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chemistry
physical chemistry

Chemical Principles 7th edition Steven S. Zumdahl, Donald J. DeCoste - Solutions

Observations of the reaction between nitrogen gas and hydrogen gas show us that 1 volume of nitrogen reacts with 3 volumes of hydrogen to make 2 volumes of gaseous product, as shown below:Determine the formula of the product and justify your answer.
The three most stable oxides of carbon are carbon mono-oxide (CO), carbon dioxide (CO2), and carbon suboxide (C3O2). The molecules can be represented asExplain how these molecules illustrate the law of multiple proportions.
Hydrazine, ammonia, and hydrogen azide all contain only nitrogen and hydrogen. The mass of hydrogen that combines with 1.00 g of nitrogen for each compound is 1.44 × 10–1 g, 2.16 × 10-1 g, and 2.40 × 10–2 g, respectively. Show how these data illustrate the law of multiple
Consider 100.0 g samples of two different compounds consisting only of carbon and oxygen. One compound contains 27.2 g of carbon, and the other has 42.9 g of carbon. How can these data support the law of multiple proportions if 42.9 is not a multiple of 27.2? Show that these data support the law of
Early tables of atomic weights (masses) were generated by measuring the mass of a substance that reacts with 1.00 g of oxygen. Given the following data and taking the atomic mass of hydrogen as 1.00, generate a table of relative atomic masses for oxygen, sodium, and magnesium.How do your values
What evidence led to the conclusion that cathode rays had a negative charge? Is there a difference between a cathode ray and a β particle?
From the information in this chapter on the mass of the proton, the mass of the electron, and the sizes of the nucleus and the atom, calculate the densities of a hydrogen nucleus and a hydrogen atom.
A chemistry instructor makes the following claim: “Consider that if the nucleus were the size of a grape, the electrons would be about 1 mile away on average.” Is this claim reasonably accurate? Provide mathematical support.
A chemist in a galaxy far, far away performed the Millikan oil drop experiment and got the following results for the charge on various drops. What is the charge of the electron in zirkombs? 2.56 × 10-12 zirkombs7.68 × 10-12 zirkombs3.84 × 10-12 zirkombs6.40 × 10-13 zirkombs
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare with the mass of the electron? Which particles make the greatest contribution to the mass of an atom? Which particles make the greatest contribution to the chemical properties of an
Consider Ernest Rutherford€™s Î±-particle bombardment experiment illustrated in Fig.. How did the results of this experiment lead Rutherford away from the plum pudding model of the atom to propose the nuclear model of the atom?
Distinguish between the following terms.a. Molecule versus ionb. Covalent bonding versus ionic bondingc. Molecule versus compoundd. Anion versus cation
What is the distinction between atomic number and mass number? Between mass number and atomic mass?
a. Classify the following elements as metals or nonmetals.b. The distinction between metals and nonmetals is really not a clear one. Some elements, called metalloids, are intermediate in their properties. Which of these elements would you reclassify as metalloids? What other elements in the
a. List the noble gas elements. Which of the noble gases has only radioactive isotopes? (This situation is indicated on most periodic tables by parentheses around the mass of the element. See inside front cover.) b. Which lanthanide element and which transition element have only radioactive
Consider the elements of the carbon family: C, Si, Ge, Sn, and Pb. What is the trend in metallic character as one goes down a group in the periodic table? What is the trend in metallic character going from left to right across a period in the periodic table?
Identify the elements that correspond to the following atomic numbers. Label each as either a noble gas, a halogen, an alkali metal, an alkaline earth metal, a transition metal, a lanthanide metal, or an actinide metal. a. 17 b. 4 c. 63 d. 72 e. 2 f. 92 g. 55
The number of protons in an atom determines the identity of the atom. What does the number and arrangement of the electrons in an atom determine? What does the number of neutrons in an atom determine?
For lighter, stable isotopes, the ratio of the mass number to the atomic number is close to a certain value. What is the value? What happens to the value of the mass number to atomic number ratio as stable isotopes become heavier?
Write the atomic symbol (A ZX) for each of the isotopes described below.a. Number of protons = 27, number of neutrons = 31b. The isotope of boron with mass number 10c. Z = 12, A = 23d. Atomic number 53, number of neutrons = 79e. Z = 9, number of neutrons = 10f. Number of protons = 29, mass number
How many protons, neutrons, and electrons are in each of the following atoms or ions?
Complete the following table.
What is the symbol for an ion with 63 protons, 60 electrons, and 88 neutrons? If an ion contains 50 protons, 68 neutrons, and 48 electrons, what is its symbol?
What is the symbol of an ion with 16 protons, 18 neutrons, and 18 electrons? What is the symbol for an ion that has 16 protons, 16 neutrons, and 18 electrons?
Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in each case?a. Rab. Inc. Pd. Tee. Brf. Rb
For each of the following atomic numbers, use the periodic table to write the formula (including the charge) for the simple ion that the element is most likely to form in ionic compounds. a. 13 b. 34 c. 56 d. 7 e. 87 f. 35
The compounds AlCl3, CrCl3, and ICl3 have similar formulas, yet each follows a different set of rules to name it. Name these compounds, and then compare and contrast the nomenclature rules used in each case.
Each of the following compounds has three possible names listed for it. For each compound, what is the correct name and why aren’t the other names used? a. N2O: nitrogen oxide, nitrogen (I) oxide, dinitrogen monoxide b. Cu2O: copper oxide, copper (I) oxide, dicopper monoxide c. Li2O: lithium
Name each of the following compounds.
Name the following compounds. a. NaClO4 b. Mg3(PO4)2 c. Al2(SO4)3 d. SF2 e. SF6 f. Na2HPO4 g. NaH2PO4 h. Li3N i. NaOH j. Mg(OH)2 k. Al(OH)3 l. Ag2CrO4
Name each of the following compounds. a. CuI b. CuI2 c. CoI2 d. Na2CO3 e. NaHCO3 f. S4N4 g. SeBr4 h. NaOCl i. BaCrO4 j. NH4NO3
Name the following compounds. Assume the potential acids are dissolved in water. a. HC2H3O2 b. NH4NO2 c. Co2S3 d. ICl e. Pb3(PO4) f. KClO3 g. H2SO4 h. Sr3N2 i. Al2(SO3)3 j. SnO2 k. Na2CrO4 l. HClO
Write formulas for the following compounds. a. Sulfur dioxide b. Sulfur trioxide c. Sodium sulfite sulfate d. Potassium hydrogen e. Lithium nitride f. Chromium (III) g. Chromium (II) acetate h. Tin (IV) fluoride i. Ammonium hydrogen j. Ammonium hydrogen sulfite phosphate k. Potassium perchlorate l.
Write formulas for the following compounds. a. Sodium oxide b. Sodium peroxide c. Potassium cyanide d. Copper(II) nitrate e. Silicon tetrachloride f. Lead(II) oxide g. Lead(IV) oxide h. Copper(I) chloride i. Gallium arsenide j. Cadmium selenide k. Zinc sulfide l. Mercury(I) chloride m. Nitrous
The common names and formulas for several substances are given below. What are the systematic names for these substances? a. Sugar of lead Pb(C2H3O2)2 b. Blue vitriol CuSO4 c. Quicklime CaO d. Epsom salts MgSO4 e. Milk of magnesia Mg(OH)2 f. Gypsum CaSO4 g. Laughing gas N2O
Each of the following compounds is incorrectly named. What is wrong with each name, and what is the correct name for each compound? a. FeCl3, iron chloride b. NO2, nitrogen(IV) oxide c. CaO, calcium(II) monoxide d. Al2S3, dialuminum trisulfide e. Mg(C2H3O2)2, manganese diacetate f. FePO4, iron(II)
Name the following acids.
What discoveries were made by J. J. Thomson, Henri Becquerel, and Lord Rutherford? How did Dalton’s model of the atom have to be modified to account for these discoveries?
Consider the chemical reaction depicted to the right. Label as much as you can using the terms atom, molecule, element, compound, ionic, gas, and solid.
Section 2.3 describes the postulates of Dalton’s atomic theory. With some modifications, these postulates hold up very well regarding how we view elements, compounds, and chemical reactions today. Answer the following questions concerning Dalton’s atomic theory and the modifications made
Tell which of the following are oxidation–reduction reactions. For those that are, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced.a. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)b. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) c. Cr2O72-(aq) +
Many oxidation– reduction reactions can be balanced by inspection. Try to balance the following reactions by in-spection. In each reaction, identify the substance reduced and the substance oxidized. a. Al(s) + HCl(aq) → AlCl3(aq) + H2(g) b. CH4(g) + S(s) → CS2(l) + H2S(g) c. C3H8(g) + O2(g)
Balance each of the following oxidation– reduction reactions by using the oxidation states method. a. C2H6(g) + O2(g) → CO2(g) + H2O(g) b. Mg(s) + HCl(aq) → Mg2+(aq) + Cl2(aq) + H2(g) c. Cu(s) + Ag+(aq) → Cu2+(aq) + Ag(s) d. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)
Balance the following equations by the half- reaction method.a. Fe(s) + HCl(aq) †’ HFeCl4(aq) + H2(g)
When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 5.0 M HCl is required to react completely with 3.00 g of magnesium?
Consider a 1.50- g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. This mass of the white precipitate formed is 0.641 g.a. Calculate the mass percent of magnesium chloride
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?
In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver
A mixture contains only NaCl and Fe(NO3)3. A 0.456- g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g Calculate the following.a. The mass of iron in the sampleb. The
A mixture contains only sodium chloride and potassium chloride. A 0.1586-g sample of the mixture was dissolved in water. It took 22.90 mL of 0.1000 M AgNO3 to completely precipitate all the chloride present. What is the composition (by mass percent) of the mixture?
Tris(pentafluorophenyl) borane, commonly known by its acronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass.a. What is the empirical
In a 1-L beaker, 203 mL of 0.307 M ammonium chromate was mixed with 137 mL of 0.269 M chromium(III) nitrite to produce ammonium nitrite and chromium(III) chromate. Write the balanced chemical equation for the reaction occurring here. If the percent yield of the reaction was 88.0%, how much
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250- g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. How many acidic hydrogens per molecule does citric acid have?
Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetylsalicylic acid. Acetyl-salicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?
When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2 formed can be determined by reaction with hydrogen peroxide:H2O2(aq) + SO2(g) → H2SO4(aq)The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.325- g sample of coal is
Zinc and magnesium metal each react with hydrochloric acid according to the following equations:Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)A 10.00- g mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture
A 10.00-g sample consisting of a mixture of sodium chloride and potassium sulfate is dissolved in water. This aqueous mixture then reacts with excess aqueous lead (II) nitrate to form 21.75 g of solid. Determine the mass percent of sodium chloride in the original mixture.
Consider the reaction of 19.0 g of zinc with excess silver nitrite to produce silver metal and zinc nitrite. The reaction is stopped before all the zinc metal has reacted and 29.0 g of solid metal is present. Calculate the mass of each metal in the 29.0- g mixture.
Consider an experiment in which two burets, Y and Z, are simultaneously draining into a beaker that initially contained 275.0 mL of 0.300 M HCl. Buret Y contains 0.150 M NaOH and buret Z contains 0.250 M KOH. The stoichiometric point in the titration is reached 60.65 minutes after Y and Z were
A sample is a mixture of KCl and KBr. When 0.1024 g of the sample is dissolved in water and reacted with excess silver nitrate, 0.1889 g of solid is obtained. What is the composition by mass percent of the mixture?
Polychlorinated biphenyls (PCBs) have been used extensively as dielectric materials in electrical transformers. Because PCBs have been shown to be potentially harmful, analysis for their presence in the environment has become very important. PCBs are manufactured according to the following generic
Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations.copper(II)sulfate(aq) + iron(s) → copper(s) + iron(II) sulfate(aq)copper(II) sulfate(aq) + iron(s) → copper(s) + iron(III) sulfate(aq)You place 87.7 mL of a 0.500 M
A stream flows at a rate of 5.00 × 104 liters per second (L/ s) upstream of a manufacturing plant. The plant dis-charges 3.50 × 103 L/ s of water that contains 65.0 ppm HCl into the stream. a. Calculate the stream’s total flow rate downstream from this plant. b. Calculate the
Chromium has been investigated as a coating for steel cans. The thickness of the chromium film is determined by dissolving a sample of a can in acid and oxidizing the resulting Cr3+ to Cr2O7 2- with the peroxydisulfate ion:S2O8 2-(aq) + Cr3+(aq) + H2O(l) → Cr2O7 2-(aq) + SO4 2-(aq) +
One high- temperature superconductor has the general formula YBa2Cu3Ox. The copper is a mixture of Cu(II) and Cu(III) oxidation states. This mixture of oxidation states appears vital for high temperature superconductivity to occur. A simple method for determining the average copper oxidation state
A sample is a mixture of AgNO3, CuCl2, and FeCl3. When a 1.0000- g sample of the mixture is dissolved in water and reacted with excess silver nitrate, 1.7809 g of precipitate forms. When a separate 1.0000- g sample of the mixture is treated with a reducing agent, all the metal ions in the mixture
Three students were asked to find the identity of the metal in a particular sulfate salt. They dissolved a 0.1472-g sample of the salt in water and treated it with excess barium chloride, resulting in the precipitation of barium sulfate. After the precipitate had been filtered and dried, it weighed
Characterize strong electrolytes versus weak electrolytes versus nonelectrolytes. Give examples of each. How do you experimentally determine whether a soluble substance is a strong electrolyte, weak electrolyte, or nonelectrolyte.
Which of the following statements is (are) true? Correct the false statements.
Differentiate between what happens when the following are dissolved in water. a. Polar solute versus nonpolar solute b. KF versus C6H12O6 c. RbCl versus AgCl d. HNO3 versus CO
Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.
List the formulas of three soluble bromide salts and three insoluble bromide salts. Do the same exercise for sulfate salts, hydroxide salts, and phosphate salts (list three soluble salts and three insoluble salts). List the formulas for six insoluble Pb2+ salts and one soluble Pb2+ salt.
For the reactions in Exercise 31, write the balanced molecular equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”Exercise 31When the following solutions are mixed together, what precipitate (if any) will form?a. Hg2(NO3)2(aq) + CuSO4(aq)b.
Write the balanced molecular and net ionic equations for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?
Give an example of how each of the following insoluble ionic compounds could be produced using a precipitation reaction. Write the balanced molecular equation for each reaction. a. Fe(OH)3(s) b. Hg2Cl2(s) c. PbSO4(s) d. BaCrO4(s)
What volume of 0.100 M Na3PO4 is required to precipitate all of the lead(II) ions from 150.0 mL of 0.250 M Pb(NO3)2?
A 1.00-g sample of an alkaline earth metal chloride is treated with excess silver nitrate. All of the chloride is recovered as 1.38 g of silver chloride. Identify the metal.
A mixture contains only NaCl and Al2(SO4)3. A 1.45- g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.107 g. What is the mass percent of Al2(SO4)3 in
The thallium (present as Tl2SO4) in a 9.486-g pesticide sample was precipitated as thallium(I) iodide. Calculate the mass percent of Tl2SO4 in the sample if 0.1824 g of TlI was recovered.
A 1.42-g sample of a pure compound with formula M2SO4 was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic mass
Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to
What volume of each of the following acids will react completely with 50.00 mL of 0.100 M NaOH?a. 0.100 M HClb. 0.100 M H2SO3 (two acidic hydrogens)c. 0.200 M H3PO4 (three acidic hydrogens)d. 0.150 M HNO3e. 0.200 M HC2H3O2 (one acidic hydrogen)f. 0.300 M H2SO4 (two acidic hydrogens)
What volume of 0.0521 M Ba(OH)2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4? Phosphoric acid contains three acidic hydrogens.
A 2.20-g sample of an unknown acid (empirical formula 5C3H4O3) is dissolved in 1.0 L of water. A titration required 25.0 mL of 0.500 M NaOH to react completely with all the acid present. Assuming that the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown
Differentiate between the following terms. a. Species reduced versus the reducing agent b. Species oxidized versus the oxidizing agent c. Oxidation state versus actual charge
How do you balance redox reactions by the oxidation states method?
Assign oxidation states to all atoms in each compound. a. KMnO4 b. NiO2 c. K4Fe(CN)6 (Fe only) d. (NH4)2HPO4 e. P4O6 f. Fe3O4 g. XeOF4 h. SF4 i. CO j. C6H12O6
Assign oxidation states to all of the following atoms.a. UO22+b. As2O3c. NaBiO3d. As4e. HAsO2f. Mg2P2O7g. Na2S2O3h. Hg2Cl2i. Ca(NO3)2
Assign oxidation states to all of the following atoms. a. SrCr2O7 b. CuCl2 c. O2 d. H2O2 e. MgCO3 f. Ag g. PbSO3 h. PbO2 i. Na2C2O4 j. CO2 k. (NH4)2Ce(SO4)3 l. Cr2O3
A sealed- tube manometer as shown below can be used to measure pressures below atmospheric pressure. The tube above the mercury is evacuated. When there is a vacuum in the flask, the mercury levels in both arms of the U-tube are equal. If a gaseous sample is introduced into the flask, the mercury
A compressed-gas cylinder contains 1.00 × 103 g of argon gas. The pressure inside the cylinder is 2050. psi (pounds per square inch) at a temperature of 18oC. How much gas remains in the cylinder if the pressure is decreased to 650. psi at a temperature of 26oC?
Equal moles of sulfur dioxide gas and oxygen gas are mixed in a flexible reaction vessel and then sparked to initiate the formation of gaseous sulfur trioxide. Assuming that the reaction goes to completion, what is the ratio of the final volume of the gas mixture to the initial volume of the gas
Silane (SiH4) is the silicon analogue of methane (CH4). It is prepared industrially according to the following equations:Si(s) + 3HCl(g) → HSiCl3(l) + H2(g) 4HSiCl3(l) → SiH4(g) + 3SiCl4(l)a. If 156 mL of HSiCl3 (d = 1.34 g/ mL) is isolated when 15.0 L of HCl at 10.0 atm and 35oC is used, what
A compound containing only C, H, and N yields the following data.i. Complete combustion of 35.0 mg of the compound produced 33.5 mg of CO2 and 41.1 mg of H2O.ii. A 65.2-mg sample of the compound was analyzed for nitrogen by the Dumas method, giving 35.6 mL of dry N2 at 740. torr and 25oC.iii. The
A 15.0-L tank is filled with H2 to a pressure of 2.00 × 102 atm. How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm from the tank? Assume that there is no temperature change and that the tank cannot be emptied below 1.00 atm pressure.
Consider the following diagram.A porous container (A), filled with air at STP, is contained in a large enclosed container (B), which is flushed with H2(g). What will happen to the pressure inside container A? Explain your answer.
A 100-L flask contains a mixture of methane (CH4) and argon at 25oC. The mass of argon present is 228 g and the mole fraction of methane in the mixture is 0.650. Calculate the total kinetic energy of the gaseous mixture.
Represent the following plots.a. PV/ n (y axis) versus P (x axis) for a real gas that obeys the equation PV/ n = a + βPb. Change in momentum per impact versus mass of an individual gas particle for a series of ideal gases all at the same temperaturec. P versus T (oC) for an ideal gas where n and V
A spherical glass container of unknown volume contains helium gas at 25oC and 1.960 atm. When a portion of the helium is withdrawn and adjusted to 1.00 atm at 25oC, it is found to have a volume of 1.75 cm3. The gas remaining in the first container shows a pressure of 1.710 atm. Calculate the volume
A compound Z is known to have a composition of 34.38% Ni, 28.13% C, and 37.48% O. In an experiment 1.00 L of gaseous Z is mixed with 1.00 L of argon, where each gas is at P = 2.00 atm and T = 25oC. When this mixture of gases is put in an effusion chamber, the ratio of Z molecules to Ar molecules in

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