Ch.3 - Molecules, Compounds & Chemical Equations

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Tro 4th Edition

Ch.3 - Molecules, Compounds & Chemical Equations

Problem 52b,c

Name each acid. b. HClO₂(aq) c. H₂SO₄(aq)

Problem 54

Write the formula for each acid. a. phosphoric acid b. hydrocyanic acid c. chlorous acid

Problem 55d

Refer to the nomenclature flowchart (Figure 3.11) to name each compound. d. HC2H3O2(aq)

Problem 56a

Refer to the nomenclature flowchart (Figure 3.11) to name each compound. a. HNO₂(aq)

Problem 57a,b,c

Refer to the nomenclature flowchart (Figure 3.11) to name each compound. a. KClO₃ b. I₂O₅ c. PbSO₄

Problem 58a,b

Refer to the nomenclature flowchart (Figure 3.11) to name each compound. a. XeO₃ b. KClO

Problem 59a,b,c,d

Calculate the formula mass for each compound. a. NO₂ c. C₆H₁₂O₆ b. C₄H₁₀ d. Cr(NO₃)₃

Problem 60a,b,c,d

Calculate the formula mass for each compound. a. MgBr₂ b. HNO₂ c. CBr₄ d. Ca(NO₃)₂

Problem 61

Calculate the number of moles in each sample: a. 72.5 g CCl4 b. 12.4 g C12H22O11 c. 25.2 kg C2H2 d. 12.3 g dinitrogen monoxide

Problem 62

What is the mass of each sample? a. 15.7 mol HNO3 b. 1.04 × 10^-3 mol H2O2 c. 72.1 mmol SO2 d. 1.23 mol xenon difluoride

Problem 63

Determine the number of moles (of molecules or formula units) in each sample. a. 25.5 g NO₂ b. 1.25 kg CO₂ c. 38.2 g KNO₃ d. 155.2 kg Na₂SO₄

Problem 64a

Determine the number of moles (of molecules or formula units) in each sample. a. 55.98 g CF₂Cl₂

Problem 64b

Determine the number of moles (of molecules or formula units) in each sample. b. 23.6 kg Fe(NO₃)₂

Problem 64c

Determine the number of moles (of molecules or formula units) in each sample. c. 0.1187 g C₈H₁₈

Problem 64d

Determine the number of moles (of molecules or formula units) in each sample. d. 195 kg CaO

Problem 65a,c,d

How many molecules are in each sample? a. 6.5 g H₂O c. 22.1 g O₂ d. 19.3 g C₈H₁₀

Problem 66

How many molecules (or formula units) are in each sample? a. 85.26 g CCl₄ b. 55.93 kg NaHCO₃ c. 119.78 g C₄H₁₀ d. 4.59×10⁵ g Na₃PO₄

Problem 67a,b,c

Calculate the mass (in g) of each sample. a. 5.94×10²⁰ SO₃ molecules b. 2.8×10²² H₂O molecules c. 1 glucose molecule (C₆H₁₂O₆)

Problem 68a

Calculate the mass (in g) of each sample. a. 4.5×10²⁵ O₃ molecules

Problem 68b,c

Calculate the mass (in g) of each sample. b. 9.85×10¹⁹ CCl₂F₂ molecules c. 1 water molecule

Problem 69

A sugar crystal contains approximately 1.8×10¹⁷ sucrose (C₁₂H₂₂O₁₁) molecules. What is its mass in mg?

Problem 70

A salt crystal has a mass of 0.12 mg. How many NaCl formula units does it contain?

Problem 71a,b

Calculate the mass percent composition of carbon in each carbon-containing compound. a. CH₄ b. C₂H₆

Problem 71c

Calculate the mass percent composition of carbon in each carbon-containing compound. c. C₂H₂

Problem 71d

Calculate the mass percent composition of carbon in each carbon-containing compound. d. C₂H₅Cl

Problem 72a,b

Calculate the mass percent composition of nitrogen in each nitrogen-containing compound. a. N₂O b. NO

Problem 72c

Calculate the mass percent composition of nitrogen in each nitrogen-containing compound. c. NO₂

Problem 73

Most fertilizers consist of nitrogen-containing compounds such as NH₃, CO(NH₂)₂, NH₄NO₃, and (NH₄)₂SO₄. Plants use the nitrogen content in these compounds for protein synthesis. Calculate the mass percent composition of nitrogen in CO(NH₂)₂.

Problem 74

Iron in the earth is in the form of iron ore. Common ores include Fe₂O₃ (hematite), Fe₃O₄ (magnetite), and FeCO₃ (siderite). Calculate the mass percent composition of iron for each of these iron ores. Which ore has the highest iron content?

Problem 75

Copper(II) fluoride contains 37.42% F by mass. Calculate the mass of fluorine (in g) in 55.5 g of copper(II) fluoride.