'4 mol' diaporamas de présentation

Homeostasis of internal enviroment

Homeostasis of internal enviroment. Acid-base homeostasis. External environment of organism. 1865 Claude Bernard. Internal environment of the cells. External environment of organism.

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PRINCIPLES OF CHEMISTRY II CHEM 1212 CHAPTER 14

PRINCIPLES OF CHEMISTRY II CHEM 1212 CHAPTER 14. DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university. CHAPTER 14 CHEMICAL EQUILIBRIUM. CHEMICAL EQUILIBRIUM. - Many reactions do not go to completion

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CHEMICAL REACTIONS Chapter 4

CHEMICAL REACTIONS Chapter 4. Reactants: Zn + I 2. Product: Zn I 2. Chemical Equations. Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al(s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The numbers in the front are called stoichiometric coefficients

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Chapter 12 Solutions

Ethylene glycol is added to a radiator to form a aqueous solution that has a lower freezing point than water. Chapter 12 Solutions. 12.7 Properties of Solutions. Solutions. Solutions contain small particles (ions or molecules) that are uniformly dispersed in the solvent

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Stoichiometry

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Chapter 12: Day 5

Chapter 12: Day 5. Ch12_stoic. Mass product. Mass reactant. Moles reactant. Moles product. STOICHIOMETRY CALCULATIONS. Molar mass Unknown. Molar mass given. Stoichiometric factor.

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STOICHIOMETRY

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A-B = Solid ice, temperature is increasing.

Heating and cooling curve for water heated at a constant rates. A-B = Solid ice, temperature is increasing. Particles gain kinetic energy, vibration of particles increases. Ice.

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STOICHIOMETRY

STOICHIOMETRY. Mole-Mole Mole- Mass Mass-Mass. STOICHIOMETRY. - the study of the quantitative aspects of chemical reactions. Moles reactant. Moles product. STOICHIOMETRY CALCULATIONS. Stoichiometric factor. Coef. Want Coef. given. Mole -Mole Problems. Moles of the

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Starter for 10

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Stoichiometry

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Stoichiometry

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المنظومة التالية توضح العلاقات التي تربط قانون الغازات العام مع ك

PV = nRT. الكثافة. الوزن الجزيئي M.wt. الكتلة Wt. (gm). الضغط. الحرارة. ثابت الغاز. الحجم. المول. المنظومة التالية توضح العلاقات التي تربط قانون الغازات العام مع كل من قانون المول الوزني وقانون المولارية الحجمي مع الكثافة كالتالي:. m. V. P M. =. RT. dRT. P.

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9.1 NOTES Stoichiometry

9.1 NOTES Stoichiometry. I. What is Stoichiometry? Definition: 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 and energy.

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STOICHIOMETRY

STOICHIOMETRY. - the study of the quantitative aspects of chemical reactions. STOICHIOMETRY. It rests on the principle of the conservation of matter. 2 Al(s) + 3 Br 2 (liq) ------> Al 2 Br 6 (s).

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Stoichiometry Part II

Stoichiometry Part II. Converting Past Mole-Mole. Many stoichiometry problems follow a pattern: grams(x) ? moles(x) ? moles(y) ? grams(y). We can start anywhere along this path depending on the question we want to answer.

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REACTION STOICHIOMETRY FACTOR LABEL LOGIC

REACTION STOICHIOMETRY FACTOR LABEL LOGIC 2 C 6 H 14(g) + 19 O 2 (g) ? 12 CO 2(g) + 14 H 2 0 (g). CALCULATE THE YIELD OF WATER IN GRAMS IF 32 GRAMS OF OXYGEN IS CONSUMED IN THE ABOVE BALANCED REACTION. KNOWN 32.O g O 2. ( ). ( ). ( ). OBJECTIVE 13.23 g H 2 O.

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Stoichiometry: Loss of CO 2

Stoichiometry: Loss of CO 2. General Chemistry 101/102 Laboratory Manual University of North Carolina at Wilmington. Stoichiometry: Loss of CO 2. Purpose. To apply the concept of limiting reactant to determine the stoichiometry of a reaction using the method of continuous variation.

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Stoichiometry

Stoichiometry. Mrs. Russotto. Working a Stoichiometry Problem. E) How many grams of K 2 O will be produced from 0.50 g of K ?. 4 K + 1 O 2 ? 2 K 2 O. 0.50 g K. 1 mol K. 2 mol K 2 O. 94.20 g K 2 O. =. ? g K 2 O. 4 mol K. 1 mol K 2 O. 39.10 g K. 0.60 g K 2 O.

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The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction

The equilibrium constant, K, is 24 x 10^1 at a certain temperature for the reaction 2NO (g) ? N 2 (g) + O 2 (g) For which of the following sets of conditions is the system at equilibrium? For those that are not at equilibrium, in which direction will the system shift?

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