Moles and Molar Mass Objective: I will be able to convert moles of a substance to mass and mass to moles. Entry Task: The LD50 for arsenic (III) oxide,

Slides:

Advertisements

Similar presentations

Chapter 10: Chemical Quantities

Advertisements

Unit 4: TOXINS Stoichiometry, Solution Chemistry, and Acids and Bases

7.3 USING CHEMICAL FORMULAS APRIL 27, USING CHEMICAL FORMULAS Formula Masses: Sum of all the average atomic masses of all atoms represented.

Mole  measurement of the number of particles in a sample  1 mol He (g) = 6.02 x atoms  1 mol CO 2(g) = 6.02 x molecules.

Chemical Formulas and Compounds Using Chemical Formulas.

Formula Mass and Composition of Compounds

Chapter 7: Chemical Formulas and Chemical Compounds

Unit 6: Chemical Quantities

Chemical Quantities The Mole: A Measurement of Matter

Chem Catalyst - What is the atomic mass of: - Cl? - Fe? - KCl? - H 2 O?

Chemical Quantities Avogadro’s Number.

Mass Relationships The Mole and Stoichiometry. The Mole A mole is the number of atoms in exactly 12 grams of 12 C (carbon-12 isotope)A mole is the number.

Conversion Factor Analysis practice Write down and answer these questions: 1)Molar Mass of C 6 H 12 O 6 = ____________ 2)How many C atoms in 1.74 mol of.

Molar Mass of ionic compounds. Molar Mass Molar mass- same as atomic mass but for a compound rather than an atom. To determine the molar mass of any compound.

Moles of Compounds. A properly written compound shows the ratio of atoms in the compound. For example, sodium carbonate (Na 2 CO 3 ) shows that for every.

The chemical formula for water is H 2 O. How many atoms of hydrogen and oxygen are there in one water molecule? H2OH2O 2 hydrogen atoms 1 oxygen atom.

Once you know the number of particles in a mole (Avogadro’s number = 6.02 x ) and you can find the molar mass of a substance using the periodic table,

Molar Mass, Moles, and Molecules 7.3 Using Chemical Formulas.

6.5 Mass & Number of Entities pp Avogadro's constant (N A ) is the link between the mass of a substance and the number of entities present.

Molar Conversions. Moles The standard unit of measure for the amount of a substance in numbers.

The Mole Calculating -Molecular Weight -Formula Weight -Molar Mass.

MOLAR MASS Molar mass of a substance = mass in grams of one mole of the substance. A compound’s molar mass is NUMERICALLY equal to its formula mass. Formula.

Avogadro’s Number and Molar Conversions Mole: the SI base unit used to measure the amount of a substance whose number of particles is the same as the number.

THE MOLE Measuring Matter. What is a mole? In Chemistry, a mole is the unit used to measure the amount of a substance represented by the coefficient in.

Using Chemical Formulas

MOLAR MASS CHAPTER 7-2.

Conversion factors from chemical formula

Bell Ringer How many moles of Nitric acid are there in 250 g?

Chapter 7 “Chemical Formulas and Chemical Compounds”

5.3 – Molar Mass Ms. Munir.

Molar Mass (M) Topic 1.2.

The Mole: A Measurement of Matter

Molar Mass and Molar Volume

Unit 4: Formula Stoichiometry

Using Chemical Formulas

Ch 7.3 Using Chemical Formulas

Living By Chemistry SECOND EDITION

How many ions are in a mole of chloride, Cl- ?

Empirical and Molecular Formulas

Empirical Formula Molecular Formula

average mass of H2O molecule: amu

Simplest Chemical formula for a compound

Section 3.1 The Mole and Molar Mass

Empirical and Molecular Formulas

Percent Composition and Chemical Formulas

BELL WORK - CHEMISTRY 525 molecules of CO2 = _______ moles of CO2

From percentage to formula

Living By Chemistry SECOND EDITION

Living By Chemistry SECOND EDITION

Unit 6 Mole Calculations

Molar Conversions.

Empirical and Molecular Formulas

Empirical Formulas and Mole Ratios

Empirical and Molecular Formulas

Bellwork Wednesday Dig around in your brain and fill in the following…

mole (symbolized mol) = 6.02 x particles

Empirical and Molecular Formulas

Molar Conversions.

Show Down 2 Step Mole Conversions

Ch. 7: Chemical Formulas and Compounds

From percentage to formula

The Mole Mole: convenient measure of chemical quantities.

Empirical Formula of a Compound

Unit 8 Stoichiometry.

Ch. 7: Chemical Formulas and Compounds

The Mole Chapter 7-1.

Chemical Composition.

Chapter 7- Sec. 3 and 4 “Chemical Formulas and Chemical Compounds”

QOTD What is atomic mass? How is atomic mass determined?

Chemical Reactions & Reaction Stoichiometry

Presentation transcript:

Moles and Molar Mass Objective: I will be able to convert moles of a substance to mass and mass to moles. Entry Task: The LD50 for arsenic (III) oxide, As2O3, is 15 mg/kg. Figure out the lethal dose for a 150 lb adult (1 kg = 2.2 lb) How many molecules do you think are in a lethal dose? What would you need to know to figure this out?

Mass of an atom, mass of a mole of atoms Atomic mass of 1 atom (from periodic table): Mass of C = 12.011 amu Mass of As = 74.922 amu Mass of O = 16 amu Actual mass of 1 mole: Mass of 1 mol C atoms = 12.011 g Mass of 1 mol As atoms = 74.922 g Mass of 1 mol O atoms = 16 g

Mass of molecules Atomic Mass of Molecules (add mass of all atoms): Mass of CO2 = 12.011 + 16 + 16 = 44.011 amu Mass of As2O3 = 74.922+74.922+16+16+16 = 198.844 amu 1 mol of CO2 = 1 mole of C atoms and 2 moles of O atoms 1 mol of As2O3 = 2 moles of As atoms and 3 moles of O atoms Actual mass of 1 mole: Mass of 1 mol CO2 = 12.011 + 16 + 16 = 44.011 g Mass of 1 mol As2O3 = 74.922+74.922+16+16+16 = 198.844 g

What is the mass of 1 molecule of... PbCl2 = H2O = C12H22O11 = CaCO3 = 207.2+35.453+35.453 = 278.106 amu 1.01+1.01+16 = 18.02 amu 12(12.011) + 22(1.01) + 11(16) = 342.352 amu 40.078+12.011+16+16+16= 100.089 amu

What is the mass of 1 MOLE of... PbCl2 = H2O = C12H22O11 = CaCO3 = 207.2+35.453+35.453 = 278.106 g 1.01+1.01+16 = 18.02 g 12(12.011) + 22(1.01) + 11(16) = 342.352 g 40.078+12.011+16+16+16= 100.089 g Mass of 1 mole of a substance is known as the MOLAR MASS

What are the Molar Masses of: Name of drug Chemical formula Molar Mass Adult dose Moles in adult dose? acetomen-iphen C8H9NO2 500 mg aspirin C9H8O4 325 mg ibuprofen C13H18O2 400 mg 151.2 g 0.0033 mol 180.2 g 0.0018 mol 206.3 g 0.0019 mol

Moles-Mass conversions Mass to moles: # of moles (mol) = mass(g) / molar mass(g/mol) Moles to mass: mass(g) = # of moles(mol) x molar mass(g/mol) I have an 11g sample of Cl2. How many moles do I have? I have 3.0 moles of MgO. What mass does the sample have? 11g / 70.906(g/mol) = 0.16 mol 3 mol x 40.305(g/mol) = 120.915 g

Exit Ticket Methadone is a medication used as a painkiller and as a treatment for those recovering from heroin addiction. The LD50 for methadone is 95 mg/kg. Would you consider methadone to be more or less toxic than acetomenaphen (LD50 = 2404 mg/kg)? Than aspirin (LD50 = 200 mg/kg)? Explain how you would calculate the amount of methadone that would be lethal to a human.