Moles practice Q’s Ch 10 Pearson.

Slides:

Advertisements

Similar presentations

Moles, volume and density

Advertisements

Chapter 10: Chemical Quantities

Quantities in Chemistry The Relationship Between Mole and Molar Mass.

Molar & atomic Mass Mole  > particles Mass  > Mole Molar Volume of Gas Gas Density

 What is the percent composition of N and O in NO 2 ?

The Mole Chapter 9 What is a mole? A mole of a substance is the amount of that substance which contains 6 x particles of that substance.

Chemical Quantities.  Calculate the mass of compounds.  Calculate the molar volumes of gases.  Solve problems requiring conversions between mass, and.

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

The Mole: A measurement of Matter

Using Moles to Count Atoms

The MOLE CH 11.

Do you know your mole equalities? Answer: True or False.

Chapter 7: Chemical Formulas and Chemical Compounds

Unit 2: Chemical Quantities SCH 4C. The Chemist’s Dozen  How many in a couple?  How many in a few?  How many in a dozen?  How many in a ream? 2 3.

The Mole and Avogadro’s Number

Moles. Definition A mole is the mass of a substance which contains the same number of particles as 12 grams of the isotope carbon 12. These particles.

The Mole Chapter 7 Chemical Quantities Determine the percent composition of Fe(OH) 2 Fe – 1 x 55.8 = 55.8 O – 2 x 16 = 32 H – 2 x 1 = 2 Molar mass =

THE MOLE Chapter 10: Chemical Quantities Measuring Matter What is a mole? It is the SI unit that measures the amount of substance.

Quantities in Chemistry The Mole and Molar Mass. Mole Review A Mole is a unit of measurement in chemistry. It represents 6.02 x of an entity. One.

7.2 More Mole Conversions!!!. - Molecular Oxygen = O 2 - Atomic Oxygen = O from the periodic table 7 elements that exist as diatomic molecules (MEMORIZE)

10.1 THE MOLE Q4TP – CHEM MATT T.. THE MOLE: A MEASUREMENT OF MATTER What are three methods for measuring the amount of something? How is Avogadro’s number.

Unit 5 Review The Mole. 1. What is the mass of 1 mole of iron atoms? A amu B L C x D g.

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,

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.

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

Chemical quantities Chapter Ways to measure matter Length/width/height Volume Density Surface Area Etc.

Unit 6 Review The Mole.

The Mole. What is the a mole? A unit to measure the amount of a substance. Commonly abbreviated mol. The symbol is n.

UNIT 6: CHEMICAL QUANTITIES Chapter 10: Mole and Volume Relationships.

Chemical Quantities Chapter 10. The Mole: A Measurement of Matter We can measure mass (g), volume (L), count atoms or molecules in MOLES Pair: 1 pair.

Chapter 7 Lesson 2 Chemical Quantities. Mass-Mole Calculations What is the mass of 1.33 moles of titanium, Ti? What is the mass of 1.33 moles of titanium,

Mole Measures Problems Random Vocab. $100 $200 $300 $400 $500 $400 $500.

Molar Mass (M) Topic 1.2.

Chapter 10 Chemical Quantities

Glencoe: Chapter 11 Sections 11.1 & 11.2

The Mole and Avogadro’s Number

Molar Mass and Molar Volume

Defining the Mole & Mole Practice Problems

10.5 NOTES Avogadro Molar Volumes

Chapter 10 Review “Chemical Quantities”

Ch. 10 Chemical Quantities

Chapter 10 Chemical Quantities

Chemistry I Mole Review.

Chapter 10 Review “Chemical Quantities”

The Mole Unit 3.

Density of a Gas at STP Lesson # 4.

mass of one mole of particles

Moles Foothill Chemistry.

3.3 The Molar Volume Pages

Molar Conversions.

Molar Conversions (p.80-85, )

Avogadro’s Number: 1 mole = 6.02 x 1023 particles

mass of one mole of particles

Chapter 19 Avogadro’s Principle.

Measure amounts of something with three different methods—

Chapter 10 Chemical Quantities

Moles and Gas Volume (3.4) Avogadro’s Hypothesis: equal volumes of different gases at the same temperature and pressure contain the same number of particles.

Molar Conversions.

Moles, Volume and Density

The Mole Concept.

The Mole Mole: convenient measure of chemical quantities.

Unit 8 Stoichiometry.

Chapter 11 The Mole.

C2H6 CH3 B. Empirical Formula

Presentation transcript:

Moles practice Q’s Ch 10 Pearson

What is the mass of 2.50 moles of FeS? 220. g 35.2 g .0284 g

How many moles of Fe is 3.3 × 1015 atoms of Fe? 1.8 x 1015 mol 9.2 x 107 mol 5.5 x 10-9 mol

True or False Representative particles can be atoms, molecules, or ions present in a substance.

How many atoms in 2 moles of hydrogen? 6.022 x 1023 atoms 1.204 x 1024 atoms 3.011 x 1023 atoms

What is the density of CO2, a gas, at STP? 985.8 g/L 44.01 g/L 1.965 g/L

True or False The mole is the SI unit that measures the amount of a substance.

How many moles are in 6.00 grams of F2? 2.28 x 1025 mol

What is the molar mass of methane, CH4? 16.06 g/mol Not enough information 6.022 x 1023

Please make your selection What is Avogadro’s number? 6.022 x 1023 atoms 12.01 atoms 3.011 x 1023 atoms 22.4 L

True or False The molar mass of a substance is found by adding together the masses of each element in the substance from the Periodic Table.

What is the volume of 32.0 grams of O2 at STP?