'10 23 molecules' diaporamas de présentation

Lesson 3 Percentage Yield and Energy

Lesson 3 Percentage Yield and Energy. PERCENTAGE YIELD AND PERCENTAGE PURITY:. Percentage Yield : is used to describe the amount of product actually obtained as a percentage of the expected amount . 2 reasons: 1. reactants may not all react 2. some products are lost

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CHEMISTRY

CHEMISTRY. The Mole. Atomic or molecular Mass The molar mass of an element is the same as the atomic mass with the units called atomic units. Molecules. An Atom. A Formula Unit. Does it add up?. What is the atomic mass of Sulfur? Look on the periodic table.

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CHEMICAL QUANTITIES

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$1 Million

50:50. Who Wants to Be a Chemist ?. 15. $1 Million. 14. $500,000. 13. $250,000. 12. $125,000. 11. $64,000. 10. $32,000. 9. $16,000. 8. $8,000. 7. $4,000. 6. $2,000. 5. $1,000. 4. $500. 3. $300. 2. $200. 1. $100. 15. $1 Million. 14. $500,000. 13. $250,000. 12.

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Mole Problems

Mole Problems. Calculating molar mass. Round all masses to the 10ths place. Calculate the molecular weight of F e 2 O 3. Step One: two atoms of iron and three of oxygen Step Two: Fe = 55.8 amu and O = 16.0 amu Step Three: (2 x 55.8) + (3 x 16.0)

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Lesson 3 Percentage Yield and Energy

Lesson 3 Percentage Yield and Energy. Sometimes reactions do not go to completion. Reaction can have yields from 1% to 100%. 1. How many grams of Fe are produced by the reaction of 100. g of Fe 2 O 3, if the percentage yield is 75.0%? 2Fe 2 O 3 + 3C ? 4Fe + 3CO 2 100. g ? g

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Molar Volume

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#47 Give three common ways that matter is measured. Give examples of each

#47 Give three common ways that matter is measured. Give examples of each. Counting: Example, counting sheep. Volume: Example: estimating the # of jelly beans in a large jar. Mass: Example: Weighing out some NaCl. #48 Name the representative particle of each substance:

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Chapter 8

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Nomenclature and Stochiometry

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Mole Calculations 1

Mole Calculations 1. Chemical Calculations. Atoms and molecules are extremely small. If they are so small and so light, how can we weigh them?. We weigh large numbers of them. Avogadro took 1.00 g of the smallest atom (H) and determined how many H atoms there are in 1.00 g of H .

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Ch. 10: The Mole

Ch. 10: The Mole. Sec. 10.1: Measuring Matter. Objectives Describe how a mole is used in chemistry. Relate a mole to common counting units. Convert moles to number of representative particles and vice versa. The Mole.

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Grams to Moles to Molecules

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Prentice Hall Chemistry (c) 2005

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Performing Stoichiometry Calculations Notes and Practice for ALMOST every possible calculation

Performing Stoichiometry Calculations Notes and Practice for ALMOST every possible calculation. Masses to moles Steps: 1) Determine molar mass of given substance 2) Divide amount given in problem by the molar mass you calculated. 1. How many moles does 80.0 grams of H 2 O represent?

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Unit 5: The Mole and Stoichiometry

Unit 5: The Mole and Stoichiometry. Mole as a Bridge. Moles and Gases. At standard temperature and pressure (STP) . . . 1 mole of any gas will occupy the same volume as any other gas at the same temperature and pressure. At STP (which is 0 o C and 1 atm):

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Charles Law V 1 = V 2 P constant T 1 T 2

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Conversions WS III

Conversions WS III. Answers. Perform the following conversions. Show all your work and include units in your answer!!. 1. How many molecules are in 0.95 moles of I 2 ? 5.72 x 10 23 molecules 2. How many molecules are in 326 g of Cu(NO 3 ) 2 ? 1.04 x 10 24 molecules

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