + Cl2(g) → CH3Cl(g) + HCl(g)CH3Cl(g) + Cl2(g) → CH2Cl2(l) + HCl(g)Starting with 50.0 g CH4 in the first reaction and an excess of Cl2(g), the number of grams of CH2Cl2 formed in the second reaction is(a) 50.0 x 0.81 x (85/16)(b) 50.0
Write balanced equations based on the information given.(a) Solid magnesium + nitrogen gas → solid magnesium nitride(b) Solid potassium chlorate → solid potassium chloride + oxygen gas(c) Solid sodium hydroxide + solid ammonium chloride → solid sodium chloride + gaseous ammonia + water
A hydrochloric acid solution consists of 28.0% HCl by mass and has a density of 1.14 g/mL. What volume of this solution is required to react completely with 1.87 g AI?
(A) How many milligrams of H2 are produced when one drop (0.05 mL) of the hydrochloric acid solution described in Example 4-6 reacts with an excess of aluminum?(B) A particular vinegar contains 4.0% CH3COOH by mass. It reacts with sodium carbonate to produce sodium acetate, carbon dioxide, and
Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) Butane, C4H10(g);(b) Isopropyl alcohol, CH3CH(OH)CH3(l);(c) Lactic acid,CH3CH(OH)COOH(s).
A solution is prepared by dissolving 25.0 mL ethanol, CH3CH2OH (d = 0.789 g/mL), in enough water to produce 250.0 mL solution. What is the molarity of ethanol in the solution?
(A) A 22.3 g sample of acetone (see the model here) is dissolved in enough water to produce 1.25 L of solution. What is the molarity of acetone in this solution?(B) If 15.0 mL of acetic acid, CH3COOH (d = 1.048 g/mL), is dissolved in enough water to produce 500.0 mL of solution, then what is the
What mass of K2CrO4 is needed to prepare exactly 0.2500 L (250.0 mL) of a 0.250 M K2CrO4 solution in water? (See Figure 4-5.)Figure 4-5 (a) 250 (b) O
Write balanced equations to represent the complete combustion of each of the following in excess oxygen: (a) Propylene, C3H6(g); (b) Thiobenzoic acid, C6H5COSH(l);(c) Glycerol, CH2(OH)CH(OH)CH2OH(l).
(A) An aqueous solution saturated with NaNO3 at 25 °C is 10.8 M NaNO3. What mass of NaNO3 is present in 125 mL of this solution at 25 °C?(B) What mass of Na2SO4 . 10 H2O is needed to prepare 355 mL of 0.445 M Na2SO4?

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