AP Notes, Outlines, Study Guides, Vocabulary, Practice Exams and more!

Mole

Chemistry Chp. 9 Review

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemistry
Stoichiometry
Nature
Chemical reactions
Chemical reaction engineering
Equations
Yield
Limiting reagent
Conversion
Mole
Air–fuel ratio
Chemical reaction

Holt Modern Chemistry Review CHAPTER 9: STOICHIOMETRY The following pages contain the bulk (but not all) of the information for the chapter 9 test. Focus on this content, but make sure to review class notes, activities, handouts, questions, etc. If you study this document and NOTHING else, you should at least be able to PASS the test. ***** Test items will be recall, examples, and/or application of this content. ***** OUTCOMES Collaborate with peer(s) to understand chemistry content (C C) Communicate chemistry content to teacher and peer(s) (E C) 9.1: Determine number of moles from balanced chemical equations. (T & R) 9.2: Perform stoichiometry calculations such as: mole to mole, mole to gram, gram to mole, and gram to gram. (F & PK)

Chemistry Chp. 9 Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemistry
Stoichiometry
Nature
Chemical reactions
Chemical reaction engineering
Yield
Limiting reagent
Conversion
Mole
Air–fuel ratio
Molar mass
Chemical reaction

Chapter 9 - Stoichiometry 9-1 Introduction to Stoichiometry Composition Stoichiometry - deals with mass relationships of elements in compounds Reaction Stoichiometry - Involves mass relationships between reactants and products in a chemical reaction I. Reaction Stoichiometry Problems A. Four problem Types, One Common Solution given mass ? given moles ? unknown moles ? unknown mass 1. Given and unknown quantities are in moles 2. Given is an amount in moles and the unknown is a mass (usually in grams) 3. Given is a mass in grams and the unknown is an amount in moles 4. Given is a mass in grams and the unknown is a mass in grams B. Mole Ratio 1. A conversion factor that relates the amounts in moles of any two substances involved in a chemical reaction

Chemistry The Central Science Chapter 3

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemistry
Nature
Stoichiometry
Chemical reactions
Mass
Chemical reaction engineering
Yield
Mole
Amount of substance
Molar mass
Empirical formula
Limiting reagent

Chapter 3 Chemical Reactions and Reaction Stoichiometry James F. Kirby Quinnipiac University Hamden, CT Lecture Presentation ? 2015 Pearson Education, Inc. Stoichiometry The study of the mass relationships in chemistry Based on the Law of Conservation of Mass (Antoine Lavoisier, 1789) ?We may lay it down as an incontestable axiom that, in all the operations of art and nature, nothing is created; an equal amount of matter exists both before and after the experiment. Upon this principle, the whole art of performing chemical experiments depends.? ?Antoine Lavoisier ? 2015 Pearson Education, Inc. Chemical Equations Chemical equations are concise representations of chemical reactions. Stoichiometry ? 2015 Pearson Education, Inc. 3 What Is in a Chemical Equation?

Stoichiometry Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemical engineering
Stoichiometry
Mole
CNote
World Wide Web
Film
Measurement
Humanities
Technology
Tags: 
Stoichiometry

Stoichiometry mass and amount relationships between reactants and products in a chemical reaction Rules for Solving Stoichiometry Problems A balanced, properly written equation is essential because the coefficients tell you the mole to mole ratio. Converting to moles is essential! Example: When CaC2 reacts with water, acetylene gas (C2H2) and calcium hydroxide are produced. How many grams of water are required to produce 1.55 moles of C2H2? Step 1: Write a balanced equation. CaC2 + 2H2O ? C2H2 + Ca(OH)2 Step 2: Determine what info you have and what you are trying to determine. You know you need to produce 1.55 moles of C2H2, and you need to determine how many grams of water are required to do this.

mols

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Mole
Amount of substance
Wilhelm Ostwald
CNote
World Wide Web
Chemistry
Science and technology in Germany
Measurement
The mole is a unit of measurement for the amount of substance or chemical amount. It is one of the base units in the International System of Units, and has the unit symbol mol.[1] The name mole is an 1897 translation[2][3] of the German unit Mol, coined by the chemist Wilhelm Ostwald in 1893,[4] although the related concept of equivalent mass had been in use at least a century earlier. The name is derived[5] from the German word Molekül (molecule).

molarity and dilution

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemistry
Analytical chemistry
Solutions
Chemical properties
Colloidal chemistry
Dilution
Equations
Molar concentration
Mole
Technology

Molarity Worksheet 1. Sea water contains roughly 28.0 g of NaCl per liter. What is the molarity of sodium chloride in sea water? 2. What is the molarity of 245.0 g of H2SO4 dissolved in 1.00 L of solution? 3. What is the molarity of 5.30 g of Na2CO3 dissolved in 400.0 mL solution? 4. What is the molarity of 5.00 g of NaOH in 750.0 mL of solution? 5. How many moles of Na2CO3 are there in 10.0 L of 2.0 M soluton? 6. How many moles of Na2CO3 are in 10.0 mL of a 2.0 M solution? 7. How many moles of NaCl are contained in 100.0 mL of a 0.20 M solution? 8. What weight (in grams) of NaCl would be contained in problem 7? 9. What weight (in grams) of H2SO4 would be needed to make 750.0 mL of 2.00 M solution? 10. What volume (in mL) of 18.0 M H2SO4 is needed to contain 2.45 g H2SO4?

AP Chemistry

Subject: 
Chemistry
Rating: 
0
No votes yet
SocialTags: 
Chemistry
Nature
Mass
Chemical properties
Stoichiometry
Nuclear chemistry
Chemical reactions
Atomic mass
Mole
Limiting reagent
Oxygen
Chemical formula
Tags: 
chapter 1-3
Chapter1 • Precision vs accuracy • Sig figs • Metrics • Classification of matter o Pure substances o Compounds, elements, mixtures o Examples o Homogeneous vs heterogeneous mixtures o Separation of mixtures • Dimensional analysis (show correct set-up, units, cancellations) • History of atomic theory o Dalton model o JJ Thomson o Plum pudding model o Rutherford’s experiment and model o Millikan’s experiment • Atomic structure o Atomic number o Mass number o Isotope designations o Ions • NOMENCLATURE • Atomic mass o Define  Calculate atomic mass, given isotope abundances  Disc why samples of elements with same mass rations as atomic mass mean equal number of atoms (Avogadro’s Hypothesis) • Mole o Define
Subscribe to RSS - Mole

Need Help?

We hope your visit has been a productive one. If you're having any problems, or would like to give some feedback, we'd love to hear from you.

For general help, questions, and suggestions, try our dedicated support forums.

If you need to contact the Course-Notes.Org web experience team, please use our contact form.

Need Notes?

While we strive to provide the most comprehensive notes for as many high school textbooks as possible, there are certainly going to be some that we miss. Drop us a note and let us know which textbooks you need. Be sure to include which edition of the textbook you are using! If we see enough demand, we'll do whatever we can to get those notes up on the site for you!