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

Stoichiometry

Mass Relationships in Chemical Reactions Practice QuestionsG

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Stoichiometry
Chemistry
Chemical properties
Mass
Chemical formulas
Yield
Atomic mass
Mole
Limiting reagent
Conversion
Mass fraction
Molar mass

Atomic mass mass of an atom in atomic mass units An atomic mass unit is equal to? One twelth the mass of one carbon-12 atom The average atomic mass is equal to? atomic mass on the periodic table Isotopes are atoms of the same element with a different number of ___ and so they have different ___ 1) neutron 2) masses Mole Is a counter and relates to mass.* It is similar to a dozen. *It can count the number atoms/molecules/particles. Molar Mass *is the mass of one mole of the substance. *g/mol = atomic mass of the element *molar mass of an element contains mols of atoms Avogadro's number particles/atoms/molecueles > moles *6.022x10^23 Percent Composition Mass of element/ mass of compound x 100 Tell how much an element contributes to the mass of the compound

AP Chemistry Zumdahl 7E Chapter 3 Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Stoichiometry
Chemical properties
Mass
Amount of substance
Chemical reactions
Yield
Mole
Limiting reagent
Atomic mass
Empirical formula
Molar mass
Chemistry

AP Chemistry A. Allan Chapter 3 Notes - Stoichiometry 3.1 Atomic Masses A. C-12, the Relative Standard 1. C-12 is assigned a mass of exactly 12 atomic mass units (amu) 2. Masses of all elements are determined in comparison to the carbon - 12 atom (12C) the most common isotope of carbon 3. Comparisons are made using a mass spectrometer B. Atomic Mass (Average atomic mass, atomic weight) 1. Atomic masses are the average of the naturally occurring isotopes of an element 2. Atomic mass does not represent the mass of any actual atom 3. Atomic mass can be used to "weigh out" large numbers of atoms 3.2 The Mole A. Avogadro's number 1. 6.022 x 1023 units = 1 mole 2. Named in honor of Avogadro (he did NOT discover it) B. Measuring moles

Periodic Table - Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Periodic Table
Chemical properties
Stoichiometry
Chemistry
Nuclear physics
Chemical element
Relative atomic mass
Alkali metal
Atomic mass
Atomic number
Isotope
Extended periodic table

Notes ? Periodic Table Do you know all your elements? http://www.privatehand.com/flash/elements.html Squares on the Periodic Table Each square contains Element Symbol Element Name Atomic Number = Protons Average Atomic Mass = Molar Mass Some contain the physical state at Room Temperature What is the atomic mass? The mass of one atom is VERY small therefore we use a relative scale called the AMU. One AMU is exactly 1/12 the mass of a carbon-12 atom. Protons + Neutrons = AMU = Atomic Mass Unit What is the average atomic mass? In a sample of many atoms, various isotopes exist. The abundance of each isotope impacts the average mass of the sample. To find the average atomic mass, multiply the mass times the abundance of each isotope and add these together.

Double Replacement Products - Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Solutions
Chemical properties
Chemical equation
equations
Stoichiometry
Spectator ion
Metal halides
Precipitation
Lead(II) chloride
Salt metathesis reaction
Sodium sulfate
solubility

Notes - Double Replacement Products TERMS Soluble - substances that can be dissolved in water. Insoluble - substances that cannot be dissolved in water. Precipitate - a substance that falls out of solution when it is one of the products of a reaction. Precipitates are insoluble in water. The symbol for a precipitate is ? and would be a solid (s) for the state of matter RULES In a double replacement reaction the metal parts of each reactant switch places. Write down the new products. Look up the new products in a table of solubilities. If a product is listed as being insoluble, this product is a precipitate. Write the symbol for a precipitate, ? , after any product that is listed in the table of solubilities as being insoluble.

Chemical Reactions - Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Chemical properties
Solutions
Chemical reactions
Chemical equation
equations
Stoichiometry
Salt metathesis reaction
Aqueous solution
Precipitation
Chemistry
Catalysis
solubility

REACTANTS ?PRODUCTS 1.? Starting substances (reactants) becomes new substances (products). 2. Bonds are broken and new bonds are formed, but atoms are not created or destroyed (just rearranged). Law of Conservation of Mass PRODUCTS REACTANTS SENTENCE EQUATION Iron reacts with oxygen to produce rust WORD EQUATION Iron + oxygen ? iron (III) oxide SKELETON EQUATION Fe + O2 ?Fe2O3 These DO NOT indicate the relative amounts of the reactants and products. BALANCED EQUATION most correct equation includes the physical states of each substance uses coefficients 4Fe(s) + 3O2(g)?2 Fe2O3(s) Learn chart of symbols on page 206 in text. Skeleton equation Word equation Sentence equation Balanced equation Skeleton equation Word equation Sentence equation

Principles of Chemistry I Chapter 3

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Analytical chemistry
Empirical formula
Stoichiometry
Limiting reagent
Molar concentration
Mole
Molar mass
Amount of substance
C18H37NO2
C10H12O4

Chapter 3 ? Stoichiometry this term refers to mass relationships and changes during a chemical reaction. Mass is conserved, but atoms in product are arranged differently than they are reactants. I) Mole ? A) molecules composed of atoms in definite proportion by mass and in specific ratio: butyric acid has 54.5% C, 36.4% O and 9.1 % H it also has the atoms C/H/O in the ratio 2/4/1 B) Mole is used as a measure of the amount of a substance. 1 mole is the number of 126C atoms in 12.00 g Notice it relates number of atoms to mass of those atoms in grams. It is always 6.02 x 1023 So 6.02 x 1023 atoms of 12C weigh 12.00 g Instead of looking at masses of isotopes, can use average atomic mass of atoms: Find Se on periodic table

Principles of Chemistry Chapter 5

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Gases
Physical chemistry
Gas laws
Atmospheric thermodynamics
Fluid dynamics
Partial pressure
Gas
Pressure
Stoichiometry
Atmospheric pressure
Volume
Ideal gas

Chapter 5: Gases Section 5.2: Pressure Sunday, October 19, 2014 12:43 PM Pressure = Force / Area ? **note: atmospheric pressure is caused by the weight of air molecules as they are attracted by gravity (hence why pressure decreases as altitude decreases) ? Measuring Pressure ? Barometer - device that measures atmospheric pressure Long tube filled with mercury, essentially you pour the mercury out of the tube until it stops because the mercury creates a seal and a vacuum in the closed end of the tube -pressure decreases cause the mercury seal to fall lower -pressure increases cause the mercury seal to fall higher ? Units of Pressure ? Pascal - (Pa) unit for pressure, equal to one Newton / meter squared --> Force / area

Principles of Chemistry Chapter 4

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

Chapter 4: Stoichiometry Section 4.2: Fundamentals of Stoichiometry Monday, September 15, 2014 2:32 PM Stoichiometry - study of relationships between quantities of reactants and products in chem reactions ? Obtaining Ratios from Balanced Equations ? -from the coefficients in the equation, all atoms are in ratios with one another Equation: CH4 + 2O2 = CO2 + 2H2O Ex: 1 mol CH4 : 2 mol O2 AND 1 mol CH4 : 1 mol CO2 **these are called "mole ratios" -frequently written as fractions -"molar mass ratios" relate molecular mass and molar mass ? ? This is a typical approach to solving reaction stoichiometry! ? Keep in mind the units for your final answer (in this case, grams of water) -also, use unit cancellation ? ?

Principles of Chemistry Chapter 3

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Chemical properties
Solutions
Equilibrium chemistry
Physical chemistry
Analytical chemistry
Stoichiometry
Dissociation
Aqueous solution
Chemical equation
Mole
solubility
Molar concentration

Chapter 3: Molecules and Chem Equations Section 3.2: Chemical Formulas and Equations Monday, September 8, 2014 2:44 PM Chemical Equations: symbolic representation of a chemical reaction Left side: reactants (original materials) Right side: products (compounds formed from reaction) ? Notation: Reaction w/ heat is indicated by delta Reaction w/ light energy is indicated by hv (called a photochemical reaction) ? Hints: Balance elements that occur in only one compound on each side first Balance free elements last Balance polyatomic ions as groups ? Balancing Chemical Equations Remember LAW OF CONSERVATION OF MATTER Stoichiometry: study of relationships between reactants and products in a chemical reaction (numbers in chem equations are stoichiometric coefficients) ?

Gas Stoich Notes

Subject: 
Chemistry
Rating: 
0
No votes yet
Tags: 
Gases
Atmospheric thermodynamics
Amount of substance
Gas laws
thermodynamics
Avogadro's law
Stoichiometry
Gas
Ideal gas
Standard conditions for temperature and pressure
Volume
Monatomic gas

preAP Chemistry 2013-2014 1 Name ___________________________ Period ______ I. Avogadro?s Law ? Avogadro?s Law states that ____________ volumes of gases at the __________ temperature and pressure contain equal numbers of particles. - At STP, _________________ particles (1 mol) will have a volume of ___________ Using Avogadro?s Law EX 1: Determine the volume (in L) occupied by 212 g of oxygen at STP. EX 2: Determine the density of nitrogen at STP. II. Ideal Gas Law ? Up to now we have always kept the ______________ of gas constant. Recognize that as the amount of gas changes, its corresponding _________________ changes. (Avogadro?s Law)

Pages

Subscribe to RSS - Stoichiometry

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!