Stoichiometry: Batches
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This document discusses stoichiometry and the steps to calculate the grams of water produced from the combustion of 165 grams of propane. It outlines 8 steps: 1) analyze the question; 2) write the balanced chemical equation; 3) determine moles of propane; 4) convert moles to batches; 5) determine number of batches of propane; 6) convert batches to moles of products; 7) determine molar mass of water; 8) calculate grams of water produced.
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This document provides information about performing calculations using balanced chemical equations. It discusses the three main types of calculations: (1) mole-to-mole conversions using mole ratios from balanced equations, (2) mole-to-mass conversions using molar masses, and (3) mass-to-mass conversions that involve multiple steps. Sample problems are provided as examples for each type of calculation. Key steps like identifying the problem, finding the appropriate conversion factor, and using dimensional analysis are emphasized.
Unit 7 2 stoichiometry - mole
Stoichiometry is the process of using the coefficients in a balanced chemical equation to mathematically relate the quantities of substances involved in a chemical reaction. An example shows how to use the mole ratios from a balanced equation to calculate the moles of oxygen needed for a given number of moles of hydrogen, and the moles of water that would be produced. Key aspects are setting up conversion factors using the mole ratios and canceling out the given amount to solve for the desired quantity. Practice problems demonstrate calculating unknown reactants or products from amounts of other substances in the reaction.
Stoichiometry
The document discusses different types of stoichiometry calculations encountered in AS Organic Chemistry, including:
1) Percentage yield calculations from chemical reactions.
2) Determining empirical formulas from elemental analysis data involving masses, percentages, or combustion analysis.
3) Calculating molecular formulas using empirical formulas and experimentally determined molar masses.
1/31/12
The document discusses chemical reactions, including identifying reactants and products, applying the law of conservation of matter stating the mass of reactants equals the mass of products, and recognizing that chemical reactions can form gases or precipitates. Reactants in the example reaction are S2O3 and I2, and products are S4O6 and 2I. If reactants are 12g, products are also 12g, and if reactants mass is more, a gas was likely formed. A precipitate is a solid that forms in a solution.
the mathematics of chemistry stoichiometry dimensional analysis.ppt
Here is a stoichiometry question I wrote for the given reaction:
If 3.25 grams of barium chloride are available to react, how many grams of barium sulfate can be produced?
Similar to Stoichiometry: Batches (20)
Module 6 - Calculations with Balanced Equation.pptx
Module 6 - Calculations with Balanced Equation.pptx
the mathematics of chemistry stoichiometry dimensional analysis.ppt
the mathematics of chemistry stoichiometry dimensional analysis.ppt
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みなさんこんにちはこれ何文字まで入るの？40文字以下不可とか本当に意味わからないけどこれ限界文字数書いてないからマジでやばい文字数いけるんじゃないの？えこ...
ここ3000字までしか入らないけどタイトルの方がたくさん文字入ると思います。
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みなさんこんにちはこれ何文字まで入るの？40文字以下不可とか本当に意味わからないけどこれ限界文字数書いてないからマジでやばい文字数いけるんじゃないの？えこ...
みなさんこんにちはこれ何文字まで入るの？40文字以下不可とか本当に意味わからないけどこれ限界文字数書いてないからマジでやばい文字数いけるんじゃないの？えこ...
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Stoichiometry: Batches
- 1. Javerlyn Walls Amanda Hodge Sergio Camacho
- 2. Stoichiometry • A branch of chemistry that deals with the relative quantities of reactions and products in chemical reactions. (Balancing Equations)
- 3. – Step one: Analyze the question • What is it asking? – How many grams of H2O after reaction.
- 4. –Step three: Write the Formula. C3H8 + O2 CO2 + H2O
- 5. Step Five is a long Process – Step five: Determine the number of batches in Propane. • Write the formula for propane – C3H8 • Determine the molar mass. – C = 12 ; C3 = 36 – H=8;H=8 – 36+8 = 44. Molar mass = 44. • Divide the total grams by the molar mass. – 165 44 3.75 batches
- 7. Final Steps. – Step Seven: Determine the molar mass of Water. • Write the formula. – H2O • Solve for the molar mass. – H=1.1X2=2 – O = 16. – 2 + 16 = 18. The molar mass is 18 – Step eight: Determine the overall mass. • Multiply. 15 18 270 How many grams of water do you get from the combustion of 165 grams of propane?