'5 moles' diaporamas de présentation

The Mole 1

The Mole 1. The Mole 2. The Mole 3. Stoichiometry Mole to Mole. Stoichiometry. Potpourri. The Mole 1. The Mole 2. The Mole 3. Stoichiometry mole to mole. Stoichiometry. Potpourri. $100. $100. $100. $100. $ 100. $100. $200. $200. $200. $200. $200. $200. $300. $300. $300.

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The Mole

The Mole. Chap. 11. No, not that mole!. Counting Particles. Counting Particles. There are common units to count things. Counting Particles. There are common units to count things. Pair. Counting Particles. There are common units to count things. Pair = 2 Dozen. Counting Particles.

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CHAPTER 11

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O.A # 11

O.A # 11. Mole Ratio. Objective. Determine the mole ratios from a balanced equation. Page # 7 Mole to Mole Stoichiometry Mole Ratio is a ratio between the number of moles of any 2 substances in a chemical equation. Stoichiometric Calculations.

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$$$ Quiz $$$ Solutions

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Stoichiometry

Stoichiometry. What is Stoichiometry?. Stoichiometry is the study of quantitative relationships between the amounts of reactants used and products formed by a chemical reaction; based on the law of conservation of mass. Goals for the unit. Write mole ratios from balanced chemical equations

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Molar Weight

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Properties of Solutions Solution: Homogenous mixture of 2 or more substances

Properties of Solutions Solution: Homogenous mixture of 2 or more substances Solutions can be liquid, solid or gaseous Examples: Ocean, sugar water Gold alloy Air, humid oxygen. Solvent: Substance present in a solution in the greatest amount

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Understanding Chemical Reactions

Understanding Chemical Reactions. Lesson: Calculations in Chemistry 2. Page 175 Q 4. One mole of ZnO has a RAM of 65 + 16 = 81g 0.2 moles will have a mass of 0.2 X 81 = 16.2 g. Page 175 Q 4. b) 1 mole of H 2 S has a mass of (2x1) + 32 = 34g 2.5 moles will have a mass of

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So what unit do chemists use to count particles?

So what unit do chemists use to count particles? Particles are so tiny, chemists use the unit of moles. A mole contains 6.02 x 10 23 atoms. 602, 000, 000, 000, 000, 000, 000, 000. 602,000,000,000,000,000,000,000.

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Catalyst

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Way Back Wednesday!

Way Back Wednesday!. What is the difference between an ionic and covalent bond? Name one element in the family of the halogens . Which of these is a nonmetal: K, Ni, As, Cl ?. You must be silent and working for credit B e on time E nter silently G rab papers I mmediately start work

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Mole and # of Particles

Mole and # of Particles. A mole contains 6.02 x 10 23 particles. How many particles are in 2.0 moles of particles? 2 mol x 6.02 x 10 23 particles/mol = 12.04 x 10 23 particles = 1.2 x 10 24 particles When changing moles to number of particles simply

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TOPIC: Predicting amounts of reagents needed or amounts of products made Do Now:

TOPIC: Predicting amounts of reagents needed or amounts of products made Do Now:. Coefficients in Chemical Equations. Numbers in front of formulas called coefficients Microscopic: Coefficients represent numbers of individual atoms or molecules Macroscopic: Coefficients give mole ratios!

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Ch. 10.2 Mole-Mass and Mole-Volume Relationship

Ch. 10.2 Mole-Mass and Mole-Volume Relationship. The Mole-Mass Relationship. Molar mass of any substance is the mass in grams of one mole of that substance. Applies to atoms, molecules, formula units, etc.

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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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TYPES OF FORMULA

TYPES OF FORMULA. EMPIRICAL FORMULA. - lowest whole number ratio of the elements in a compound STEPS 1. Given the % composition, change the percent to grams. 2. Change the grams to moles using the formula n = GW MM 3. Calculate the lowest whole number ratio of the moles.

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When 3 cm 3 of ethylene and 12 cm 3 of hydrogen are mixed

When 3 cm 3 of ethylene and 12 cm 3 of hydrogen are mixed under appropriate conditions, they react to form ethane: C 2 H 4(g) + H 2(g) C 2 H 6(g) What is the final volume of the reaction mixture ?. When 3 cm 3 of ethylene and 12 cm 3 of hydrogen are mixed

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3) What is the % by mass of oxygen in H 2 SO 4 ? [ GFM=98]

3) What is the % by mass of oxygen in H 2 SO 4 ? [ GFM=98]. % COMP (MASS) = PART X 100 WHOLE. % Oxygen = 63.9976 X 100 98. = 65.3 % ~ 65 %.

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