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Mole

Mass Relationships in Chemical Reactions Practice QuestionsG

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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

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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

Percent composition and mole conversions pt 2 - Notes

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Percent Composition PURPOSE and PROCEDURE To find out the percentage (by mass) of a particular element in a chemical compound. Calculate the molar mass for the compound. Divide the mass of the element you want to find the percentage of by the molar mass of the compound. Write the answer you get from step B in percentage form. Round your percentage to the tenth. EXAMPLES What percent of Cu2O is O? 2 x Cu = 2 x 63.5 = 127.0 g 1 x O = 1 x 16.0 = 16.0 g molar mass = 143.0 grams/mol % O = Part ? Total = 16.0 ? 143 = .1118 x 100% = 11.2% Example What percent of Al2O3 is Al? 2 x Al = 2 x 27.0 = 54.0 g 3 x O = 3 x 16.0 = 48.0 g molar mass = 102.0 grams/mole % Al = Part ? Total = 54 ? 102 = .5294 x 100% = 52.9% Practice - Find the percent composition

Mole conversions - Notes

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Chemical Quantities The MOLE CHAPTER 7 THE MOLE: A MEASUREMENT OF MATTER A mole (mol) is a unit of measurement Types of measurement include Counting/weighing/volume/ number of units Examples of other Quantitative measurement units Pair/Dozen/Ream Mole The term representative particles is a generic term that can refer to Atoms (single element), or Diatomic molecules (two of one type of element), or Formula units (what makes up an ionic compound) or Molecules (what makes up a molecular compound), or electrons or protons, or ions, etc Mole It is typically referred to as a mole of atoms or a mole of molecules A mole is also called Avogadro?s number For example: One mole would be 6.022 x 1023 representative particles Why use moles?

inorganic chemistry lab report: Water Hydration

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1 Experiment 4: Water Hydration Objective: The objective of this experiment is to determine the formula of the hydrate and the percent water in the hydrate by heating the hydrate and dry out the water and determine the mole of water and anhydrate in the hydrate. Method:

Principles of Chemistry I Chapter 3

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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 4

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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

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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) ?

Chapter 4

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Chemistry 1210: General Chemistry Dr. Gina M. Florio 13 September 2012 Jespersen, Brady, Hyslop, Chapter 4 The Mole and Stoichiometry CHE 1210 Lecture Slides G.M. Florio 1 Conversion Factors Conversion Factor ? relates one quantity to another ? used to convert between two units in chemistry What is my height in centimeters (cm) if I am 5 feet 4 inches tall? 1. How many inches are in a foot? 2. How many inches are in a centimeter? 12 inches = 1 foot 1 inch = 2.54 cm Factor Label Method The factor-label method, or dimensional analysis lets us treat a numerical problem as one involving a conversion from one kind of units to another using conversion factors.

Bob Jones PPT Notes -- Chapter 10c

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Gases and the Mole Gay-Lussac formulated the law of combining volumes. Law of Combining Volumes Gases at the same temperature and pressure react with one another in volume ratios of small whole numbers. Law of Combining Volumes Example 1: H2 + Cl2 2HCl 1 L + 1 L 2 L Law of Combining Volumes Example 2: 2H2 + O2 2H2O 2 L + 1 L 2 L Avogadro?s law The volume of a gas, maintained at a constant temperature and pressure, is directly proportional to the number of moles of the gas. Molar Volume the volume that a mole of gas occupies at standard temperature and pressure Molar Volume 1 mole of ANY gas at STP occupies 22.4 L. Sample Problem 1 What volume would 7 moles of carbon dioxide occupy at STP? = 157 L CO2 7 mol CO2 22.4 L 1 mol Change 228 L of O2 at STP to moles. 470 moles 426 moles

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