Two Relationships 1 mole = molar mass in grams of any element or compound (use periodic table) 1 mole = 6.022 x 1023 particles (molecules, atoms, formula.

Slides:

Advertisements

Similar presentations

Chapter 10 Worksheet Examples

Advertisements

Chapter 10: Chemical Quantities

1 Section 3.3 The Mole: A Measurement of Matter n OBJECTIVES: –Describe how Avogadro’s number is related to a mole of any substance.

Unit 5 Moles and Stoichiometry Lesson 2: The Molar Relationships.

The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance? 10.2.

Factor Label Practice

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 10: Chemical Quantities

The Mole: A measurement of Matter

Ch. 10: The Mole *Part of Sec. 13.2: Avogadro’s Principle (pages ) Sec. 10.3: Moles of Compounds (pages 333 – 334 & )

Avogadro’s Number Avogadro’s number (symbol N) is the number of atoms in grams of carbon. Its numerical value is 6.02 × Therefore, a

Unit 5: The Mole and Stoichiometry

MOLAR MASS What is molar mass? How do you calculate molar mass?

The Mole and Avogadro’s Number

AP Notes Chapter 7 Mole Representative Particles Molecular Mass (mm) - gam used for atoms - gmm used for molecules - gfm used for formula units MoleVolume.

Counting Atoms Chapter 9. MOLE?? Moles of Particles In one mole of a substance, there are 6 x particles.

THE MOLE. Atomic and molecular mass Masses of atoms, molecules, and formula units are given in amu (atomic mass units). Example: Sodium chloride: (22.99.

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

CH 9: The Mole Renee Y. Becker CHM 1025 Valencia Community College 1.

IIIIIIIV The Mole I. Molar Conversions A. What is the Mole? n A counting number (like a dozen) n Avogadro’s number n 1 mol = 6.02  items A large.

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

1 The Mole 6.02 X What is “The Mole??” A counting unit (similar to a dozen) 6.02 X (in scientific notation) = 602 billion trillion = 602,000,000,000,000,000,000,000.

Chapter 9 Vanessa N. Prasad-Permaul CHM 1025 Valencia College Chapter 9 1 © 2011 Pearson Education, Inc. The Mole Concept.

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

Unit 6 Review The Mole.

MOLE CALCULATIONS. Moles to Mass Find the mass of one mole of NaCl 58.5g Find the mass of two moles of NaCl 117.0g How did you get the answer? 2 moles.

The Mole.  Matter can be measured in 3 ways:  Counting particles  Mass  Volume.

Miss Fogg Spring 2016  A particle can refer to an individual atom OR a type of molecule ◦ Jellybean ◦ Baseball ◦ Carbon atoms ◦ Hydrogen atoms ◦ Water.

WHITEBOARD PRACTICE TEST REVIEW. How many molecules of ethane, C 2 H 6 are present in g C 2 H 6 ?

Chemical Quantities Chapter 10. The Mole  a mole is an amount of matter  mass is also an amount of matter, however the mole is much more useful to chemists,

The Mole Introduction to Chemistry. The Mole Atoms and molecules are too small to count out individually Avogadro’s Number = 6.02 x particles /

Moles to Grams Grams to Moles Liters to Moles Moles to Liters

Chapter 10 Chemical Quantities

The Mole and Avogadro’s Number

Chapter 10 Chemical Quantities

Stoichiometry & the Mole

Molar Mass and Molar Volume

MOLE AND STOIKIOMETRI We measure mass in grams. g

Chemical Quantities & Stoichiometry

Ch 7.3 Using Chemical Formulas

Identify the Representative Particle

Chapter 10 “Chemical Quantities”

Bellwork What is the gram molar mass of methane? Methane’s formula is CH4.

Unit 3: Moles!!!.

Chapter 10 – The Mole.

Chapter 10 Chemical Quantities

Unit: Chemical Quantities

The Mole Molar Conversions.

Chapter 9 “Chemical Quantities”

Mole-Mass and Mole-Volume Relationships

II. Molar Conversions.

Ch. 11: Molecular Composition of Gases

3.3 The Molar Volume Pages

Chemical Quantities or

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

Chapter 19 Avogadro’s Principle.

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities

Avogadro’s Law.

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.

Chapter 10: Chemical Quantities

The Mole Concept.

10.2 Molar Relationships.

C2H6 CH3 B. Empirical Formula

Molar Volume Chapter 7-2.

Unit 5A Mole – Volume Relationships

The Mole Molar Conversions.

Chapter 10: Chemical Quantities Mole – Volume Relationships

Presentation transcript:

Two Relationships 1 mole = molar mass in grams of any element or compound (use periodic table) 1 mole = 6.022 x 1023 particles (molecules, atoms, formula units) Put these relationships on the back of your periodic table.

Each group of two will need a small whiteboard and marker. One eraser per table

How many molecules are in 4 moles of C6H12O6? How many moles of Mg are in 3.01 x 1022 atoms of Mg? What is the mass in grams of .720 mol Be? How many moles of NaCl are in a 124.68 g sample? How many moles are in 32L of CO2 at STP? How many liters are in 5.2 moles of water vapor?

Calculating the Volume and Moles of a Gas at STP STP-Standard Temperature and Pressure 0⁰C and 1 atm Only deals with gases 1 mole of a gas occupies a volume of 22.4 L 1 mole = 22.4 L Called molar volume of a gas

Example Problems 1. When carbon dioxide is at STP what would be the volume of .00320 moles of that carbon dioxide gas? 2. At STP, how moles of sulfur dioxide gas are in 67.2 Liters? 3. What is the volume of 3.70 moles of nitrogen gas at STP? 4. If .880 L of He gas is at STP how many moles would make up that volume of gas?

Multi-Step Problems Determine what you are given and what you are trying to find. Are they directly related? Can you convert from one unit to another using one of the three relationships If not, how can we connect them? The mole! We will need to use multiple relationships-multiple steps Using the mole to connect them

Answer the following questions : How many atoms are in .360 mol of Aluminum? How many moles are in 465.2 g of potassium nitrate? How many formula units are in 4.65 g of sodium chloride? How many grams are 9.64 x 1023 atoms of Copper? How many formula units are in 0.0273 moles of MgCl2? How many grams of lead is 9.3 x 1015 atoms of lead? What is the volume of 2.63 x 1025 molecules of carbon dioxide gas @ STP. How many atoms are in 789.3 grams of ethane, C2H6?

How many grams of lead is 9.3 x 1015 atoms of lead? 2. What is the volume of 2.63 x 1025 molecules of carbon dioxide gas @ STP.

Answer the Following questions in your notebook How many liters of Fluorine gas @ STP are in .365 grams? How many atoms are in 82.0 g of Kr? How many formula units are in 2.73 moles of CaCl2? How many grams of Iron (III) oxide is 9.3 x 1017 molecules?