GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
11th Edition
ISBN: 9780134193601
Author: Petrucci
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Question
Chapter 3, Problem 94IAE
Interpretation Introduction
Interpretation:
The mass percentage of silver from an impure sample of silver should be determined.
Concept introduction:
From the mixture of silver and impurity only silver will react and will form silver chloride. One mole of pure silver produces one mole of silver chloride.
Number of moles is equal to the ratio of mass to the molar mass. The mathematical expression is given by:
Number of moles =
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
1. Provide the chemical formula (including brackets where appropriate) or systematic name for the following compounds.
(a) gold(I) hypoiodite
(b) HI(aq):
(f) Ca(ClO4)2·4H2O:
2. What mass (in g) of chlorine atoms are there in a sample that consists of 5e+23 molecules of molecular chlorine?
INSTRUCTIONS: Report your answer to 3 significant figures in scientific notation unless stated otherwise. DO NOT include the units in your answer.
(c) A metal has six naturally occurring isotopes. The isotopes, their fractions, and their atomic
weights are presented in the table below. Calculate the average atomic weight of the metal.
Fraction
Atomic weight
Isotope 1
0.16%
173.940 amu
Isotope 2
5.26%
175.941 amu
Isotope 3
18.60%
176.943 amu
Isotope 4
27.28%
177.944 amu
Isotope 5
13.62%
178.946 amu
Isotope 6
35.08%
179.947 amu
Element XYZ has two isotopes: XYZ-79 (mass =69.9943 amu) and XYZ-81 (mass=80.9893 amu). If the relative percent abundancy of XYZ-79 is 50.6865% while XYZ-81 is 49.3135%, calculate for the average molar mass of XYZ. Express your answer in 3 significant figures.
Chapter 3 Solutions
GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
Ch. 3 - Refer to the color scheme given Figure 3-3, and...Ch. 3 - Give the molecular formulas for the molecules...Ch. 3 - Give the structure formulas of the molecules shown...Ch. 3 - Give the structure formulas of the molecules shown...Ch. 3 - Calculate the total number of (a) atoms one...Ch. 3 - Determine the mass, in grams, of a. 7.34molNO2 b....Ch. 3 - The amino acid methionine, which is essential in...Ch. 3 - Determine the number of moles of Br2 in a sample...Ch. 3 - Without doing detailed calculations, explain which...Ch. 3 - Without doing detailed calculations, determine...
Ch. 3 - Determine the number of moles of a. N2O4 in a 115...Ch. 3 - Determine the mass, in grams, of a. 2.10102 molS2...Ch. 3 - The content of is 15.5g/100 mLblood. The molar...Ch. 3 - In white phosphorus, P atoms are joined into P,...Ch. 3 - Prob. 15ECh. 3 - Prob. 16ECh. 3 - For the mineral torbernite, Cu( UO2)2( PO4)2,8H2O...Ch. 3 - For the compound Ge[S( CH 2 )4CH2]4 determine a....Ch. 3 - Determine the mass percent H in the hydrocarbon...Ch. 3 - Determine the mass percent O in the mineral...Ch. 3 - Determine the mass percent H in the hydrocarbon...Ch. 3 - Prob. 22ECh. 3 - Determine the mass percent of each of the elements...Ch. 3 - Prob. 24ECh. 3 - Determine the percent, by mass,of the indicated...Ch. 3 - All of the following minerals are semiprecious or...Ch. 3 - Without doing calculations, arrange the following...Ch. 3 - Prob. 28ECh. 3 - Two oxides of sulfur have nearly identical...Ch. 3 - An oxide of chromium used in chrome plating has a...Ch. 3 - Diethylene glycol, used to de-ice aircraft, is a...Ch. 3 - Prob. 32ECh. 3 - Determine the empirical formula of (a) the...Ch. 3 - Prob. 34ECh. 3 - A compound of carbon and hydrogen consists of...Ch. 3 - Selenium, an element used in the manufacture of...Ch. 3 - Indigo, the dye for blue jeans, has a percent...Ch. 3 - Prob. 38ECh. 3 - Prob. 39ECh. 3 - The element X forms the compound XOCI2 containing...Ch. 3 - Prob. 41ECh. 3 - Two compounds of CI and X are found to have...Ch. 3 - A 0.1888 g sample of a hydrocarbon produces 0.6260...Ch. 3 - Para-cresol (p-cresol) is used as a disinfectant...Ch. 3 - Dimethylhydrazine is a carbon-hydrogen-nitrogen...Ch. 3 - Prob. 46ECh. 3 - Without doing detailed calculations, explain which...Ch. 3 - Prob. 48ECh. 3 - A 1.562 g sample of the alcohol CH2CHOHCH2CH2 is...Ch. 3 - Prob. 50ECh. 3 - Indicate the oxidation state of the underlined...Ch. 3 - Indicate the oxidation state of S in (a) SO42 (b)...Ch. 3 - Prob. 53ECh. 3 - Prob. 54ECh. 3 - Prob. 55ECh. 3 - Hydrogen and oxygen usually have oxidation states...Ch. 3 - Prob. 57ECh. 3 - Name these compounds: (a)Ba(...Ch. 3 - Prob. 59ECh. 3 - Prob. 60ECh. 3 - Prob. 61ECh. 3 - Prob. 62ECh. 3 - Write a formula for (a) the chloride of titanium...Ch. 3 - Write formula for (a) an oxide of nitrogen with N...Ch. 3 - Prob. 65ECh. 3 - Supply the formula for the acids: (a) hydrofluoric...Ch. 3 - Name the following compounds and specify which...Ch. 3 - Prob. 68ECh. 3 - Prob. 69ECh. 3 - Prob. 70ECh. 3 - Anhydrous CuSO4 can be used to dry liquids in...Ch. 3 - Anhydrous sodium sulfate, Na2SO4 absorbs water...Ch. 3 - A certain hydrate is found to have the composition...Ch. 3 - An 8.129 g sample of MgSO4H2O is heated until all...Ch. 3 - Prob. 75ECh. 3 - Prob. 76ECh. 3 - Prob. 77ECh. 3 - Prob. 78ECh. 3 - Prob. 79ECh. 3 - Prob. 80ECh. 3 - Prob. 81ECh. 3 - Prob. 82ECh. 3 - The mineral spodumene has the empirical formula...Ch. 3 - Prob. 84IAECh. 3 - Prob. 85IAECh. 3 - The important natural sources of boron compounds...Ch. 3 - Prob. 87IAECh. 3 - By analysis, a compound was found to contain 26.58...Ch. 3 - Prob. 89IAECh. 3 - What is the molecular formula of a hydrocarbon...Ch. 3 - A hydrocarbon mixture consists of 601% by mass of...Ch. 3 - A 0.732 g mature of methane, CH4 and ethane, C2H5...Ch. 3 - The density of a mixture of H2SO4 and water is...Ch. 3 - Prob. 94IAECh. 3 - Prob. 95IAECh. 3 - Prob. 96IAECh. 3 - Prob. 97IAECh. 3 - Prob. 98IAECh. 3 - The metal M forms the sulfate M2( SO4)2. A 0.738 g...Ch. 3 - Prob. 100IAECh. 3 - Prob. 101IAECh. 3 - Prob. 102IAECh. 3 - A 1.013 g sample of ZnSO4H2O is dissolved in water...Ch. 3 - The iodide ion in a 1.552 g sample of the compound...Ch. 3 - Prob. 105IAECh. 3 - The insecticide dieldrin contains carbon, oxygen,...Ch. 3 - Prob. 107IAECh. 3 - The atomic mass of Bi is to be determined by...Ch. 3 - A piece of gold (Au) foil measuring 0.25mm15mm is...Ch. 3 - Prob. 110IAECh. 3 - Prob. 111IAECh. 3 - All-purpose fertilizers contain the essential...Ch. 3 - A hydrate of copper(II) sulfate, when heated, goes...Ch. 3 - Prob. 114FPCh. 3 - Prob. 115SAECh. 3 - Prob. 116SAECh. 3 - Prob. 117SAECh. 3 - Prob. 118SAECh. 3 - Prob. 119SAECh. 3 - Three of the following formulas might be ether an...Ch. 3 - Prob. 121SAECh. 3 - Prob. 122SAECh. 3 - Iron is present red blood and acts to carry oxygen...Ch. 3 - Prob. 124SAECh. 3 - Prob. 125SAECh. 3 - Prob. 126SAECh. 3 - Prob. 127SAECh. 3 - Prob. 128SAECh. 3 - Prob. 129SAECh. 3 - Which compound has a molar mass of...Ch. 3 - Prob. 131SAECh. 3 - Prob. 132SAECh. 3 - A hydrate of Na2SO2 contains almost exactly 50%...Ch. 3 - Malachite is a common copper-containing mineral...Ch. 3 - Prob. 135SAECh. 3 - Ibuprofen is a compound used in painkiller. When a...Ch. 3 - Prob. 137SAE
Knowledge Booster
Similar questions
- What is the molecular (formula) mass (in AMU) of C 4H 80 2? Key Concept: The molecular mass is obtained by summing the total mass of each element in the compound. E.g. the molecular mass of Ni(NO 3) 2 is MW = 1*58.69 + 2*(1*14.01 + 3*16.0) = 182 amu.arrow_forwardIn 1961, scientists agreed that the atomic mass unit (amu) would be defined as 1/ 12 the mass of an atom of 12C. Before then, it was defined as 1 /16 the average mass of an atom of naturally occurring oxygen (a mixture of 16O, 17O, and 18O). The current atomic mass of oxygen is 15.9994 amu. (a) Did Avogadro’s number change after the definition of an amu changed and, if so, in what direction? (b) Did the definition of the mole change? (c) Did the mass of a mole of a substance change? (d) Before 1961, was Avogadro’s number 6.02x1023 (to three significant figures), as it is today?arrow_forwardInstructions: Make sure to make your explanations precise and show your complete solutions. Analyze situational problem/s involving chemical reactions and apply the Law of Mass Conservation. Jan Baptista van Helmont (1579–1644) recorded the mass of a young willow tree and the soil in which the tree was planted. Five years later he found that the mass of soil had decreased by only 0.057 kg, while that of the tree had increased by 75 kg. During that period, he had added only water to the bucket in which the tree was planted. Helmont concluded that essentially all the mass gained by the tree had come from the water. Was this a valid conclusion? Explain. ______________________________________________________________________________________________ ______________________________________________________________________________________________ ______________________________________________________________________________________________arrow_forward
- 1. The sugar glucose contains C, H, and O and has a mass of 180.0634 amu as determined by high-resolution mass spectrometry. Glucose contains an equal number of carbon and oxygen atoms. What is the molecular formula of glucose? (1H = 1.00783 amu, 12C = 12.00000 amu, 160 = 15.99491 amu). Provide a thorough explanation.arrow_forwardA compound Y containing carbon, hydrogen and oxygen only have the following composition by mass:C: 40.0% ; H: 6.7% ; O: 53.3%(a) Calculate the empirical formula of the compound. (Relative atomic masses: H =1.0, C = 12.0, O = 16.0) (b) Given that the relative molecular mass of compound Y is 180. Find its molecular formula.arrow_forwardGiven the table of atomic weights listed below, determine the molecular mass (weight) of the sulphuric acid molecule H2S04. Enter your answer without units as a whole number i.e. rounded to zero decimal places. Atomic Weight (g/mol) Element Symbol Hydrogen 1.01 Carbon 12.01 Nitrogen 14.01 Охудеп 16.00 Phosphorous P 30.97 Sulphur 32.06 Chlorine CI 35.45 Potassium K 39.10arrow_forward
- The molar masses of the four natural isotopes of chromium are 50 g mol-1, 52 g mol -1 53 g mol -1 and 54 g mol -1. The mass fractions of these isotopes in the element are 0.0431; 0.8376; Find the molar mass of chromium since it is determined as 0.0955 and 0.0238.arrow_forwardCalculate the number of atoms of silicon (Si) in 415 cm3of the colorless gas disilane at 0°C and atmospheric pressure, where its density is 0.00278 g cm-3 . The molecular formula of disilane is Si2H6.arrow_forwardA hypothetical element exists as two isotopes: I = 85.50 amu and II = 88.70 amu. If the percent abundance of isotope I is (2.16x10^1)%, what would be the calculated atomic mass (in amu)? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:arrow_forward
- The technique of mass spectrometry cannot... be used in conjunction with an HPLC. be used in the analysis of very large molecules like proteins. differentiate enantiomers differentiate the different isotopes of the elements in a sample. O be used for elemental analysis of a sample.arrow_forwardThere are two isotopes of an unknown element, X-19 and X-21. The abundance of X-19 is 14.63%. Now that you have the contribution from the X-19 isotope (2.780) and from the X-21 isotope (17.93), what is the average atomic mass (in amu) of this element using four significant figures? ►arrow_forwardGiven the following average atomic masses (in atomic mass unit, u),Hydrogen: 1.008 u, Oxygen: 15.999 u, and sulfur: 32.06 u.What percentage of sulfuric acid’s (H2SO4) mass is oxygen? Express your answer to 2 decimal places.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning