Key: Compound Calculations and Compound Stoichiometry.

Slides:

Advertisements

Similar presentations

Mole Problems Solution Guide.

Advertisements

Chapter 10 Chemical Quantities

Stoichiometry Chapter 12.

Section Percent Composition and Chemical Formulas

1 Chapter 6 Chemical Quantities. 2 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count pieces.

1 Chapter 8 Chemical Quantities. 2 How you measure how much? How you measure how much? n You can measure mass, n or volume, n or you can count pieces.

Molar Mass and Mole Calculation Problems

» What are ions formed from a single atom called? » Monatomic ions.

HELP CENTER SCHEDULE STUDY GROUP SURVEY- CHECK YOUR ! LAB POTASSIUM HYDROXIDE SUB’D FOR SODIUM HYDROXIDE IN OLD VERSION OF PRE-LAB YOU DON’T NEED.

Chapter 7 – The Mole and Chemical Composition

MOLE (mol)‏ Mass (g)‏ Particles (atoms,m’c or f.u.) DO NOW: Copy the conversion factors that allow you to convert from mass to moles and from particles.

7.3. Formula Mass – for any molecule, formula unit, or ion, it is the ____ of the ________ masses of all atoms represented in its formula. H 2 O for example.

Molecular Weight and Atomic Weight Na Cl Molecular Weight or Molar Mass =

 Molar mass is the mass in grams of one mole of particles (atoms, ions, molecules, formula units).  Equal to the numerical value of the average atomic.

Chemical Quantities.  Calculate the mass of compounds.  Calculate the volume of a given mass of a gas from its density at a given temperature and pressure.

Percent Composition, Empirical Formulas, Molecular Formulas.

Molar Mass & Conversions. The Mole mole (mol)- SI Unit for the amount of a substance that contains as many particles as there are atoms in exactly 12g.

Q3U2 :Theoretical Yield, Mass Percents, and Empirical Formulas.

Quantities in Chemical Reactions Review Definitions $100 $200 $300 $400 $500 Quantities Balanced Chemical Equations Additional Calculations Team 1Team.

MOLE (mol)‏ Particles (atoms or molecules)‏ DO NOW: Which conversion factor allows you to convert from moles to particles? 1 mol x particles.

Lesson 25 Percent Composition

Chapter 6 Chemical Quantities. How you measure how much?  You can measure mass, or volume, or you can count pieces.  We measure mass in grams.  We.

7.3 Using Chemical Formulas  Review  Mole: SI unit for the amount of a substance (contains avogadro’s number of particles)  Avogadro’s Number:

Chemical Formulas and Molar Masses A few old ideas revisited and a few new.

Chemical Formulas and Molar Masses A few old ideas revisited and a few new.

1 Chapter 12 Chemical Quantities. 2 How do you measure things? How do you measure things? n We measure mass in grams. n We measure volume in liters. n.

Chapter 6 Chemical Quantities How you measure how much? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure.

Chapter 10: Chemical Quantities

The Mole and Chemical Composition

The Mole and Chemical Composition

 What is the molar mass of water?  What % of the mass comes from hydrogen?  What % of the mass comes from oxygen?

Stoichiometry Balancing Equations Molecular and Empirical Formulas Percent Composition Mole Conversions

CHEMICAL COMPOUNDS AND THE MOLE Chapter 7. Formula Mass  Mass of H 2 O? H 2(1.01) + O 16.00_ amu  Formula Mass: mass of molecule, formula unit,

Chemical Formulas and Moles. Example: 1.water (C) – every molecule of water contains 2 atoms of hydrogen & one atom of oxygen - 2 molecules of H 2 O would.

Molar Mass = mass in grams of one mole –Units grams/mole For elements, molar mass = atomic mass Why aren’t all atomic masses whole numbers? –Remember that.

 Dalton used the percentages of elements in compounds and the chemical formulas to deduce the relative masses of atoms  Unit is the amu(atomic mass.

Using the Mole. The Mole 1 mole = 6.02 X Particles Particle = atoms, compounds, or molecules Molar ratio: Tells us the number of moles of each chemical.

Using Molar Mass as a Conversion Factor.  A molar mass is the mass in grams of one mole of a substance.  One mole of any substance contains Avogadro’s.

Oh My!!.  Mole (mol) can be defined as the number equal to the number of carbon atoms in grams of carbon (in an chemical equation it is the coefficients.

Chemical Calculations Stoichiometry OBJECTIVES: – Calculate stoichiometric quantities from balanced chemical equations using units of moles and mass.

Stoichiometry u Greek for “measuring elements” u The calculations of quantities in chemical reactions based on a balanced equation. u We can interpret.

Molar Mass & Percent Composition. The mass of 1 mole of an element or compound – The mass in grams from the Periodic Table Unit = grams per mole (g/mol)

Chemical Quantities.  Calculate the mass of compounds.  Calculate the volume of a given mass of a gas from its density at a given temperature and pressure.

1 7 Chemical Formulas and Composition Stoichiometry.

Chapter 11: The Mole Table of Contents 11.1: Measuring Matter 11.2: Mass and the Mole 11.3: Moles of Compounds.

Chemical Calculations Stoichiometry u OBJECTIVES: Calculate stoichiometric quantities from balanced chemical equations using units of moles, mass, representative.

Stoichiometry The mathematics of Chemistry. What is Stoichiometry? The proportional relationship between two or more substances during a chemical reaction.

Mole (symbolized mol) = 6.02 x particles (602,000,000,000,000,000,000,000) Avogadro’s Number (N A ) molar mass – mass (usually in grams) of one mole.

CHEMICAL COMPOUNDS AND THE MOLE Chapter 7. Formula Mass  Mass of H 2 O?  Formula Mass: mass of molecule, formula unit, or ion is sum of masses of all.

IIIIII Formula Calculations The Mole. A. Percentage Composition n the percentage by mass of each element in a compound.

Chemical Calculations Mole to Mass, Mass to Moles.

Stoichiometry – Chemical Quantities Notes. Stoichiometry Stoichiometry – Study of quantitative relationships that can be derived from chemical formulas.

Review Self-Quiz for Stoichiometry 1.Write the formula for a compound made from sodium and chlorine. 2.Write a chemical reaction for the following: Na.

Chapter 7 “Chemical Formulas and Chemical Compounds” Yes, you will need a calculator for this chapter!

Got Mole Problems?.

 Predict the products and write a balanced equation for the following: BaCl 2 + MgSO 4 

Formula (Molar) Mass Li Mn K. Formula (Molar) Mass Add atomic mass of each atom in formula Unit: g/mol Mass of one mole of a pure substance.

MOLE (mol)‏ Mass (g)‏ Particles (atoms,m’c or f.u.) Which conversion factors that allow you to convert from mass to moles and from particles to moles.

Mass Measurements In Chemistry Calculating Formula Weight of Hydrates.

Percent Composition KMnO 4. Percent Composition (NH 4 ) 3 PO 4.

Entry Task: March 11 th Monday Entry task question: 2AgCl + Mg  MgCl 2 + 2Ag Question: How many grams of silver can be produced if grams of magnesium.

III. Formula Calculations

Simplest Chemical formula for a compound

Chemical Reactions Unit

Stoichiometric Calculations

Molar Conversions.

mole (symbolized mol) = 6.02 x particles

Stoichiometry Greek for “measuring elements”

Molar Conversions.

Presentation transcript:

Key: Compound Calculations and Compound Stoichiometry

KNO 3 K --> 1 x = N --> 1 x = O --> 3 x = amu MgCl 2 Mg --> 1 x = Cl --> 2 x = amu

Na 2 SO 3 Na --> 2 x = S --> 1 x = O --> 3 x = amu (NH 4 ) 3 PO 4 N --> 3 x = H --> 12 x 1.01 = P --> 1 x = O --> 4 x = amu

CH 3 OH C --> 1 x = H --> 4 x 1.01 = 4.04 O --> 1 x = amu NaClO Na --> 1 x = (22.99/74.44)100 = 30.9 Cl --> 1 x = (35.45/74.44)100 = 47.6 O --> 1 x = (16.00/74.44)100 = grams

Copper II sulfate CuSO 4 Cu --> 1 x = (63.55/159.61)100 = 39.8 S --> 1 x = (32.06/159.61)100 = 20.1 O --> 4 x = (64.00/159.61)100 = grams Aluminum oxide Al 2 O 3 Al --> 2 x = (53.96/101.96)100 = 52.9 O --> 3 x = (48.00/101.96)100 = grams

SiO 2 Si --> 1 x = (28.09/60.09)100 = 46.7 O --> 2 x = (32.00/60.09)100 = grams Ammonium sulfate (NH 4 ) 2 SO 4 N --> 2 x = (28.02/132.16)100 = 21.2 H --> 8 x 1.01 = 8.08 (8.08/132.16)100 = 6.1 S --> 1 x = (32.06/132.16)100 = 24.3 O --> 4 x = (64.00/132.16)100 = grams

Ammonium phosphate (NH 4 ) 3 PO 4 N --> 3 x = (42.03/149.12)100 = 28.2 H --> 12 x 1.01 = (12.12/149.12)100 = 8.1 P --> 1 x = (30.97/149.12)100 = 20.8 O --> 4 x = (64.00/149.12)100 = grams

Element%=gramsMoles (divide by molar mass) Smallest Ratio (divide by smallest mole) Compound’s Chemical Formula Fe /55.85 = /1.137 = 1 FeS S /32.06 = /1.137 = 1 K /39.10 = /.815 = 1 KClO 3 Cl /35.45 = /.815 = 1 O /16.00 = /.815 = 3 F /19.00 = /3.40 = 4 F 4 C C /12.01 = /3.40 = 1

Element % = gramsMoles (divide by molar mass) Smallest ratio (divide by smallest moles) Compound’s Chemical Formula Cd / = /.686 = 1 CdS S /32.06 = /.686 = 1 Al32 32/26.98 = /1.2 = 1 AlF 3 F68 68/19.00 = /1.2 = 3 Ca /40.08 = /.8323 = 1 CaSO 3 S /32.06 = /.8323 = 1 O /16.00 = /.8323 = 3 Ag87 87/ =.81.81/.41 = 2 Ag 2 S S13 13/32.06 =.41.41/.41 = 1

18. n = 52.08/13.02 = 4 4(CH) = C 4 H n = 60.06/30.03 = 2 2(CH 2 O) = C 2 H 4 O n = / = 2 2(PO 2 ) = P 2 O n = /77.47 = 3 3(OCNCl) = O 3 C 3 N 3 Cl B 78.3/10.81 = /7.24 = 1 H 21.7/1.01 = /7.24 = 3 BH 3 n = 27.67/13.84 = 2 2(BH 3 ) = B 2 H 6

2) 2.5 moles O 2 = ? molecules 2.5 moles O 2 x (6.02x10^23) molecules = 1.5x10^24 molecules 1 1 mole 4) moles C 13 H 18 O 2 = ? molecules moles C 13 H 18 O 2 x (6.02x10^23) molecules = 1.4x10^21 molecules 1 1 mole 4) 500 mg  0.5 g C 13 H 18 O 2 = ? molecules 0.5 g C 13 H 18 O 2 x (6.02x10^23) molecules = 1.4x10^21 molecules g

6) 47.5 g C 3 H 8 O 3 = ? molecules 47.5 g C 3 H 8 O 3 x (6.02x10^23) molecules = 3.10x10^23 molecules g 8) x10^13 particles = ? moles x10^13 particles x _____1 mole____ = x10^-10 mole 1 (6.02x10^23 particles) 10) 3.12 mol MgCl 2 = ? grams 3.12 mol MgCl 2 x grams = 297 grams 1 1 mole