stoichiometry calculating quantities needed in a chemical reaction 1
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Stoichiometry
Calculating quantities needed in a chemical reaction
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Importance of stoichiometryEssential Learning
• Manufacturing– Pharmaceuticals, plastics, detergents, cosmetics,
fibers and dyes, fertilizers, etc. – How much materials are needed to meet
customer orders? – How much starting material must be ordered or
made? • Research: Tracking a predicted reaction based
on the amount of product
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Essential to Stoichiometry Set-up of problems
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
The mole ratio is the heart of the stoichiometry calculation
Important foundation knowledge for stoichiometry
• Mole Conversion
• Balancing chemical equations
• Writing correct formulas: – Word equations– Names & formulas
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Essential to Stochiometry Mole conversions
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Mole
Stoichiometry• Calculations to determine the __________ of
products produced or the ___________ of reactants needed in a chemical reaction.
(A) Stoichiometry calculations MUST have(1) (2)
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B. Balanced equations are the ___________ for the chemical reactions.
C. Stoichiometry calculations always use only ________ substances in the reaction.
You assume that there is a sufficient amount of other substances to react.
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Mole Ratio
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Mole ratio: tells the correct proportions of substances for a chemical reaction.
Mole ratio: Starts with a balanced equation_ H₂SO₄+__ NaOH→__ Na₂SO₄+__ H₂0
H₂SO₄ NaOH Na₂SO₄ H₂0
Name
# molecules
# moles
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Writing a Mole Ratio:
• Always use the _____________ of a ______________ equation.
• Always in a calculation, write: Mole:___________ Mole:
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Writing the mole ratio: 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
Given Mole Ratio Unknown
H₂SO₄ Na₂SO₄
H₂SO₄ H₂0
NaOH Na₂SO₄
NaOH H₂0
H₂0 H₂SO₄
Na₂SO₄ NaOH
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Types of Stoichiometry Problems
• Mole• Mass • Volume • Combinations of above (mixed problems)
• Particles (compounds, molecules, atoms)Only sometimes
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III. Mole to Mole Stoichiometry Problems
• Need ______________ equation • Need ______________ ratio
Given x
Mole Ratio = Unknown
Amount of given substance in moles
mole unknown mole given
= Amount of unknown substance in moles
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X
Mole to Mole Calculations 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• How many moles of water will be produced if there are 10 moles of sodium hydoxide?
• How many moles of sulfuric acid are required if 135 moles of sodium sulfate must be produced?
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Mole to Mole Calculations 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• How many moles of sodium hydroxide must be available to produce 17 moles of sodium sulfate?
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Review: How many moles are in 120 grams of Sodium Sulfate?
• Formula for sodium sulfate
• Molar mass of sodium sulfate
• Mole conversion
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Review: Mole to Mole Calculations
• How many moles of hydrochloric acid must be available to produce 20 moles of magnesium chloride?
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Hydrochloric acid reacts with magnesiumto yield magnesium chloride and hydrogen
IV. Gram to Gram Calculations• Must use molar mass conversions
– Molar mass means: – Use the ____________ ____________
Given Conversion Mole Ratio Conversion Unknown
Mass of given substance(grams)
X 1 mole
Molar mass of given
X Mole
unknownMole
Given
XMolar mass of unknown
1 mole
= Mass of unknown substance
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Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• Must determine the molar mass (grams)
H₂SO₄ NaOH Na₂SO₄ H₂0
Molar mass(grams of 1 mole)
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Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• If 600 grams of sodium sulfate are required, how many grams of sodium hydroxide must be used?
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Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• If 325 grams of sodium sulfate are required, how many grams of sulfuric acid must be used?
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Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• If 540 grams of sodium hydroxide are available, how much sodium sulfate ( in grams) will be produced?
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Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• If 540 grams of sodium hydroxide are available, how many grams of sulfuric acid must be used?
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Silent Lunch
• Why? Poor clean-up of the cafeteria– Expectation: You are responsible that all trash is
properly thrown away
• What: Silence– Walk down together to cafeteria in silence– Sit together in silence– All trash is thrown away and area is cleaned
• Failure to comply starts with ASD
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Agenda – Dec. 3rd
• Warm-up: Stoichiometry preparation & practice
• Stoichiometry – Graphic organizer – Practice problems – individual, pair or team– Percent Yield
• Analysis of chemical reaction problems• Mole conversion practice
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2 Li(OH)(s) + CO₂(g) → Li₂CO₃(s)+ H₂O(l)
Solid lithium hydroxide is used in the space shuttle to remove excess carbon dioxide from the living areas.
Show the problem set-up for each problem. Remember to label all quantities with units and formulas.
1. How many moles of lithium hydroxide are required to react with 15 moles of carbon dioxide?
2. If 200 grams of carbon dioxide must be removed each day, how many grams of lithium hydroxide are needed per day of the space voyage?
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Skip slides for p4
• Skip slide 40 - 46
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Mole to Gram Calculation2 Li(OH)(s) + CO₂(g) → Li₂CO₃(s)+ H₂O(l)
• If 10 moles of lithium hydroxide are available, how many grams of water will be produced?
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Gram to Liter Calculation 2 Li(OH)(s) + CO₂(g) → Li₂CO₃(s)+ H₂O(l)
• If 100 grams of lithium hydroxide are available, how many liters of carbon dioxide must be used?
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Help for Stoichiometry Problems
• Foldable • Graphic organizer
• Shows: – Mole ratio as heart (center) of all calculations– Given and Unknown – Mole conversions
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Graphic organizer
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Mole Ratio
Mole________Mole
Mole Mole
X
Foldable
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Foldable
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Foldable
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Practice problemsTeacher led
PartnersAlternate problems with calculations
One student calculates the problem & then explains how she/he did it to the other student.
(Why? The process of explaining helps you in gaining and retaining the information.)
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NO + O₂→ NO₂
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NO O₂ NO₂
# moles
Molar mass
CS₂ + O₂→ CO₂ + SO₂
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CS₂ O₂ CO₂ SO₂
# moles
Molar mass (g)
Review: Gram to Gram Calculation 1H₂SO₄+ 2NaOH→ 1Na₂SO₄+ 2H₂0
• If 540 grams of sodium hydroxide are available, how many grams of sulfuric acid must be used?
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Percent Yield
• Stoichiometry calculations always give the maximum amount that can be produced.This is called the _________ ________.
• In real life, the maximum amount is never produced. Reactions do not proceed perfectly. The _________ ________
is produced.
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Percent Yield
• Percent yield: Actual Yield x 100 = % Theoretical Yield
• In the last stoichiometry problem, 661.5 grams of sulfuric acid was calculated. However, the sample was weighed and found to
be 650.7 grams. The percent yield is: ______________ x 100 = %
Note: the % yield is always less than 100%
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Analysis of Chemical Reaction problems
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Putting all the steps together in a stoichiometry calculation
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Putting all the steps together in a stoichiometry calculation
• Propane (C₃H₈) reacts with oxygen to produce carbon dioxide and water vapor.
• Balanced equation:
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Example 1:
• How many moles of oxygen are required to completely react 10 moles of propane?
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Example 1: • How many moles of oxygen are required to
completely react 10 moles of propane?
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Example 2: • How many grams of oxygen are required to
completely react 10 moles of propane?
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Molar mass of oxygen:
Example 3:
• How many liters of oxygen are required to completely react 10 moles of propane? Given:
Amount & Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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1 mole of oxygen at STP = ____________ liters
Magnesium reacts with hydrochloric acid to yield magnesium chloride and
hydrogen gas.
• Balanced equation:
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Example 4: • How many moles of magnesium chloride will be produced if a
chemist starts with 120 grams of magnesium metal and plenty* of hydrochloric acid?
*Chemistry language: “with an excess of hydrochloric acid”
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Molar mass of magnesium:
Example 5: • How many grams of magnesium chloride will be produced if a
chemist starts with 60 grams of magnesium metal and an excess of hydrochloric acid?
Given: Amount &
Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Molar mass of magnesium: Molar mass of magnesium chloride:
Example 6: • How many liters of Hydrogen gas will be produced
with 60 grams of hydrochloric acid and an excess of magnesium? Given:
Amount & Unit
Do I need to convert the
given to moles?
Mole Ratio Do I need to convert from
moles to another unit?
Unknown:Unit
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Molar mass of hydrochloric acid: 1 mole of hydrogen gas at STP:
Manufacturing Sulfuric Acid
Using stoichiometry in an industrial application
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Here is a typical problem:• Sulfuric acid, an important chemical in
industry, is manufactured and sold by XYZ company.
• Sulfur dioxide gas is combined with water and oxygen to make H₂SO₄.
• The company is expecting a shipment of 500 kg of SO₂ and wants to know how much H₂SO₄ can be made from this shipment.
What are the steps to determine the amount of sulfuric acid?
1.
2.
3.
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Determining sales value
• They can then calculate how much money they will make from the sale of their sulfuric acid.
• Water and oxygen are readily available and cheap, so the company uses an EXCESS of these substances, which means they use more than enough to react with the SO₂.
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Sales
• If you can sell sulfuric acid for $10 per kg, how much will be the total sales ($)?
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