Concept explainers
Calculate, to two decimal places, the formula mass of each of the following substances. Obtain the needed
- a. C12H22O11 (sucrose, table sugar)
- b. C7H16 (heptane, a component of gasoline)
- c. C7H5NO3S (saccharin, an artificial sweetener)
- d. (NH4)2SO4 (ammonium sulfate, a lawn fertilizer)
(a)
Interpretation:
Formula mass of
Concept Introduction:
Sum of atomic masses of all the atoms that are represented in chemical formula of substance is known as formula mass. If atomic mass and chemical formula of a compound is known, then formula mass can be calculated.
Answer to Problem 6.1EP
Formula mass of sucrose is
Explanation of Solution
Given chemical formula is
The formula mass of sucrose is calculated as
Formula mass of sucrose is calculated.
(b)
Interpretation:
Formula mass of
Concept Introduction:
Sum of atomic masses of all the atoms that are represented in chemical formula of substance is known as formula mass. If atomic mass and chemical formula of a compound is known, then formula mass can be calculated.
Answer to Problem 6.1EP
Formula mass of heptane is
Explanation of Solution
Given chemical formula is
The formula mass of heptane is calculated as
Formula mass of heptane is calculated.
(c)
Interpretation:
Formula mass of
Concept Introduction:
Sum of atomic masses of all the atoms that are represented in chemical formula of substance is known as formula mass. If atomic mass and chemical formula of a compound is known, then formula mass can be calculated.
Answer to Problem 6.1EP
Formula mass of saccharin is
Explanation of Solution
Given chemical formula is
The formula mass of saccharin is calculated as
Formula mass of saccharin is calculated.
(d)
Interpretation:
Formula mass of
Concept Introduction:
Sum of atomic masses of all the atoms that are represented in chemical formula of substance is known as formula mass. If atomic mass and chemical formula of a compound is known, then formula mass can be calculated.
Answer to Problem 6.1EP
Formula mass of ammonium sulfate is
Explanation of Solution
Given chemical formula is
The formula mass of ammonium sulfate is calculated as
Formula mass of ammonium sulfate is calculated.
Want to see more full solutions like this?
Chapter 6 Solutions
General, Organic, and Biological Chemistry
- A dark brown binary compound contains oxygen and ametal. It is 13.38% oxygen by mass. Heating it moderatelydrives off some of the oxygen and gives a red binary compoundthat is 9.334% oxygen by mass. Strong heatingdrives off more oxygen and gives still another binary compound,which is only 7.168% oxygen by mass. (a) Compute the mass of oxygen that is combined with1.000 g of the metal in each of these three oxides. (b) Assume that the empirical formula of the first compoundis MO2 (where M representsthe metal). Givethe empirical formulas of the second and thirdcompounds. (c) Name the metal.arrow_forwardCalculate the number of moles of carbon atoms present in eachof the following samples. l type="a"> 1.271 g of ethanol, C2H5OH i>3.982 g of 1 ,4-dichlorobenzene, C6H4Cl2 i>0.4438 g of carbon suboxide, C3O2 i>2.9 10 g of methylene chloride, CH2Cl2arrow_forwardCalculate the mass in grams of each of the following samples. l type="a"> 0.251 mole of ethyl alcohol, C2H6O i>1.26 moles of carbon dioxide 9.31104 moles of gold(III) chloride 7.74 moles of sodium nitrate 0.000357 mole of ironarrow_forward
- Calculate the number of molecules present in each of the following samples. l type="a"> 4.75 mmol of phosphine, PH3 i>4.75 g of phosphine, PH3 i>1.25102 g of lead(II) acetate, Pb( CH3 CO2)2 i>1.25 X 10 2 moles of lead(II) acetate, Pb( CH3 CO2)2 i>a sample of benzene, C6H6 , which contains a total of 5.40 moles of carbonarrow_forwardUsing the average atomic masses given inside the front cover of this book, calculate the mass in grams of each of the following samples. l type='a'> 2.17 moles ot germanium, Ge 4.24 mmcl of Iead(II) chloride (1 mmol = 1/1000 moI) 0.0971 mole of ammonia, NH3 :math>4.26103moles of hexane, C6H14 i>1.71 moles of iodine monochloride, ICIarrow_forwardOne chocolate chip used in making chocolate chip cookies has a mass of 0.324 g. (a) How many chocolate chips are there in one mole of chocolate chips? (b) If a cookie needs IS chocolate chips, how many cookies can one make with a billionth (1109) of a mole of chocolate chips? (A billionth of a mole is scientifically known as a nanomole.)arrow_forward
- hat is the difference between the empirical and molecular for mulas of a compound? Can they ever be the same? Explain.arrow_forwardUsing the average atomic masses given inside the front cover of this hook, calculate the mass in grains of each of the following samples. l type='a'> 0.341 mole of potassium nitride 2.62 mmol of neon (1 mmol = 1/1000 mol) 0.00449 mole of manganese(II) oxide 7.18105moles of silicon dioxide 0.00021 mole of iron(III) phosphatearrow_forwardCalculate the mass of carbon in grams, the percent carbon by mass, and the number of individual carbon atoms present in each of the following samples. l type="a"> 7.8 19 g of carbon suboxide, C3O2 i>1.531021 molecules of carbon monoxide 0.200 mole of phenol, C6H6Oarrow_forward
- Tetrodotoxin is a toxic chemical found in fugu pufferfish, a popular but rare delicacy in Japan. This compound has an LD50 (the amount of substance that is lethal to 50.% of a population sample) of 10.g per kg of body mass. Tetrodotoxin is 41.38% carbon by mass, 13.16% nitrogen by mass, and 5.37% hydrogen by mass, with the remaining amount consisting of oxygen. What is the empirical formula of tetrodotoxin? If three molecules of tetrodotoxin have a mass of 1.59 1021 g, what is the molecular formula of tetrodotoxin? What number of molecules of tetrodotoxin would be the LD50 dosage for a person weighing 165 lb?arrow_forwardCalculate the number of atoms of each element present in each of the following samples. l type='a'> 4.2 1 g of water 6.81 g of carbon dioxide 0.000221 g of benzene, C6H6 i>2.26 moles of C12H22O11arrow_forwardUsing the average atomic masses given inside the front cover of the text, calculate the mass in grams of each of the following samples. l type='a'> 5.0 moles of nitric acid 0.000305 mole of mercury 2.31105mole of potassium chromate 10.5 moles of’ aluminum chloride 4.9104moles of sulfur hexafluoride 1 25 moles of ammonia 0.01205 mole of sodium peroxidearrow_forward
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning