Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Textbook Question
Chapter 2, Problem 122GQ

Capsaicin, the compound that gives the hot taste to chili peppers, has the formula C18H27NO3.

(a) Calculate its molar mass.

(b) If you eat 55 mg of capsaicin, what amount (moles) have you consumed?

(c) Calculate the mass percent of each element in the compound.

(d) What mass of carbon (in milligrams) is there in 55 mg of capsaicin?

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The molar mass for given compound capsaicin should be determined using given formula.

Concept introduction:

  • Mass=Density×Volume
  • Moleofsubstance=GramofsubstanceMolarmass
  • The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
  • Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

Answer to Problem 122GQ

Molar mass of Capsaicin is 305.18g/mol

Explanation of Solution

Molecular formula of the given compound Capsaicin is C18H27NO3

Molar mass of Capsaicin can be calculated as follows,

(18×12.01massofC)+(27×1massofH)+(14massofN)+(16massofO)=305.18g/mol

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The amount of moles present in given amount of compound capsaicin should be determined.

Concept introduction:

  • Mass=Density×Volume
  • Moleofsubstance=GramofsubstanceMolarmass
  • The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
  • Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

Answer to Problem 122GQ

Amount of Capsaicin in 55 mg = 0.0001802mol

Explanation of Solution

Here 55 mg of capsaicin used. Then the amount of capsaicin can be calculated as follows,

Moleofsubstance=GramofsubstanceMolarmassMoleofCapsaicin=0.055g305.18g/mol=0.0001802mol

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass percent of each elements present in given compound capsaicin should be determined.

Concept introduction:

  • Mass=Density×Volume
  • Moleofsubstance=GramofsubstanceMolarmass
  • The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
  • Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

Answer to Problem 122GQ

  ElementsinCapsaicinMasspercentC70.83%H8.84%N4.58%O15.78%

Explanation of Solution

Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

The molecular formula of the given compound is C18H27NO3

And this compound contains 18C,27H,1Nand3Oatoms

Molar mass of Carbon in the given compound is calculated as =18×12.01=216.18g/mol

Mass percent of Carbon in C18H27NO3 is as follows,

C in C18H27NO3=MolarmassofcarbonMolarmassofCapsacin×100 =216.18305.18×100 =70.83%

Similarly,

Molar mass of Hydrogen in the given compound is calculated as =27×1=27g/mol.

Mass percent of Hydrogen in C18H27NO3 is as follows,

HinC18H27NO3=MolarmassofHydrogenMolarmassofCapsacin×100 =27305.18×100 =8.84%

Molar mass of Nitrogen in the given compound is calculated as =1×14=14g/mol.

Mass percent of Nitrogen in C18H27NO3 is as follows,

NinC18H27NO3=MolarmassofNirogenMolarmassofCapsacin×100 =14305.18×100 =4.58%

Molar mass of oxygen in the compound is calculated as =3×16=48g/mol

Mass percent of Oxygen in C18H27NO3 is as follows,

OinC18H27NO3=MolarmassofoxygenMolarmassofCapsacin×100 =48305.18×100 =15.78%

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The mass of Carbon present in given amount of capsaicin should be calculated in milligrams.

Concept introduction:

  • Mass=Density×Volume
  • Moleofsubstance=GramofsubstanceMolarmass
  • The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol)
  • Mass percentage is one way to represent the concentration of an element in a compound or a component in a mixture. Mass percent of elements of a compound is the ratio of mass of element to the mass of whole compound and multiplied with hundred.

Answer to Problem 122GQ

In 55 mg of Capsaicin 38.96mgofC will be present

Explanation of Solution

Mass percent of carbon in 55 mg of Capsaicin is 70.83%

Then,

The mass of carbon in 55 mg of Capsaicin is,

        70.83100×55mg=38.96mg

So, in 55 mg of Capsaicin 38.96mgofC will be present.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
Students have asked these similar questions
What is the molecular weight of sugar, C6H12O6 in atomic mass units? And If you had one mole of sugar molecules, how much would it weigh?
What is the mass, in grams, of Vitamin C (C6H8O6) that contains 1.076 grams of carbon?
What would be the mass, in grams, of an NO2 sample in which 100 billion (1.00 X 10 11) moleculesare present?

Chapter 2 Solutions

Chemistry & Chemical Reactivity

Ch. 2.7 - Hydrated nickel(II) chloride is a beautiful green,...Ch. 2.8 - Prob. 2.12CYUCh. 2.8 - Prob. 1.1ACPCh. 2.8 - Prob. 1.2ACPCh. 2.8 - Prob. 2.1ACPCh. 2.8 - Salvarsan was long thought to be a single...Ch. 2.8 - To determine the density of atmospheric nitrogen....Ch. 2.8 - The density of a mixture of gases may be...Ch. 2.8 - Atmospheric argon is a mixture of three stable...Ch. 2.8 - Given that the density of argon is 1.78 g/L under...Ch. 2 - Prob. 1PSCh. 2 - Define mass number. What is the difference between...Ch. 2 - An atom has a very small nucleus surrounded by an...Ch. 2 - A gold atom has a radius of 145 pm. If you could...Ch. 2 - Give the complete symbol(ZAX), including atomic...Ch. 2 - Give the complete symbol(ZAX), including atomic...Ch. 2 - Prob. 7PSCh. 2 - Atomic structure. (a) The synthetic radioactive...Ch. 2 - Prob. 9PSCh. 2 - In 1886 Eugene Goldstein observed positively...Ch. 2 - Marie Curie was born in Poland but studied and...Ch. 2 - Prob. 12PSCh. 2 - The mass of an 16 O atom is 15.995 u. What is its...Ch. 2 - What is the mass of one 16O atom, in grams? (The...Ch. 2 - Cobalt has three radioactive isotopes used in...Ch. 2 - Naturally occurring silver exists as two isotopes...Ch. 2 - Name and describe the composition of the three...Ch. 2 - Which of the following are isotopes of element X,...Ch. 2 - Thallium has two stable isotopes, 203TIand 205Tl....Ch. 2 - Strontium has four stable isotopes. Strontium-84...Ch. 2 - Verify that the atomic weight of lithium is 6.94,...Ch. 2 - Verify that the atomic weight of magnesium is...Ch. 2 - Gallium has two naturally occurring isotopes, 69Ga...Ch. 2 - Europium has two stable isotopes, 151Eu and 153Eu,...Ch. 2 - Titanium and thallium have symbols that are easily...Ch. 2 - In Groups 4A-6A, there are several elements whose...Ch. 2 - How many periods of the periodic table have 8...Ch. 2 - Prob. 28PSCh. 2 - Prob. 29PSCh. 2 - Prob. 30PSCh. 2 - Classify the following elements as metals,...Ch. 2 - Prob. 32PSCh. 2 - Prob. 33PSCh. 2 - Prob. 34PSCh. 2 - What is the charge on the common monatomic ions of...Ch. 2 - What is the charge on the common monatomic ions of...Ch. 2 - Prob. 37PSCh. 2 - Prob. 38PSCh. 2 - When a potassium atom becomes a monatomic ion, how...Ch. 2 - When oxygen and sulfur atoms become monatomic...Ch. 2 - Prob. 41PSCh. 2 - Prob. 42PSCh. 2 - Give the formula and the number of each ion that...Ch. 2 - Give the formula and the number of each ion that...Ch. 2 - Prob. 45PSCh. 2 - Prob. 46PSCh. 2 - Prob. 47PSCh. 2 - Prob. 48PSCh. 2 - Prob. 49PSCh. 2 - Prob. 50PSCh. 2 - Prob. 51PSCh. 2 - Prob. 52PSCh. 2 - Write the formulas for the four ionic compounds...Ch. 2 - Write the formulas for the four ionic compounds...Ch. 2 - Sodium ions, Na+, form ionic compounds with...Ch. 2 - Consider the two ionic compounds NaCl and CaO. In...Ch. 2 - Prob. 57PSCh. 2 - Name each of the following binary, nonionic...Ch. 2 - Prob. 59PSCh. 2 - Prob. 60PSCh. 2 - Calculate the mass, in grams, of each the...Ch. 2 - Calculate the mass, in grams, of each the...Ch. 2 - Calculate the amount (moles) represented by each...Ch. 2 - Calculate the amount (moles) represented by each...Ch. 2 - You are given 1.0-g samples of He, Fe, Li, Si, and...Ch. 2 - You are given 0.10-g samples of K, Mo, Cr, and Al....Ch. 2 - Analysis of a 10.0-g sample of apatite (a major...Ch. 2 - A semiconducting material is composed of 52 g of...Ch. 2 - Calculate the molar mass of each of the following...Ch. 2 - Calculate the molar mass of each of the following...Ch. 2 - Calculate the molar mass of each hydrated...Ch. 2 - Prob. 72PSCh. 2 - What mass is represented by 0.0255 mol of each of...Ch. 2 - Assume you have 0.123 mol of each of the following...Ch. 2 - Sulfur trioxide, SO3, is made industrially in...Ch. 2 - How many ammonium ions and how many sulfate ions...Ch. 2 - Acetaminophen, whose structure is drawn below, is...Ch. 2 - An Alka-Seltzer tablet contains 324 mg of aspirin...Ch. 2 - Calculate the mass percent of each element in the...Ch. 2 - Calculate the mass percent of each element in the...Ch. 2 - Calculate the mass percent of copper in CuS,...Ch. 2 - Calculate the mass percent of titanium in the...Ch. 2 - Succinic acid occurs in fungi and lichens. Its...Ch. 2 - An organic compound has the empirical formula...Ch. 2 - Prob. 85PSCh. 2 - Complete the following table:Ch. 2 - Acetylene is a colorless gas used as a fuel in...Ch. 2 - A large family of boron-hydrogen compounds has the...Ch. 2 - Cumene, a hydrocarbon, is a compound composed only...Ch. 2 - In 2006, a Russian team discovered an interesting...Ch. 2 - Mandelic acid is an organic acid composed of...Ch. 2 - Nicotine, a poisonous compound found in tobacco...Ch. 2 - A compound containing xenon and fluorine was...Ch. 2 - Elemental sulfur (1.256 g) is combined with...Ch. 2 - Epsom salt is used in tanning leather and in...Ch. 2 - You combine 1.25 g of germanium, Ge, with excess...Ch. 2 - The mass spectrum of nitrogen dioxide is...Ch. 2 - The mass spectrum of phosphoryl chloride. POF3, is...Ch. 2 - The mass spectrum of CH3Cl is illustrated here....Ch. 2 - Prob. 100PSCh. 2 - Fill in the blanks in the table (one column per...Ch. 2 - Potassium has three naturally occurring isotopes...Ch. 2 - Crossword Puzzle: In the 2 2 box shown here, each...Ch. 2 - The following chart shows a general decline in...Ch. 2 - Copper atoms. (a) What is the average mass of one...Ch. 2 - Prob. 106GQCh. 2 - Prob. 107GQCh. 2 - Identify two nonmetallic elements that have...Ch. 2 - Prob. 109GQCh. 2 - Prob. 110GQCh. 2 - Prob. 111GQCh. 2 - When a sample of phosphorus burns in air, the...Ch. 2 - Although carbon-12 is now used as the standard for...Ch. 2 - A reagent occasionally used in chemical synthesis...Ch. 2 - Prob. 115GQCh. 2 - Prob. 116GQCh. 2 - Which of the following compounds has the highest...Ch. 2 - Which of the following samples has the largest...Ch. 2 - The structure of one of the bases in DNA, adenine,...Ch. 2 - Prob. 120GQCh. 2 - A drop of water has a volume of about 0.050 mL....Ch. 2 - Capsaicin, the compound that gives the hot taste...Ch. 2 - Prob. 123GQCh. 2 - Write the molecular formula and calculate the...Ch. 2 - Malic acid, an organic acid found in apples,...Ch. 2 - Your doctor has diagnosed you as being anemicthat...Ch. 2 - A compound composed of iron and carbon monoxide,...Ch. 2 - Ma huang, an extract from the ephedra species of...Ch. 2 - Saccharin, a molecular model of which is shown...Ch. 2 - Prob. 130GQCh. 2 - Write the formula for each of the following pounds...Ch. 2 - Complete the table by placing symbols, formulas,...Ch. 2 - Empirical and molecular formulas. (a)...Ch. 2 - Cacodyl, a compound containing arsenic, was...Ch. 2 - The action of bacteria on meat and fish produces a...Ch. 2 - In the laboratory you combine 0.125 g of nickel...Ch. 2 - A compound called MMT was once used to boost the...Ch. 2 - Elemental phosphorus is made by heating calcium...Ch. 2 - Chromium is obtained by heating chromium(III)...Ch. 2 - Stibnite, Sb2S3, is a dark gray mineral from which...Ch. 2 - Direct reaction of iodine (I2) and chlorine (Cl2)...Ch. 2 - In a reaction, 2.04 g of vanadium combined with...Ch. 2 - Iron pyrite, often called fools gold, has the...Ch. 2 - Which of the following statements about 57.1 g of...Ch. 2 - The formula of barium molybdate is BaMoO4. Which...Ch. 2 - A metal M forms a compound with the formula MCl4....Ch. 2 - Pepto-Bismol, which can help provide relief for an...Ch. 2 - The weight percent of oxygen in an oxide that has...Ch. 2 - The mass of 2.50 mol of a compound with the...Ch. 2 - The elements A and Z combine to produce two...Ch. 2 - Polystyrene can be prepared by heating styrene...Ch. 2 - A sample of hemoglobin is found to be 0.335% iron....Ch. 2 - Consider an atom of 64Zn. (a) Calculate the...Ch. 2 - Estimating the radius of a lead atom. (a) You are...Ch. 2 - A piece of nickel foil, 0.550 mm thick and 1.25 cm...Ch. 2 - Uranium is used as a fuel, primarily in the form...Ch. 2 - In an experiment, you need 0.125 mol of sodium...Ch. 2 - Mass spectrometric analysis showed that there are...Ch. 2 - If Epsom salt, MgSO4 x H2O, is heated to 250 C,...Ch. 2 - The alum used in cooking is potassium aluminum...Ch. 2 - Tin metal (Sn) and purple iodine (I2) combine to...Ch. 2 - When analyzed, an unknown compound gave these...Ch. 2 - Two general chemistry students working together in...Ch. 2 - To find the empirical formula of tin oxide, you...Ch. 2 - Prob. 165SCQCh. 2 - Prob. 166SCQCh. 2 - The photo here depicts what happens when a coil of...Ch. 2 - A jar contains some number of jelly beans. To find...
Knowledge Booster
Chemistry
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
    • SEE MORE QUESTIONS
    Recommended textbooks for you
  • Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher: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
  • Chemistry: Principles and Practice
    Chemistry
    ISBN:9780534420123
    Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
    Publisher:Cengage Learning
    Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
  • Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher: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
    Chemistry: Principles and Practice
    Chemistry
    ISBN:9780534420123
    Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
    Publisher:Cengage Learning
    Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Bonding (Ionic, Covalent & Metallic) - GCSE Chemistry; Author: Science Shorts;https://www.youtube.com/watch?v=p9MA6Od-zBA;License: Standard YouTube License, CC-BY
    Stoichiometry - Chemistry for Massive Creatures: Crash Course Chemistry #6; Author: Crash Course;https://www.youtube.com/watch?v=UL1jmJaUkaQ;License: Standard YouTube License, CC-BY