Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 3, Problem 67RQ
3.67 How many kilograms of a fertilizer made of pure
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Chapter 3 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 3 - Practice Exercise 3.1
How many moles of aluminum...Ch. 3 - In a reaction to synthesize nitrogen triiodide....Ch. 3 - Your laboratory balance can weigh samples to three...Ch. 3 - How many atoms of gold are there in one ounce of...Ch. 3 - What is the average mass of one molecule of table...Ch. 3 - Most chemistry laboratories have balances that can...Ch. 3 - Practice Exercise 3.7
Aluminum sulfate is...Ch. 3 - How many moles of nitrogen atoms are combined with...Ch. 3 - Sodium bicarbonate is used to soften water. How...Ch. 3 - How many grams of iron arc needed to combine with...
Ch. 3 - Bromine trifluoride explodes upon contact with...Ch. 3 - When 0.5462 g of a compound was decomposed. 0.2012...Ch. 3 - An organic compound weighing 0.6672 g is...Ch. 3 - Calculate the theoretical percentage composition...Ch. 3 - Practice Exercise 3.15
Calculate the theoretical...Ch. 3 - A 1.525 g sample of a compound between nitrogen...Ch. 3 - Practice Exercise 3.17
Sulfur forms two different...Ch. 3 - Practice Exercise 3.18
A compound of nitrogen and...Ch. 3 - When aluminum it produced by electrolysis we get...Ch. 3 - A white solid used to whiten paper has the...Ch. 3 - Cinnamon gets some of its flavor from...Ch. 3 - Prob. 22PECh. 3 - Prob. 23PECh. 3 - The empirical formula of hydrazine is NH2 and its...Ch. 3 - After determining that the empirical formulas of...Ch. 3 - Practice Exercise 3.26
When aqueous solutions of...Ch. 3 - Practice Exercise 3.27
Write the balanced chemical...Ch. 3 - In the reaction 2SO2(g)+O2(g)2SO3(g), how many...Ch. 3 - Practice Exercise 3.29
How many moles of sulfuric...Ch. 3 - Practice Exercise 3.30
Using the information in...Ch. 3 - How many grams of carbon dioxide are produced by...Ch. 3 - Practice Exercise 3.32
The reaction between the...Ch. 3 - Practice Exercise 3.33
In an industrial process...Ch. 3 - Practice Exercise 3.34
In the synthesis of aspirin...Ch. 3 - Practice Exercise 3.35
Ethanol, , can be converted...Ch. 3 - In producing a certain drug, one synthetic route...Ch. 3 - What is the definition of the mole?Ch. 3 - 3.2 Why are moles used, when all stoichiometry...Ch. 3 - Which contains more molecules:...Ch. 3 - How would Avogadros number change if the atomic...Ch. 3 - 3.5 What information is required to convert grams...Ch. 3 - Using atomic mass units, how would you estimate...Ch. 3 - How many moles of iron atoms are in one mole of...Ch. 3 - Write all the mole-to-mole conversion factors that...Ch. 3 - What information is required to convert grams of a...Ch. 3 - Why is the expression 1.0 mol of oxygen ambiguous?...Ch. 3 - 3.11 The atomic mass of aluminum is 26.98. What...Ch. 3 - 3.12 If you are given the mass of two elements and...Ch. 3 - How can percentage composition be used to identify...Ch. 3 - In general, what fundamental information, obtained...Ch. 3 - 3.15 Why can percentage composition be used to...Ch. 3 - Why are empirical formulas always used for ionic...Ch. 3 - 3.17 Under what circumstances can we change, or...Ch. 3 - How many distinct empirical formulas are shown by...Ch. 3 - 3.19 When balancing a chemical reaction, what...Ch. 3 - When given the unbalanced equation...Ch. 3 - Give a step-by-step procedure for estimating the...Ch. 3 - Prob. 22RQCh. 3 - 3.23 What information is required to determine how...Ch. 3 - A mixture of 0.020 mol of Mg and 0.020 mol of Cl2...Ch. 3 - In a report to a supervisor, a chemist described...Ch. 3 - On April 16, 1947, in Texas City, Texas, two cargo...Ch. 3 - What is a limiting reactant? And why does the...Ch. 3 - Molecules containing A and B react to form AB as...Ch. 3 - 3.29 Explain why the actual yield is always less...Ch. 3 - Prob. 30RQCh. 3 - 3.31 Determine the mass in grams of each of die...Ch. 3 - Determine the mass in grams of the following: (a)...Ch. 3 - 3.33 Calculate the formula mass of each of the...Ch. 3 - Calculate the formula mass of each of the...Ch. 3 - Calculate the mass in grams of the following. (a)...Ch. 3 - What is the mass in grams of the following? (a)...Ch. 3 - Calculate the number of moles of each compound in...Ch. 3 - Calculate the number of moles of each compound in...Ch. 3 - How many moles of nickel are in 17.7 g of Ni?Ch. 3 - How many moles of chromium are in 85.7 g of Cr?Ch. 3 - How many moles of tantalum atoms correspond to...Ch. 3 - How many moles of iodine molecules correspond to...Ch. 3 - 3.43 A nanotechnology experiment requires atoms...Ch. 3 - What is the mass, in grams, of 41017 atoms of gold...Ch. 3 - 3.45 How many atoms are in 6.00 g of carbon-12?
Ch. 3 - How many atoms are in 1.50 mol of carbon-12? How...Ch. 3 - Sucrose (table sugar) has the formula C12H22O11....Ch. 3 - Nail polish remover is usually the volatile liquid...Ch. 3 - 3.79 How many moles of Bi atoms are needed to...Ch. 3 - 3.50 How many moles of vanadium atoms, V, are...Ch. 3 - How many moles of Cr are in 2.16 mol of Cr2O3?Ch. 3 - How many moles of O atoms are in 4.25 mol of...Ch. 3 - Aluminum sulfate, Al2(SO4)3, is a compound used in...Ch. 3 - Magnetite is a magnetic iron ore. Its formula is...Ch. 3 - 3.55 How many moles of H2andN2 can be formed by...Ch. 3 - 3.56 How many moles of S are needed to combine...Ch. 3 - 3.57 How many moles of UF6 would have to be...Ch. 3 - 3.58 How many moles of Fe3O4 are required to...Ch. 3 - 3.59 How many atoms of carbon are combined with...Ch. 3 - 3.60 How many atoms of hydrogen are found in 2.31...Ch. 3 - 3.61 What is the total number of C, H, and O atoms...Ch. 3 - 3.62 What is the total number of N, H, and O atoms...Ch. 3 - 3.63 Calcium carbide, CaC2, was once used to make...Ch. 3 - 3.64 Iodized salt contains a trace amount of...Ch. 3 - How many moles of nitrogen, N, are in 0.650 mol of...Ch. 3 - 3.66 How many moles of nitrogen, N, are in 0.556...Ch. 3 - 3.67 How many kilograms of a fertilizer made of...Ch. 3 - 3.68 How many kilograms of a fertilizer made of...Ch. 3 - 3.69 Calculate the percentage composition by mass...Ch. 3 - Calculate the percentage composition by mass for...Ch. 3 - Which has a higher percentage of oxygen: morphine...Ch. 3 - Which has a higher percentage of nitrogen:...Ch. 3 - Freon is a trade name for a group of gaseous...Ch. 3 - Which has a higher percentage of fluorine:...Ch. 3 - It was found that 2.35 g of a compound of...Ch. 3 - Prob. 76RQCh. 3 - Phencyclidine (angel dust) is C17H25N. A sample...Ch. 3 - The hallucinogenic drug LSD has the molecular...Ch. 3 - How many grams of O are combined with 7.141021...Ch. 3 - How many grams of C are combined with 4.251023...Ch. 3 - Write empirical formulas for the following...Ch. 3 - What are the empirical formulas of the following...Ch. 3 - 3.83 Radioactive sodium pertechnetate is used as a...Ch. 3 - A sample of Freon was found to contain 0.423 g of...Ch. 3 - 3.85 Cinnamic acid, a compound related to the...Ch. 3 - 3.86 Vanillin, a compound used as a flavoring...Ch. 3 - A dry-cleaning fluid composed of only carbon and...Ch. 3 - One compound of mercury with a molar mass of 519...Ch. 3 - When 0.684 g of an organic compound containing...Ch. 3 - Prob. 90RQCh. 3 - 3.91 When 6.853 mg of a sex hormone was burned in...Ch. 3 - When a sample of a compound in the vitamin D...Ch. 3 - The following are empirical formulas and the...Ch. 3 - The following are empirical formulas and the...Ch. 3 - The compound described in Problem 3.91 was found...Ch. 3 - 3.96 The compound described in Problem 3.92 was...Ch. 3 - A sample of a compound of mercury and bromine with...Ch. 3 - A 0.6662 g sample of antimonal saffron, which is a...Ch. 3 - A sample of a compound of C, H, N, and O, was...Ch. 3 - 3.100 Strychnine, a deadly poison, has a formula...Ch. 3 - Prob. 101RQCh. 3 - Balance the following equations....Ch. 3 - Write the following as balanced chemical...Ch. 3 - 3.104 Write the following as balanced chemical...Ch. 3 - Prob. 105RQCh. 3 - Prob. 106RQCh. 3 - 3.107 The balanced chemical equation for the...Ch. 3 - 3.108 Draw a molecular-level diagram for the...Ch. 3 - 3.109 Write the equation that expresses in...Ch. 3 - The conversion of one air pollutant, nitrogen...Ch. 3 - A balanced chemical equation contains the term...Ch. 3 - 3.112 A balanced chemical equation contains the...Ch. 3 - 3.113 Chlorine is used by textile manufacturers to...Ch. 3 - The octane in gasoline burns according to the...Ch. 3 - Propane burns according to the following equation:...Ch. 3 - The following reaction is used to extract gold...Ch. 3 - The incandescent white of a fireworks display is...Ch. 3 - The combustion of butane, C4Hl0, produces carbon...Ch. 3 - In dilute nitric acid, HNO3, copper metal...Ch. 3 - 3.120 The reaction of hydrazine, , with hydrogen...Ch. 3 - Oxygen gas can be produced in the laboratory by...Ch. 3 - Oxygen gas can be produced in the laboratory by...Ch. 3 - Using the balanced equation...Ch. 3 - 3.124 Using the balanced chemical equation in...Ch. 3 - The thermite reaction between powdered aluminum...Ch. 3 - 3.126 Ethanol is synthesized for industrial use...Ch. 3 - 3.127 Silver nitrate, , reacts with iron(III)...Ch. 3 - Chlorine dioxide, ClO2, has been used as a...Ch. 3 - Some of the acid in acid rain is produced by the...Ch. 3 - Phosphorus pentachloride reacts with water to give...Ch. 3 - Barium sulfate, BaSO4, is made by the following...Ch. 3 - Prob. 132RQCh. 3 - Aluminum sulfate can be made by the following...Ch. 3 - 3.134 The combustion of methyl alcohol in an...Ch. 3 - Manganese(III) fluoride, MnF3, can be prepared by...Ch. 3 - Prob. 136RQCh. 3 - Mercury is an environmental pollutant because it...Ch. 3 - Prob. 138RQCh. 3 - Prob. 139RQCh. 3 - *3.140 A compound of Ca, C, N, and S was subjected...Ch. 3 - 3.141 Ammonium nitrate will detonate if ignited in...Ch. 3 - A lawn fertilizer is rated as 6.00% nitrogen,...Ch. 3 - Nitrogen is the active ingredient in many...Ch. 3 - Based solely on the amount of available carbon,...Ch. 3 - According to NASA, the space shuttles external...Ch. 3 - For a research project, a student decided to test...Ch. 3 - 3.147 Chlorine atoms cause chain reactions in the...Ch. 3 - Lime, CaO, can be produced in two steps as shown...Ch. 3 - A newspaper story describing the local celebration...Ch. 3 - Suppose you had one mole of pennies and you were...Ch. 3 - Using the above two questions as examples, devise...Ch. 3 - 3.152 List the different: ways in which a chemist...
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- You take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.arrow_forwardTungsten (W) metal, which is used to make incandescent bulb filaments, is produced by the reaction WO3+3H23H2O+W How many grams of H2 are needed to produce 1.00 g of W?arrow_forward4.28 One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) If 43.0 kg of NH3 reacts with 35.4 kg of O2, what mass of NO forms?arrow_forward
- Phosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water. 14P4O10(s)+32H2O(l)H3PO4(aq);H=96.2kJ What is H for the reaction involving 1 mol of P4O10? P4O10(s)+6H2O(l)4H3PO4(aq)arrow_forwardAspirin (C9H8O4) is synthesized by reacting salicylic acid (C7H6O3) with acetic anhydride (C4H6O3). The balanced equation is C7H6O3+C4H6O3C9H8O4+HC2H3O2 a. What mass of acetic anhydride is needed to completely consume 1.00 102 g salicylic acid? b. What is the maximum mass of aspirin (the theoretical yield) that could be produced in this reaction?arrow_forwardWhat is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?arrow_forward
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