Introduction to General, Organic and Biochemistry
12th Edition
ISBN: 9780357391594
Author: Frederick A. Bettelheim; William H. Brown; Mary K. Campbell
Publisher: Cengage Learning US
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Chapter 4, Problem 73P
Interpretation Introduction
Interpretation:
The balanced reaction for burning of MTBE should be determined.
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Chapter 4 Solutions
Introduction to General, Organic and Biochemistry
Ch. 4.2 - Problem 4-1 Following is an unbalanced equation...Ch. 4.2 - Problem 4-2 Balance this equation:Ch. 4.2 - Prob. 4.3QCCh. 4.3 - Problem 4-4 When a solution of copper(II)...Ch. 4.4 - Problem 4-5 In each equation, identify the...Ch. 4.5 - Problem 4-6 What is (a) the molecular weight of...Ch. 4.6 - Prob. 4.7QCCh. 4.6 - Problem 4-8 We wish to weigh 2.84 mol of sodium...Ch. 4.6 - Problem 4-9 How many moles of C atoms, H atoms,...Ch. 4.6 - Problem 4-10 How many moles of copper(I) ions,...
Ch. 4.6 - Prob. 4.11QCCh. 4.7 - Prob. 4.12QCCh. 4.7 - Prob. 4.13QCCh. 4.7 - Problem 4-14 Ethanol is produced industrially by...Ch. 4.7 - Prob. 4.15QCCh. 4.7 - Prob. 4.16QCCh. 4.8 - How many calories are required to heat 731g of...Ch. 4.8 - A 100g piece of iron at 25C is heated by adding...Ch. 4.8 - It required 88.2 cal to heat 13.4g of an unknown...Ch. 4.9 - Solid iron and oxygen gas react to form solid...Ch. 4 - 4-17 Balance each equation.Ch. 4 - 4-18 Balance each equation.Ch. 4 - Prob. 3PCh. 4 - 4-20 Calcium oxide is prepared by heating...Ch. 4 - 4-21 The brilliant white light in some firework...Ch. 4 - Prob. 6PCh. 4 - 4-23 When solid carbon burns in a limited supply...Ch. 4 - Prob. 8PCh. 4 - 4-25 In the chemical test for arsenic, the gas...Ch. 4 - Prob. 10PCh. 4 - Prob. 11PCh. 4 - 4-28 Answer true or false. (a) A net ionic...Ch. 4 - 4-29 Balance these net ionic equations. (a)...Ch. 4 - 4-30 In the equation (a) Identify the spectator...Ch. 4 - 4-31 Predict whether a precipitate will form when...Ch. 4 - 4-32 When a solution of ammonium chloride is added...Ch. 4 - 4-33 When a solution of hydrochloric acid, HCl, is...Ch. 4 - Prob. 18PCh. 4 - Prob. 19PCh. 4 - 4-36 Using the solubility generalizations given in...Ch. 4 - 4-37 Answer true or false. (a) When a substance is...Ch. 4 - Prob. 22PCh. 4 - Prob. 23PCh. 4 - Prob. 24PCh. 4 - Prob. 25PCh. 4 - 4-42 Calculate the formula weight of: (a) KCl (b)...Ch. 4 - 4-43 Calculate the molecular weight of: (a)...Ch. 4 - 4-44 Answer true or false. (a) The mole is a...Ch. 4 - 4-45 Calculate the number of moles in: (a) 32 g of...Ch. 4 - 4-46 Calculate the number of grams in: (a) 1.77...Ch. 4 - 4-47 Calculate the number of moles of: (a) O atoms...Ch. 4 - 4-48 Calculate the number of moles of: (a) S2-...Ch. 4 - 4-49 Calculate the number of: (a) nitrogen atoms...Ch. 4 - 4-50 How many molecules are in each of the...Ch. 4 - 4-51 What is the mass in grams of each number of...Ch. 4 - 4-52 The molecular weight of hemoglobin is about...Ch. 4 - 4-53 A typical deposit of cholesterol, C27H46O, in...Ch. 4 - 4-54 Answer true or false. (a) Stoichiometry is...Ch. 4 - 4-55 For the reaction: (a) How many moles of N2...Ch. 4 - 4-56 Magnesium reacts with sulfuric acid according...Ch. 4 - 4-57 Chloroform, CHCl3, is prepared industrially...Ch. 4 - 4-58 At one time, acetaldehyde was prepared...Ch. 4 - 4-59 Chlorine dioxide, ClO2, is used for bleaching...Ch. 4 - 4-60 Ethanol, C2H6O, is added to gasoline to...Ch. 4 - 4-61 In photosynthesis, green plants convert CO2...Ch. 4 - 4-62 Iron ore is converted to iron by heating it...Ch. 4 - Prob. 47PCh. 4 - 4-64 Aspirin is made by the reaction of salicylic...Ch. 4 - 4-65 Suppose the preparation of aspirin from...Ch. 4 - 4-66 Benzene reacts with bromine to produce...Ch. 4 - 4-67 Ethyl chloride is prepared by the reaction of...Ch. 4 - 4-68 Diethyl ether is made from ethanol according...Ch. 4 - Prob. 53PCh. 4 - How many calories are required to heat the...Ch. 4 - Prob. 55PCh. 4 - Prob. 56PCh. 4 - Prob. 57PCh. 4 - Prob. 58PCh. 4 - 4-71 Which of these reactions are exothermic, and...Ch. 4 - Prob. 60PCh. 4 - Prob. 61PCh. 4 - Prob. 62PCh. 4 - Prob. 63PCh. 4 - Prob. 64PCh. 4 - 4-77 To convert 1 mol of iron(III) oxide to its...Ch. 4 - 4-78 (Chemical Connections 4A) How does fluoride...Ch. 4 - Prob. 67PCh. 4 - Prob. 68PCh. 4 - 4-81 (Chemical Connections 4C) Balance the lithium...Ch. 4 - 4-82 When gaseous dinitrogen pentoxide, N2O5, is...Ch. 4 - Prob. 71PCh. 4 - Prob. 72PCh. 4 - Prob. 73PCh. 4 - 4-86 When an aqueous solution of Na3PO4 is added...Ch. 4 - Prob. 75PCh. 4 - 4-88 Chlorophyll, the compound responsible for the...Ch. 4 - 4-89 If 7.0 kg of is added to 11.0 kg of to form...Ch. 4 - 4-90 Lead(lI) nitrate and aluminum chloride react...Ch. 4 - 4-91 Assume that the average red blood cell has a...Ch. 4 - 4-92 Reaction of pentane, C5H12, with oxygen, O2,...Ch. 4 - 4-93 Ammonia is prepared industrially by the...Ch. 4 - 4-94 2,3,7,8-Tetrachlorodibenzo-p-dioxin (TCDD) is...Ch. 4 - Prob. 83PCh. 4 - Prob. 84PCh. 4 - Prob. 85PCh. 4 - Prob. 86PCh. 4 - Prob. 87PCh. 4 - Prob. 88PCh. 4 - Prob. 89PCh. 4 - Prob. 90PCh. 4 - Prob. 91PCh. 4 - 4-102 Aspartame, an artificial sweetener used as a...Ch. 4 - 4-103 Caffeine, a central nervous system...Ch. 4 - Prob. 94P
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- 4-20 Calcium oxide is prepared by heating limestone (calcium carbonate, CaCO3) to a high temperature, at which point it decomposes to calcium oxide and carbon dioxide. Write a balanced equation for this preparation of calcium oxide.arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forward4-25 In the chemical test for arsenic, the gas arsme, AsH3, is prepared. When arsine is decomposed by heating, arsenic metal deposits as a mirror-like coating on the surface of a glass container and hydrogen gas, H2, is given off. Write a balanced equation for the decomposition of arsine.arrow_forward
- Ethanol, C2H5OH, is a gasoline additive that can be produced by fermentation of glucose. C6H12O62C2H5OH+2CO2 (a) Calculate the mass (g) of ethanol produced by the fermentation of 1.000 lb glucose. (b) Gasohol is a mixture of 10.00 mL ethanol per 90.00 mL gasoline. Calculate the mass (in g) of glucose required to produce the ethanol in 1.00 gal gasohol. Density of ethanol = 0.785 g/mL. (c) By 2022, the U. S. Energy Independence and Security Act calls for annual production of 3.6 1010 gal of ethanol, no more than 40% of it produced by fermentation of corn. Fermentation of 1 ton (2.2 103 lb) of corn yields approximately 106 gal of ethanol. The average corn yield in the United States is about 2.1 105 lb per 1.0 105 m2. Calculate the acreage (in m2) required to raise corn solely for ethanol production in 2022 in the United States.arrow_forward4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?arrow_forwardAcetone, (CH3)2CO, is an important industrial compound. Although its toxicity is relatively low, workers using it must be careful to avoid flames and sparks because this compound burns readily in air. Write the balanced equation for the combustion of acetone.arrow_forward
- list at least three quantities that must be conserved in chemical reactions.arrow_forwardCarbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.arrow_forwardA power plant is driven by the combustion of a complex fossil fuel having the formula C11H7S. Assume the air supply is composed of only N2 and O2 with a molar ratio of 3.76:1.00, and the N2 remains unreacted. In addition to the water produced, the fuels C is completely combusted to CO2 and its sulfur content is converted to SO2. In order to evaluate gases emitted at the exhaust stacks for environmental regulation purposes, the nitrogen supplied with the air must also be included in the balanced reactions. a Including the N2 supplied m the air, write a balanced combustion equation for the complex fuel assuming 100% stoichiometric combustion (i.e., when there is no excess oxygen in the products and the only C-containing product is CO2). Except in the case of N2, use only integer coefficients. b Including N2 supplied in the air, write a balanced combustion equation for the complex fuel assuming 120% stoichiometric combustion (i.e., when excess oxygen is present in the products and the only C-containing product is CO2). Except in the case of use only integer coefficients c Calculate the minimum mass (in kg) of air required to completely combust 1700 kg of C11H7S. d Calculate the air/fuel mass ratio, assuming 100% stoichiometric combustion. e Calculate the air/fuel mass ratio, assuming 120% stoichiometric combustion.arrow_forward
- 4-61 In photosynthesis, green plants convert CO2 and H2O to glucose, C6H12O6. How many grams of CO2are required to produce 5.1 g of glucose?arrow_forward4-77 To convert 1 mol of iron(III) oxide to its elements requires 196.5 kcal: How many grams of iron can be produced if 156.0 kcal of heat is absorbed by a large-enough sample of iron(III) oxide?arrow_forward4-62 Iron ore is converted to iron by heating it with coal (carbon), and oxygen according to the following equation: If the process is run until 3940. g of Fe is produced, how many grams of CO2 will also be produced?arrow_forward
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