Bell Ringer
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Transcript of Bell Ringer
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Bell RingerAluminum + Sulfuric Acid Aluminum Sulfate + Hydrogen Gas
Which of the following is the balanced chemical equation for the reaction shown above?
A Al + H2SO4 Al2(SO4)3 + H2B 2Al + 3H2SO4 Al2(SO4)3 + 3H2C 2Al + 3H2SO4 Al2(SO4)3 + H2
D 2Al + H2SO4 Al2(SO4)3 + H2 2004 SOL
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Nerf & Poof Factor MethodCONVERSION FACTORS:
1 nerf = 3 poof 5 splunk = 6 mews
2 poof = 7 splat 2 pock = 3 splunk
4 trad = 1 pock 8 splat = 3 trad
1. 6 nerf = ? trad
2. 3.6 mews = ? pock
3. 7 poof = ? nerf
4. 3 mol Na2P = ?atoms Na
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Chocolate Chip Cookies• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
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Chocolate Chip Cookies• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
How much?
What units?
Of what?
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Chocolate Chip Cookies• 2.25 flour• 8 butter• 0.5 shortening• 0.75 sugar• 0.75 brown sugar• 1 salt• 1 baking soda• 1 vanilla• 0.5 Egg Beaters
How much?
Of what?
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Chocolate Chip Cookies• 2.25 cups • 8 Tbsp• 0.5 cups • 0.75 cups • 0.75 cups• 1 tsp • 1 tsp• 1 tsp• 0.5 cups
How much?
What units?
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Chocolate Chip Cookies• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
How much?
What units?
Of what?
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Get on with it!
What does this have to do with CHEMISTRY?
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2.25 cups flour + 8 Tbsp butter + 0.5 cups shortening +
0.75 cups sugar + 0.75 cups brown sugar + 1 tsp salt +
1 tsp baking soda + 1 tsp vanilla + 0.5 cups Egg Beaters
(a synthesis reaction)
(177ºC)
1 batch of chocolate chip cookies!
coefficient
unit substance
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Welcome to STOICHIOMETRY
Mr. Trotts
2008
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What is Stoichiometry?• The study of quantitative relationships
within chemical reactions
• A balanced equation is the key to stoichiometry!
• Tools you’ll need for this chapter:– Writing proper formulas and balanced
reactions– Converting from mass to moles and vice
versa
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Let’s Revisit the Cookies…
• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
For 1 batch: The Egg Beaters I have are close to expiring! I’d like to use the rest of them in this recipe. I have 1.5 cups of Egg Beaters.
How many batches of cookies can I make with that many Egg Beaters?
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Let’s Revisit the Cookies…
• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
For 1 batch: I have 1.5 cups of Egg Beaters.
How many batches of cookies can I make with that many Egg Beaters?
1.5 cups E.B. x1 batch cookies
0.5 cups E.B.=
3.0 batches of cookies
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Let’s Revisit the Cookies…
• 2.25 cups flour• 8 Tbsp butter• 0.5 cups shortening• 0.75 cups sugar• 0.75 cups brown sugar• 1 tsp salt• 1 tsp baking soda• 1 tsp vanilla• 0.5 cups Egg Beaters
For 1 batch: I have 1.5 cups of Egg Beaters.
How much butter do I need to deplete (use up) the Egg Beaters?
1.5 cups E.B. x8 Tbsp butter
0.5 cups E.B.=
24 Tablespoons of butter
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… Back to Chemistry• There are three types of stoichiometry
problems we will deal with today:– Mole-Mole problems (1 conversion)– Mass-Mole problems (2 conversions)– Mass-Mass problems (3 conversions)
given required
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• Step 1: Write a BALANCED EQUATION
• Step 2: Determine the mole ratio from the coefficients in the equation.– Mole ratio = moles of required substance
moles of given substance
• Step 3: Set up the problem like a unit conversion and solve!
Baby Steps… Mole-Mole Problems
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Mole-Mole ProblemsExample:
2 H2 + O22 H2O
How many moles of water can be formed from 0.5 mol H2?
0.5 mol H2 x2 mol H2
2 mol H2O = 0.5 mol H2O
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Mole-Mole Practice
CuSO4 Al Al2(SO4)3 Cu3 2 3+ +
1. a. 0.5 mol Al 3 mol CuSO4
2 mol Al=x 0.8 mol CuSO4
b.
c.
0.5 mol Al 1 mol Al2(SO4)3
2 mol Al=x 0.3 mol Al2(SO4)3
0.5 mol Al 3 mol Cu
2 mol Al=x 0.8 mol Cu
Mole ratio
0.5 mol? mol ? mol ? mol
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#2) Ca + AlCl3 CaCl2 + Al
1. Balance the formula
2. Given 2.5 moles Ca find the number of moles of AlCl3, CaCl2, and Al needed.
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Mole-Mole Practice
2. a. 2.5 mol Ca 2 mol AlCl3
3 mol Ca=x 1.7 mol AlCl3
b.
c.
2.5 mol Ca 3 mol CaCl2
3 mol Ca=x 2.5 mol CaCl2
2.5 mol Ca 2 mol Al
3 mol Ca=x 1.7 mol Al
Ca AlCl3 CaCl2 Al3 2 2+ +3
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• complete the mole to mole worksheet Do not write on the handout!!
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Quiz: mole to mole
• 5 moles of Ca(OH)2 is added to a container of HCl in an attempt to neutralize the acid. How many moles of the HCl will be neutralized as CaCl2 and water are produced? Show your work for credit to include the molar ratio.
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Mass-Mole Problems
• Step 1: Write a BALANCED EQUATION
• Step 2: Calculate the molar mass of your given substance and convert from mass to moles
• Step 3: Determine the mole ratio from the coefficients in the equation
• Step 4: Set up the conversion and solve!
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Mass-Mole ProblemsExample:
2 H2 + O22 H2O
How many moles of water can be formed from 48.0 g O2?
48.0 g O2 x1 mol O2
2 mol H2O = 3.00 mol H2O
32.00 g O2
1 mol O2 x
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Mass-Mole Practice
CuSO4 Al Al2(SO4)3 Cu3 2 3+ +
3a. 13.5 g Al 1 mol Al
26.98 g Al=x 0.751 mol
CuSO4
b.
c.
13.5 g Al 1 mol Al2(SO4)3
2 mol Al=x 0.250 mol
Al2(SO4)3
13.5 g Al 3 mol Cu
2 mol Al=x 0.751 mol
Cu
Mole ratio
x3 mol CuSO4
2 mol Al
1 mol Al
26.98 g Alx
1 mol Al
26.98 g Alx
13.5 g? mol ? mol ? mol
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#4 Ca + AlCl3 CaCl2 + Al
1. Balance the equation
2. Given 5.7 g of Calcium find the number of moles of AlCl3, CaCl2, and Al
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Mass-Mole Practice
4. a. 5.7 g Ca 2 mol AlCl3
3 mol Ca=x 0.095 mol AlCl3
b.
c.
5.7 g Ca 3 mol CaCl2
3 mol Ca=x 0.14 mol CaCl2
5.7 g Ca 2 mol Al
3 mol Ca=x 0.095 mol Al
Ca AlCl3 CaCl2 Al3 2 2+ +
1 mol Ca x
x
x
40.08 g Ca
1 mol Ca
40.08 g Ca
1 mol Ca
40.08 g Ca
3
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Mass-Mass Problems
Example:
2 H2 + O22 H2O
How many grams of water can be formed from 48.0 g O2?
48.0 g O2 x1 mol O2
2 mol H2O =32.00 g O2
1 mol O2 x x18.02 g H2O
1 mol H2O54.1 g H2O
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Mass-Mass Practice
CuSO4 Al Al2(SO4)3 Cu3 2 3+ +
5. a. 8.5 g Al 1 mol Al
26.98 g Al=x
75 g CuSO4
b. 8.5 g Al 1 mol Al2(SO4)3
2 mol Al=x
54 g Al2(SO4)3
Mole ratio
x3 mol CuSO4
2 mol Al
1 mol Al
26.98 g Alx
1 mol CuSO4
342.14 g Al2(SO4)3
1 mol Al2(SO4)3
x
x
159.61 g CuSO4
8.5 g? g ? g ? g
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Mass-Mass Practicec. 8.5 g Al 3 mol Cu
2 mol Al=x
30. g Cu
1 mol Al
26.98 g Alx x 63.55 g Cu
1 mol Cu
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#6a. How many grams of aluminum chloride would be required to completely react with 1.9 grams of Calcium?
#6b. How many grams of Calcium chloride will be produced from 1.9 grams of Calcium?
#6c. How many grams of Aluminum will be produced from 1.9 grams of Calcium?
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Mass-Mass Practice
6. a. 1.9 g Ca 2 mol AlCl3
3 mol Ca=x
4.2 g AlCl3
b. 1.9 g Ca 3 mol CaCl2
3 mol Ca=x
5.3 g CaCl2
Ca AlCl3 CaCl2 Al3 2 2+ +
1 mol Ca x
x
40.08 g Ca
1 mol Ca
40.08 g Ca
x 133.33 g AlCl3
1 mol AlCl3
x1 mol CaCl2
110.98 g CaCl2
3
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Mass-Mass Practice
c. 1.9 g Ca 2 mol Al
3 mol Ca=x
0.85 g Al
x1 mol Ca
40.08 g Ca 1 mol Al
26.98 g Alx
Ca AlCl3 CaCl2 Al3 2 2+ +3
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• Now complete the Mass to Mass handout Do not write on the handout
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Quiz
7. 7.5 moles of potassium phosphate is reacted with excess barium chloride. How many grams of potassium chloride are produced in the reaction?
Write a balanced equation
Use the equation and molar ratios to solve the problem