Pre-WARM-UP 2/17/15 Solve the following without a calculator.

Slides:

Advertisements

Similar presentations

Entry Task: Block 1 Feb 1st- 2nd Block 2

Advertisements

General Stoichiometry

Aim: How to calculate Percent Composition

5.2 Mass and The Mole Learning Goals …

Converting using molar mass

0.277 mol ammonium acetate Convert to grams: mol NH 4 C 2 H 3 O 2 Step 1: Write the formula  NH 4 C 2 H 3 O 2 Step 2: Write the given information.

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.

Friday, April 15 th : “A” Day Monday, April 18 th : “B” Day Agenda  Homework Problems/Questions  Finish Section 7.3 (we’re almost done…)  In-Class:

Titration Calculations Practice. Titration Formula: (#H + ) M a V a = M b V b (#OH - )

Review: Molar Mass of Compounds

Complete the table… If you have the workbook – it’s page 107.

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

Using Chemical Formulas 7-3 Beaker Breaker 1.Name the following compounds: CaCl 2 = ____________ P 3 O 6 = _____________ FeCl 2 =______________ H 2 SO.

Types of Chemical Reactions We will study 4 types.

To Do… Lab tomorrow. Read Chapter 13. Lon-Capa (HW2 Type 2 due Wednesday, February 5 by 7 pm). 1.

Wednesday, March 19 th : “A” Day Thursday, March 20 th : “B” Day Agenda  Collect Homework: pg. 21/22 practice worksheet  Continue Section 7.1: “Avogadro’s.

MOLAR MASS. What is Molar Mass  The SUM of the atomic masses of the atomic species as given in the molecular formula.  2 x g= g/ mole Cl.

Percent Composition. HW – Ques. 7.1 Find the mass of each of the following: a.0.50 mole of NaOH b.4.5 moles of CaCO 3 c.0.25 mole of Ba(NO 3 ) 2 d.3.00.

The Mole and Avogadro’s Number

Section 4: Moles of Compounds

Chp.12/ Activity 2 More chemical changes (page 779) Learning targets Observe examples of evidence that a chemical change is occurring Make generalizations.

3.10 Determining a Chemical Formula from Experimental Data

How is the mole concept related to chemical formulas?

Wake-up 1.Study Polyatomic Ions for about 5/10 minutes. Write NO WAKE-UP on Friday.

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.

Recall: A limiting reagent is the reactant whose entities are completely consumed in a reaction. It is the one that runs out first, and as a result, stops.

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.

Percent Composition. Percent Composition from the Chemical Formula % mass = mass of element in 1 mole of compound molar mass of compound Then multiply.

Stoichiometry Chapter 11 & 12. I. Things you should remember From the Moles Unit: Identify particles as atoms, molecules (mc), and formula units (fun)

Telling a story…. We are going to take a written description about a chemical reaction and transfer it into a balanced chemical equation !

The Mole Concept. The Mole The mole (mol) is a unit of measure for an amount of a chemical substance. A mole is Avogadro’s number of particles, that is.

Section 3 Moles of Compounds Objectives: Recognize the mole relationship shown by chemical formula Calculate the molar mass of a compound Calculate the.

What are the signs that a chemical reaction has taken place?

Aim: How to calculate Percent Composition  DO NOW: 1. What is the number of moles of potassium chloride present in 148 g? 2. What is the molar mass of.

Got Mole Problems?.

No Bell Ringer Today. We will have a test next Tuesday.

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

J OURNAL #72 How many moles of compound are there in 6.00g of ammonium sulfate? How many molecules are there in 20.0g sulfuric acid?

Percent Composition Molar Mass Molar Conversions Empirical Formulas Random

Another Practice Problem. You walk into a room and find two chemical bottles open and sitting out. One contains lead (II) nitrate and the other potassium.

Percent Composition Determine the mass percentage of each element in the compound. Determine the mass percentage of each element in the compound. Mass.

16.1 Properties of Solutions > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1. Calculate and record your % grade. Test.

Stoichiometry Pronounced: Stoy-kee-AHM-uh-tree. What is stoichiometry? Its math that helps us to see the relationship between what is used and formed.

MOLAR MASS CHAPTER 7-2.

Chemistry – Mar 15, 2017 P3 Challenge –

The Mole and Avogadro’s Number

9.5 Solutions stoichiometry.

CHEMISTRY Feb 24, 2011.

Percent Composition Calculations

WARM-UP 2/2/15 Write down a chemical equation that would show the decomposition of hydrogen peroxide (H2O2). If copper mixed with silver nitrate (AgNO3),

Chapter 7 – Chemical Formulas and Chemical Compounds

average mass of H2O molecule: amu

CONCENTRATION OF SOLUTIONS

Acids and Bases.

Chemistry 202 Dr. Don DeCoste 3014 Chemistry Annex

Chemistry – Apr 13, 2018 P3 Challenge –

Moles to Atoms Conversion Answers:

Chemistry – Apr 12, 2018 P3 Challenge –

The Mole Concept.

Warm-Up 4/16/15 Recap: From the picture below, how much NaOH was used for neutralization (mL)? Add-on: If the concentration of the NaOH solution was 0.1.

Warm Up # 1 Using the terms solution, solvent and solute, explain how dissolving works. What property of water allows it to have a lower density in its.

Chapter 12: Stoichiometry

Percent Composition.

WARM-UP 2/20/15 You will need a calculator (no phone) today. If you need one, trade something for one. If you measured the mass of the beaker with the.

1. Calculate the number of atoms in 1.5 moles of aluminum.

What is the molar mass of water?

Chemistry – Apr 5, 2018 P3 Challenge –

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

Chemistry 202 Dr. Don DeCoste 3014 Chemistry Annex

Presentation transcript:

Pre-WARM-UP 2/17/15 Solve the following without a calculator.

WARM-UP 2/17/15 What is the molar mass of copper (II) nitrate? If you measured the mass of the beaker with the sample of copper (II) nitrate to be 54.4 g and the mass of the beaker by itself was 8.2 g, what is the mass of the sample? How many moles of copper (II) nitrate are there?

Calculate moles using molar mass 2/17/15 Objective Calculate moles using molar mass 2/17/15 Agenda Warm-up Recap Friday Molar Mass Lab Independent Work Time

Recap Friday Chemical Reactions Test – By Wednesday 2) Chemical Reactions Lab Checklist – Resubmit by Friday

Molar Mass Lab – 1st Chart Compound Chemical Formula Molar Mass 1 Sodium hydroxide NaOH 39.997 g/mol 2 Zinc (II) nitrate 3 Copper 4 Iron 5 Sodium iodide 6 Copper (II) nitrate 7 Potassium chlorate 8 Lead (II) nitrate 9 Zinc 10 Sodium nitrate

Molar Mass Lab – 2nd Chart Chemical Formula Beaker Mass (g) Measured Mass (g) Compound Mass (g) Moles of Compound NaOH 5.92

Chemical Reactions Checklist Homework Chemical Reactions Checklist Resubmit by Friday 2/20/15