Compound NameFormulaMolar Mass (g) Iron (III) hydroxide Potassium nitrate Bromine gas Argon Gas Calcium phosphate Qualifying Events: Part 1: Determine.

Slides:

Advertisements

Similar presentations

Chapter 10: Chemical Quantities

Advertisements

Molar Mass and Mole Calculation Problems

Unit 5: The Mole.

Unit 7: The Mole (Chapter 10). The Mole (Ch. 10) I. Chemical Measurements (10-1) A. Atomic Mass & Formula Mass A. Atomic Mass & Formula Mass 1. The mass.

60,200,000,000,000,000,000, x

Converting using molar mass

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.

Review: Molar Mass of Compounds

Introduction to the Mole Background When you buy eggs you usually ask for a _______ eggs. You know that one dozen of any item is ______.

2 pt 3 pt 4 pt 5pt 1 pt 2 pt 3 pt 4 pt 5 pt 1 pt 2pt 3 pt 4pt 5 pt 1pt 2pt 3 pt 4 pt 5 pt 1 pt 2 pt 3 pt 4pt 5 pt 1pt ConversionsGas Laws Molar Mass Equations.

The Mole Objective What is a MOLE???? An amount of a substance A unit of measurement specific to chemistry mole mol n.

Level ONE (I) Write the correct formula for the following compounds: A. Triphosphorus Nonaselenide B. Aluminum bromide C. Cobalt (VI) Oxide.

The MOLE CH 11.

A Mole is an Unit.

Chapter 7: Chemical Formulas and Chemical Compounds

Mole-Mass Relationship. The Mole Review What is a mole? How do scientists use the concept of the mole? Who was the first person to come up with the idea.

The Mole and Avogadro’s Number

Factor Label Review & Mole Calculations. Factor Label Method 1.write down given value 2.write unit of given in denominator 3.write unit to find in numerator.

Chapter 10 – The Mole The most important concept in chemistry.

Moles Objective: To practise calculations involving a mole of a substance.

200 I’m gassy Let’s bond Stoichiometry Energizer Bunny I have the.

I. Atomic Mass 1.The unit of an element is an atomic mass unit (amu). 2.Carbon –12 has an atomic mass unit of 12. The atomic masses of other elements are.

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.

Stoichiometry and the Math of Equations Part 2: Mass-Volume.

The Mole & Stoichiometry!

I. Atomic Mass 1.The unit of an element is an atomic mass unit (amu). 2.Carbon –12 has an atomic mass unit of 12. The atomic masses of other elements are.

10.1 Measuring Matter Measuring Matter

Entry Task: Feb 4 th Monday WRITE THE QUESTION DOWN Entry Task Question: How many moles are there in 2000 grams of water (2 liters)? You have 5 minutes!

STOICHIOMETRY Calculations Based on Chemical Equations.

CHAPTER 9 Design: Winter Colors: Elemental STOICHIOMETRY.

Molar Mass Mole to Mole Mass to mass Avogadro’s Number Grab Bag

Stoichiometry It’s Finally Here!. What in the world is Stoichiometry? Stoichiometry is how we figure out how the amounts of substances we need for a.

Compound Stoichiometry. The Mole Unit for dealing with the number of atoms, ions, or molecules in a common sized sample Relationship between Moles and.

 Molar Mass. ATOMIC MASS  Mass of an atom in atomic mass units (amu)  Ex: Carbon = amu  Molecular mass—sum of atomic masses (in amu) in the.

Problem #1 For the reaction 2 H 2(g) + O 2(g)  2 H 2 O (g), how many liters of water can be made from 5 L of oxygen gas and an excess of hydrogen?

Stoichiometry is… Greek for “measuring elements” Defined as: calculations of the quantities in chemical reactions, based on a balanced equation. There.

Sections 10-1 & 10-2 Mole Conversions. 1 mole = 6.02x10 23 atoms, = molar mass (g) = 22.4 L molecules, of any gas Formula units at STP Mass – Mole Problem:

 Tin IV sulfate  Aluminum hydroxide  Oxygen gas  Iron III nitrate  Iodine.

Can’t directly measure moles Measure units related to moles: –Mass (molar mass) –Number of particles (6.02 x ) –Liters of gas (22.4 Liters at STP)

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

Molar Mass, section 7.2. A. The Molar Mass of a Substance 1) Define Molar Mass = the mass (in grams) of one mole of any element or compound Generic for.

Percent Composition. What is it? Percent composition is the percent by mass of each element present in a compound.

CO 2. WHITEBOARD PRACTICE MOLAR MASS Of COMPOUNDS.

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

Stoichiometry. Review: Dimensional Analysis Goal: To make the units cancel out Strategy: Start out with the quantity given that you are trying to convert.

Molar Mass HW 5-2.

4.3 The Mole and Volume.

The Mole: A Measurement of Matter

The Mole and Avogadro’s Number

Molar Mass and Molar Volume

CALCULATIONS USING THE MOLE (COMPOUNDS)

Ch 7.3 Using Chemical Formulas

Molar Mass HW 5-2.

Calculations Based on Chemical Equations

Bell Work 1 / Mole Map 1. Draw the Mole Map and include the relationships that exist between each section.

5.2 Stoichiometry. 5.2 Stoichiometry Moles 6.022×1023 Particles 1mol = STP 1mol = Molar Mass The mass of 1 mole of a substance in grams (also.

10.1 What is a Mole? A mole of any substance contains Avogadro’s number of representative particles, or 6.02  1023 representative particles. The term.

Warm-Up How many molecules are in 5.78 mol of ammonium nitrate?

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

(moles of solute per liter of solution)

Aim: How do chemists calculate the mass of one mole of a substance?

Calculations Based on Chemical Equations

Multi-Step Mole Conversions

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

Unit 8 Stoichiometry.

2 Step Mole Conversions: particles to Mass/Mass to Particles

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

The mole The mole is a number usually used to describe small things

Presentation transcript:

Compound NameFormulaMolar Mass (g) Iron (III) hydroxide Potassium nitrate Bromine gas Argon Gas Calcium phosphate Qualifying Events: Part 1: Determine the molar mass for each of the compounds/molecules. Record your completion time for all 5 problems.

ProblemWorkAnswer: If 1.4 moles of Iron (III) hydroxide are needed for an experiment, how many grams is this? How many moles of Potassium nitrate are represented by g of the substance? If 34.6 moles of Bromine gas necessary for a reaction, how many grams of the gas are needed? grams of Argon Gas are released from a broken light bulb, how many moles of gas were released? moles of Calcium phosphate are needed in a reaction, how many grams is this? Part 2: Mole-Grams Calculations. Record your completion time for all 5 problems.

ProblemWorkAnswer: If 1.4 moles of Iron (III) hydroxide are needed for an experiment, how many formula units is this? How many moles of Potassium nitrate are represented by 4.532x10 21 formula units of the substance? If 34.6 moles of Bromine gas necessary for a reaction, how many molecules of the gas are needed? moles of Argon Gas are released from a broken light bulb, how many atoms were released? 1.89 x moles of Calcium phosphate are needed in a reaction, how many formula units is this? Part 3: Mole-Particles Calculations. Record your completion time for all 5 problems.

ProblemWorkAnswer: If 1.4 moles of water vapor (at STP) are needed for an experiment, how many liters is this? How many moles of O 2 are represented by L of the substance at STP? If 34.6 moles of Bromine gas necessary for a reaction, how many liters of the gas are needed? (At STP) moles of Argon Gas are released from a broken light bulb, how many liters were released? (at STP) 1.89 x moles of hydrogen gas are needed in a reaction, how many liters is this? (at STP) Part 4: Mole-Liter Calculations. Record your completion time for all 5 problems.

ProblemWorkAnswer: If 1.4 g of Iron (III) hydroxide are needed for an experiment, how many formula units is this? How many grams of Potassium nitrate are represented by 4.532x10 21 formula units of the substance? If 34.6 grams of Bromine gas necessary for a reaction, how many liters of the gas are needed? (at STP) liters of Argon Gas are released from a broken light bulb, how many atoms were released? (At STP) 1.89 x formula units of Calcium phosphate are needed in a reaction, how grams are needed? Part 5: Mixed Calculations. Record your completion time for all 5 problems.