'Kclo3' presentation slideshows

Balancing Equations Double Odd Start Over

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Chapter 3

Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Objectives. Learn how to use chemical formulas to write chemical equations. Learn different type of reactions. Learn the relationships between masses of substances with number of moles, atoms and molecules.

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Unit 10: Solutions

Chemistry. Unit 10: Solutions. e.g., water . e.g., salt . Solution Definitions. solution : a homogeneous mixture. -- . evenly mixed at the particle level . -- e.g., . salt water . alloy : a solid solution of metals . -- e.g., . bronze = Cu + Sn brass = Cu + Zn .

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Section 1C.1 & C.2 Reading Solubility Curves

Section 1C.1 & C.2 Reading Solubility Curves. What is Solubility?. Solubility: the maximum amount of solute that will dissolve in a certain amount of solvent at a given temperature Solute = substance dissolved Solvent = does the dissolving

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Chapter 3 Chemical Calculations

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Chapter 3 Chemical Calculations

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Stoichiometry

Stoichiometry. Chapter 12. 12. 1 What is stoichiometry?. Stoichiometry is the study of quantitative relationships between the amounts of reactants used and products formed by a chemical reaction.

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Using chemical Formulas

Section 3. Using chemical Formulas. Section 3 Using Chemical Formulas. Chapter 7. A chemical formula indicates: the elements present in a compound the relative number of atoms or ions of each element present in a compound

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1 Precipitation

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Stoichiometry

Stoichiometry. 6 mol H 2 O . 4 mol NO . 1 1 .33 mol NO. 0.21 1 2 mol H 2 O. x . x . = . = . 6 mol H 2 O. 5 mol O 2. Stoichiometry questions (1). Consider : 4NH 3 + 5O 2 ? 6H 2 O + 4NO How many moles of H 2 O are produced if 0.176 mol of O 2 are used?

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Chemical Equations

Chemical Equations. These interactions are called chemical reactions . A substance that undergoes a chemical reaction is called a reactant . A substance that is formed in a chemical reaction is called a product .

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Test REVIEW

Test REVIEW. Unit 10 Thermochemistry. 1. How much heat energy is needed to raise the temperature of a 55 g sample of aluminum from 22.4 ? C to 94.6 ? C (a) in J, and (b) in calories? The specific heat of aluminum is 0.900 J/g ? C. Q = mc ?T. Q = (55 g). (0.900 J/g o C). (72.2 o C).

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PRACTICE PROBLEMS

PRACTICE PROBLEMS. How many moles of glucose, C 6 H 12 O 6 , can be burned when 10.0 mol of oxygen is available? C 6 H 12 O 6 ( s ) + 6O 2 ( g ) ? 6CO 2 ( g ) + 6H 2 O( l ). How many moles of H 3 PO 4 are produced when 71.0 g P 4 O 10 reacts completely to form H 3 PO 4 ?.

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2KClO 3 (s) ? 2KCl (s) + 3O 2 (g)

Given the following UNBALANCED equation, determine how many moles of potassium chlorate are needed to produce 10.0 mol of oxygen gas. 2KClO 3 (s) ? 2KCl (s) + 3O 2 (g). 10 mol O 2 x 2 mol KClO 3 = 6.67 mol KClO 3 3 mol O 2.

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Warm Up: Chemical Reactions #7 Sodium iodide solution is mixed with lead (II) nitrate solution

Block 64: W 4/2 and Th 4/3. Warm Up: Chemical Reactions #7 Sodium iodide solution is mixed with lead (II) nitrate solution Write the chemical equation for the reaction. Include state signifiers. Balance it. Identify the reaction type. Does this reaction occur? How do you know?

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Solubility Graph Warm Up

Solubility Graph Warm Up. How many grams of potassium nitrate can dissolve in 100 g of water at 50 ? C? a. 75 g b. 85 g c. 95 g d. 105 g What two solutions have the same solubility at 32 ? C? a. Potassium nitrate and ammonia b. Potassium nitrate and sodium sulfate

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