'G h2o' presentation slideshows

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Bell Ringer

2. 2. 1 mol O 2. 10 mol Mg. 5 mol O 2. x. =. 2 mol Mg. Bell Ringer. Please take out a piece of paper and answer the following question individually : When magnesium metal is burned, it forms MgO. How many moles of oxygen gas are needed to burn 10 moles of Mg? A 2 B 5 C 10

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Ch 17-18 Review

Ch 17-18 Review. 1. A clear solution of silver nitrate is mixed with a solution of sodium chloride and a white precipitate forms. Write a balanced equation for this reaction. Write a complete ionic equation. Write a net-ionic equation. 2. Define the following: a. Hydrogen bonds

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Freezing Point Studies of Ethylene Glycol Solutions Freshman Chemistry

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Percentage Yield

Percentage Yield. Assignment: Read 5.6 up to sample (238-9) Define the following terms: yield, theoretical yield, actual yield, percentage yield. Based on your reading, give 4 reasons why the actual yield in a chemical reaction often falls short of the theoretical yield.

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XI. RELATIVE HUMIDITY

XI. RELATIVE HUMIDITY. A. RH range outside B. High RH conditions in greenhouse Apr--May & Aug--Sept bright cool days cool nights June--July bright warm days cooler but warm nights C. Low RH conditions in greenhouse Oct--Mar usually heating cooler air dry to very dry environment.

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THERMODYMANICS

THERMODYMANICS. Thermodynamics is the study of the motion of heat energy as it is transferred from the system to the surrounding or from the surrounding to the system. The transfer of heat could be due to a physical change or a chemical change.

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Limiting and Excess Reactants

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Digital Help Sessions to Enhance Chemistry Courses

Digital Help Sessions to Enhance Chemistry Courses. Dr. Robert R. Klepper Professor of Chemistry Iowa Lakes Community College Estherville, Iowa . Challenges Faced. Too few instructors Too many students Many times under prepared students Not enough time

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Chapter 12: Stoichiometry

Chapter 12: Stoichiometry. Mr. Samaniego Lawndale High. Problem 12.2 (moles of product). How many moles of ammonia are produced when 0.60 mol of nitrogen reacts with hydrogen?. mol = ? (NH 3 ) 0.60 mol N 2. N 2 + H 2 NH 3. 3. 2. 0.60 mol N 2. = 1.2 mol NH 3.

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Limiting and Excess Reactants

Limiting and Excess Reactants. LIMITING REACTANTS. LIMIT HOW MUCH OF THE PRODUCT CAN ACTUALLY BE PRODUCED DURING THE REACTION. EXCESS REACTANTS. The reactants that are left over when the reaction stops. *When all the limiting reactant is used up. How to find the limiting reactants.

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Section 13.1 Quantitative Expressions of Concentration

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Chapter 13

Chapter 13. Solids and Liquids. Molar Heat of Vaporization. The amount of heat energy required to vaporize one mole of liquid at its boiling point. Joules are the standard unit to measure heat energy. Molar heat of vaporization for water is 40.7 kJ/mole .

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Mass Relationships in Chemical Reactions

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Solubility vs. Temperature

gases. solids. Solubility vs. Temperature. 140. KI. 130. 120. NaNO 3. 110. 100. KNO 3. 90. 80. HCl. NH 4 Cl. 70. Solubility (grams of solute/100 g H 2 O). 60. NH 3. 50. KCl. 40. 30. NaCl. KClO 3. 20. 10. SO 2. 0 10 20 30 40 50 60 70 80 90 100.

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Combustion Analysis

Combustion Analysis. P. Perkerson. A little reminder!.

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Molecular Formula Calculations Combustion & Weight Percent

Molecular Formula Calculations Combustion & Weight Percent. C x H y + ( x + y/4) O 2 ? x CO 2 + y/2 H 2 O C 2 H 5 OH + 3 O 2 ? 2 CO 2 + 3 H 2 O. Combustion Analysis. C x H y + O 2 ? x CO 2 + y/2 H 2 O. y 4. y 2. C x H y + ( x + ) O 2 (g) ? x CO 2(g) + H 2 O (g).

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Changes in Matter

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Combustion Analysis

Combustion Analysis. The composition of a substance is often determined by using a specified reaction to break down the substance into known measurable compounds. Organic compounds are often analyzed by combustion. 1. Define combustion.

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Determining the Formula of a Hydrocarbon by Combustion

Determining the Formula of a Hydrocarbon by Combustion. CCR, page 138. Using Stoichiometry to Determine a Formula. Burn 0.115 g of a hydrocarbon, C x H y , and produce 0.379 g of CO 2 and 0.1035 g of H 2 O . C x H y + some oxygen ---> 0.379 g CO 2 + 0.1035 g H 2 O

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