GENERAL CHEMISTRY-SOLUTIONS MANUAL
11th Edition
ISBN: 9780132925044
Author: Petrucci
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Textbook Question
Chapter 4, Problem 141SAE
In the decomposition of silver carbonate to form metallic silver, carbon dioxide gas, and oxygen gas, (a) one mol of oxygen gas is formed forevery 2mol of carbon dioxide gas; (b) 2 mol of silver metal is formed for every 1 mol of oxygen gas; (c) equal numbers of moles of carbon dioxide and oxygen gases are produced; (d) the same number of moles of saver metal are formed as of the silver carbonate decomposed.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Iron(II) sulfate forms several hydrates with the general formula FeSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure FeSO4 behind.
Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by45.%. Which hydrate is it? That is, what is x?
Copper(II) sulfate forms several hydrates with the general formula CuSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CuSO4 behind.
Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 31.%. Which hydrate is it? That is, what is x?
Photosynthesis is a process that incorporates carbon dioxide and water and yields food in the form of glucose (CGH1206) for the plant with oxygen (02) as the by-product. In a (5) five minute period a tree consumes 600 grams of water and enough carbon dioxide that is in excessive amounts in the atmosphere. Determine the amount of glucose and oxygen that is produced
Chapter 4 Solutions
GENERAL CHEMISTRY-SOLUTIONS MANUAL
Ch. 4 - Balance the following equations by inspection. a....Ch. 4 - Balance the following equations by inspection. a....Ch. 4 - Balance the following equations by inspection. a....Ch. 4 - Balance the following equations by inspection. a....Ch. 4 - Write balanced equations based on the information...Ch. 4 - Write balanced equations based on the information...Ch. 4 - Write balanced equations to represent the complete...Ch. 4 - Write balanced equations to represent the complete...Ch. 4 - Write balanced equations to represent a. the...Ch. 4 - Write balanced equations to represent: a. the...
Ch. 4 - Write a balanced chemical equation for the...Ch. 4 - Write a balanced chemical equation for the...Ch. 4 - Prob. 13ECh. 4 - A 3.104 g sample of an oxide of manganese contains...Ch. 4 - Iron metal reacts with chlorine gas. How many...Ch. 4 - If 75.8gPCI2 is produced by the reaction...Ch. 4 - A laboratory method of preparing O2g involves the...Ch. 4 - A commercial method of manufacturing hydrogen...Ch. 4 - How many grams of Ag2CO2 are decomposed to yield...Ch. 4 - How many kilograms of HNO2 are consumed to produce...Ch. 4 - The reaction of calcium hydride with water can be...Ch. 4 - The reaction of potassium superoxide, KO2, is used...Ch. 4 - Prob. 23ECh. 4 - Sold silver oxide, Ag2O (s), decomposes at...Ch. 4 - Decarborane, B10H14, was used as a fuel for...Ch. 4 - The rocket boosters of the space shuttle...Ch. 4 - Prob. 27ECh. 4 - An excess of aluminum foil is allowed to react...Ch. 4 - Prob. 29ECh. 4 - Prob. 30ECh. 4 - What are the molarities of the following solutes...Ch. 4 - Prob. 32ECh. 4 - What are the molarities of the following solutes?...Ch. 4 - What ere the molarities of the following solutes?...Ch. 4 - How much a. glucose, C5H12O5, in grams, must be...Ch. 4 - Prob. 36ECh. 4 - Prob. 37ECh. 4 - In many communities, water is fluoridated to...Ch. 4 - Prob. 39ECh. 4 - Prob. 40ECh. 4 - Prob. 41ECh. 4 - Prob. 42ECh. 4 - A 10.00 mL sample of 2.05MKNO2 is diluted to a...Ch. 4 - What volume of 2.00MAgNO2 must be diluted with...Ch. 4 - Water is evaporated from 125 mL of 0.198MK2SO4...Ch. 4 - A 25.0 mL sample of HCl(aq) is diluted to a volume...Ch. 4 - Prob. 47ECh. 4 - Prob. 48ECh. 4 - Prob. 49ECh. 4 - Excess NaHCO2 is added to 525 mL of 0.220MCu(...Ch. 4 - How many milliliters of 0.650MK2CrO4 are needed to...Ch. 4 - Consider the reaction below....Ch. 4 - Exactly 1.00 mL of an aqueous solution of HNO2 is...Ch. 4 - A 5.00 mL sample of an aqueous solution of H2PO4...Ch. 4 - Prob. 55ECh. 4 - Prob. 56ECh. 4 - How many grams of Ag2CrO4 will precipitate if...Ch. 4 - What volume of MKMnO4 is necessary to convert 12.5...Ch. 4 - Prob. 59ECh. 4 - A method of lowering the concentration of HCI(aq)...Ch. 4 - Prob. 61ECh. 4 - A 25.00 mL sample of HCI(aq) was to a 0.1000 g...Ch. 4 - How many moles of NO(g) can be produced in the...Ch. 4 - The reaction of calcium hydride and water produces...Ch. 4 - A 0.696 mol sample of Cu is added to 136 mL of...Ch. 4 - How many grams of H2O are produced by the reaction...Ch. 4 - Prob. 67ECh. 4 - Lithopone is a brilliant white pigment used in...Ch. 4 - Ammonia can be generated by heating together he...Ch. 4 - Chlorine can be generated by heating together...Ch. 4 - Chromium(II) sulfate. CrSO4, is a reagent that has...Ch. 4 - Titanium tetrachloride, TiCl4 , is prepared by the...Ch. 4 - In the reaction of 277 g CCI4 an excess of HF,...Ch. 4 - In the reaction shown, 100.0gC5H10OH yielded 64.0...Ch. 4 - Prob. 75ECh. 4 - Nitrogen gas, N2 can be prepared by passing...Ch. 4 - The reactionof 15.0 g C4H2OH, 22.4 g NaBr, and...Ch. 4 - Prob. 78ECh. 4 - How many grams of commercial acetic acid (97%...Ch. 4 - Suppose that reactions (a) and (b) each have a 92%...Ch. 4 - An essentially 100% yield is necessary for a...Ch. 4 - Prob. 82ECh. 4 - How many grams of HCI are consumed the reaction of...Ch. 4 - How many grams of CO2 are produced in the complete...Ch. 4 - Dichlorodifluoromethane, once widely used a...Ch. 4 - Prob. 86ECh. 4 - Prob. 87ECh. 4 - Sodium bromide, used to produce silver bromide for...Ch. 4 - Prob. 89ECh. 4 - The following set of reactions is to be used as...Ch. 4 - Prob. 91ECh. 4 - A mixture of Fe2O2 and FeO was analyzed and found...Ch. 4 - Prob. 93IAECh. 4 - Prob. 94IAECh. 4 - Prob. 95IAECh. 4 - Prob. 96IAECh. 4 - Hydrogen gas, H2O, is passed over Fe2O2(s) at 400...Ch. 4 - A sulfide of iron, 36.5% S by mass, is heated in...Ch. 4 - Prob. 99IAECh. 4 - Prob. 100IAECh. 4 - What volume of 0.149 M HCI must be added to 1.00 ×...Ch. 4 - Prob. 102IAECh. 4 - Prob. 103IAECh. 4 - Prob. 104IAECh. 4 - Prob. 105IAECh. 4 - Prob. 106IAECh. 4 - Prob. 107IAECh. 4 - Prob. 108IAECh. 4 - Prob. 109IAECh. 4 - Prob. 110IAECh. 4 - Prob. 111IAECh. 4 - A 0.155 g sample of an Al-Mg alloy reacts with an...Ch. 4 - Prob. 113IAECh. 4 - The following chemical equation represents the...Ch. 4 - Prob. 115IAECh. 4 - Prob. 116IAECh. 4 - Prob. 117IAECh. 4 - Prob. 118IAECh. 4 - Write a chemical equation to represent the...Ch. 4 - Prob. 120IAECh. 4 - Prob. 121IAECh. 4 - When sulfur (S5) and chlorine are mixed in a...Ch. 4 - Prob. 123IAECh. 4 - Prob. 124IAECh. 4 - Prob. 125IAECh. 4 - Prob. 126IAECh. 4 - Prob. 127IAECh. 4 - Melamine, C2N2( NH2)2, is used in adhesives and...Ch. 4 - Prob. 129IAECh. 4 - A fundamental principle green chemistry is atom...Ch. 4 - The industrial productionof hydrazine (N2H2) by...Ch. 4 - Prob. 132IAECh. 4 - Prob. 133FPCh. 4 - Prob. 134FPCh. 4 - Prob. 135SAECh. 4 - Prob. 136SAECh. 4 - Prob. 137SAECh. 4 - Prob. 138SAECh. 4 - Prob. 139SAECh. 4 - Prob. 140SAECh. 4 - In the decomposition of silver carbonate to form...Ch. 4 - Prob. 142SAECh. 4 - What is the volume (in ML) of 0.160MKNO2 that must...Ch. 4 - To prepare a solution that is 0.50 M KCI starting...Ch. 4 - An aqueous solution that is 5.30% LiBr by mass...Ch. 4 - Prob. 146SAECh. 4 - Consider the reaction 2Fe2O2+3C4Fe+3CO2 . What is...Ch. 4 - Prob. 148SAECh. 4 - The incomplete combustion of gasoline produces...Ch. 4 - Prob. 150SAECh. 4 - Prob. 151SAECh. 4 - Prob. 152SAECh. 4 - For each of the following compounds,write a...Ch. 4 - Appendix E descries a useful study aid known as...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 3.50 A test of an automobile engine's exhaust revealed that g of NO2 was emitted in 10 minutes of operation. How many moles of NO2 would this engine release if it were used for a 45-minute commute, assuming that this mea- sured number is representative of the emission under all circumstances?arrow_forwardAn air bag is deployed by utilizing the following re tion the nitrogen gas produced inflates the air bag): :math>2NaN3(s)2Na(s)+3N2(g) 10.5 g of NaN1 is decomposed, what theoretical mass of sodium should be produced? If only 2.84 g of sodium is actually collected, what is the percent yield?arrow_forwardWhen potassium chlorate is subjected to high temperatures, it decomposes into potassium chloride and oxygen. (a) Write a balanced equation for the decomposition. (b) In this decomposition, the actual yield is 83.2%. If 198.5 g of oxygen are produced, how much potassium chlorate decomposed?arrow_forward
- You have a chemical in a sealed glass container filled with air. The setup is sitting on a balance as shown below. The chemical is ignited by means of a magnifying glass focusing sunlight on the reactant. After the chemical has completely burned, which of the following is true? Explain your answer. a. The balance will read less than 250.0 g. b. The balance will read 250.0 g. c. The balance will read greater than 250.0 g. d. The scales reading cannot be determined without knowing the identity of the chemical.arrow_forwardA possible practical way to eliminate oxides of nitrogen(such as NO2 ) from automobile exhaust gases uses cyanuricacid, C3N3(OH)3 . When heated to the relatively lowtemperature of 625°F, cyanuric acid converts to gaseousisocyanic acid (HNCO). Isocyanic acid reacts with NO2 inthe exhaust to form nitrogen, carbon dioxide, and water,all of which are normal constituents of the air. (a) Write balanced equations for these two reactions. (b) If the process described earlier became practical, howmuch cyanuric acid (in kilograms) would be requiredto absorb the 1.71010kgNO2 generated annuallyin auto exhaust in the United States?arrow_forwardThe meat from one hazelnut has a mass of 0.985 g. (a) What is the mass of a millionth of a mole (106) of hazelnut meats? (A millionth of a mole is also called a micromole.) (b) How many moles are in a pound of hazelnut meats?arrow_forward
- or each of the following reactions, give the balanced chemical equation for the reaction and state the meaning of the equation in terms of individual molecules and in terms of moles of molecules. msp;MnO2(s)+Al(s)Mn(s)+Al2O3(s) msp;B2O3(s)+CaF2(s)BF3(g)+CaO(s) msp;NO2(g)+H2O(l)HNO3(aq)+NO(g) msp;C6H2(g)+H2C6(g)H12(g)arrow_forwardA 100.0-g mixture made up of NaCl03, Na2CO3, NaCl, and NaHCO3 is heated, producing 5.95 g of oxygen, 1.67 g of water, and 14.5 g of carbon dioxide. NaCl does not react under the conditions of the experiment. The equations for the reactions that take place are: 2NaClO3(s)2NaCl(s)+3O2(g)Na2CO3(s)2Na2O(s)+CO2(g)2NaHCO3(s)Na2O(s)+2CO2(g)+H2O Assuming 100% decomposition of NaClO3, Na2CO3, and NaHCO3, what is the composition of the mixture in grams?arrow_forwardWhen elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. :math>C(s)+O2(g)CO2(g) wever, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. :math>2C(s)+O2(g)CO(g) at mass of each product is expected when a 5.00-g sample of pure carbon is burned under each of these conditions?arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningWorld of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College Div
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
World of Chemistry
Chemistry
ISBN:9780618562763
Author:Steven S. Zumdahl
Publisher:Houghton Mifflin College Div
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY