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Mole

Bob Jones PPT Notes -- Chapter 9b

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Chemistry
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Chemistry
Chemical reactions
Stoichiometry
Limiting reagent
Mole
Zinc
Neutralization
water
Yield

Stoichiometry 1 Literally means ?to measure the elements? Answers questions like?How much is needed?? and ?How much is produced?? Stoichiometry Unit analysis 365 days 1 year 24 hrs 1 day 3600 sec. 1 hr 1 year How many seconds are in a year? = 31,536,000 sec. Unit analysis We use unit analysis in stoichiometric problems also. Grams-to-moles conversion factors are found in the periodic table. Unit analysis Mole-to-mole conversion factors are found in the coefficients of the equation. A mole-to-mole conversion changes moles of one substance to moles of another substance. ?Skeleton Equation?

Chapter 3/4

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Chemistry
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Chemistry
Stoichiometry
Bases
Physical chemistry
Equilibrium chemistry
Chemical reactions
Titration
solubility
Strong electrolyte
Chemical equation
Mole
Limiting reagent

Claire Rafson Chapter 3 notes 3.1 You can count things by weight 3.2 Atomic mass determined on a mass spectrometer Average atomic mass = atomic mass for the element 3.3 Avogadro?s number = 6.02214 X 10^23 1 mole = avogadro?s number 3.4 molar mass= mass in grams of one mole of the compound 3.5 Percent comp of compounds Mass percent- weight percent can be computed by comparing the mass of carbon Find moles of all divide by smallest number find whole number etc. 3.6 Molecular formula= (empirical formula)n N is an integer To find molec formula take molar mass/ empirical formula mass and that is n SEE PAGE 96 IF CONFUSED 3.7- Chemical Reactions- Reactants on left and products on the right. Aq- dissolved in water 3.8- Balance reactions 3.9- Stoichiometry-

Chapter 3

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Chemistry
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Chemistry
SI base units
Mass
Chemical properties
Analytical chemistry
Molar mass
Mass fraction
Mass spectrometry
Mole
Kilogram
Molecular mass
Molar volume

Chapter 3.1 Average mass= total mass/ number of objects massed 3.2 Mass spectrometer- most accurate method currently availbe for comparing masses of atoms 3.3 Avogadro?s number- 6.022X 10^23 = one mole of something Molar mass- mass in grams of one mole of the compound g/mol Find on periodic table 3.5 Percent comp: Mass/ weight percent= (Mass of element in compound/ mass of compound)X100 3.6 Molecular formula= (empirical formula)n N is an integer To find molec formula take molar mass/ empirical formula mass and that is n SEE PAGE 96 IF CONFUSED
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AP Chemistry Lab: Determination of the Empirical Formula of Magnesium Oxide

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Chemistry
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Chemistry
matter
Chemical elements
Magnesium
Analytical chemistry
Crucible
Laboratory equipment
Oxygen
Oxide
Mole
health

Conclusion 1) One error could be if the Magnesium did not heat all the way, then there were still solid pieces of Magnesium that could have made the mass greater. Extra mass in the crucible could cause the oxygen to be too low because extra mass would consume more space and would lessen the amount of space for oxygen within the crucible. 2) a. If you put more water in to the crucible than is needed for reaction 3, and did not wait for the excess water to dry out, then there would be to little oxygen. This is because the product in the crucible and the water would increase the amount of weight of the crucible/product as a whole and would leave little space for oxygen.

Stoichiometry review questions

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Chemistry
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Chemistry
Mass
Greenhouse gases
Chemical elements
Dietary minerals
Reducing agents
Limiting reagent
Molecular mass
Mole
Molar mass
Ethane
Stoichiometry

A substance with the formula AB has the composition by mass of 30% A and 70% B. What is the composition by mass of the compound A2B? 70% A, 30% B 50% A, 50% B 46% A, 54% B 60% A, 40% B 65% A, 35% B A mass of 21.5 grams of calcium hydroxide reacts with an excess of phosphoric acid. What mass of calcium phosphate could be recovered from solution? 31.6 grams 94.7 grams 326 grams 284 grams 186 grams Given the equation 3A + 4B ? 2C + 3D, you react 5 moles of A with 7 moles of B. Which of the following statements is true? B has a greater molar mass than A A is the limiting reactant A has a greater molar mass than B

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