Date post: | 13-Dec-2015 |
Category: |
Documents |
Upload: | alan-chase |
View: | 223 times |
Download: | 1 times |
Stoichiometry
Calculations based on a balanced chemical equation
Chapter 9 (12)
Why do I need to know about stoichiometry?
Sample recipe for 1 loaf of bread:8 cups flour1 cup sugar2 cups milk1.5 cups eggs1/2 cup of butter1/8 cup yeast
How many loaves of bread can be made
from: • 3 cups eggs
2 loaves • 1 cup
milk 1/2 loaf
• 6 cup flour 3/4 loaf
Example using stoichiometry:
8 Fl + 1 S + 2 M + 1.5 E + 1/2 B + 1/8 Y => 1 Lf
“Chemical Equation” for bread recipe:
Sample recipe for 1 loaf of bread:8 cups flour1 cup sugar2 cups milk1.5 cups eggs1/2 cup of butter1/8 cup yeast
Review of Balancing Equations
KClO3 --> KCl + O2322
What do the coefficients mean?
a) Molecules
“2 molecules KClO3 produces 3 molecules of O2”
Review of Balancing Equations
KClO3 --> KCl + O2322
What do the coefficients mean?
a) Molecules
“2 molecules of KCl are formed when 3 molecules of O2 are formed”
Review of Balancing Equations
KClO3 => KCl + O2322
What do the coefficients mean?
b) Moles
“2 moles of KCl are formed when 3 moles of O2 are formed”
Review of Balancing Equations
KClO3 => KCl + O2322
What do the coefficients mean?
b) Moles
“2 moles of KCl are formed when 2 moles of KClO3 are decomposed”
In the following reaction how many moles of PbCl2 are formed if 5.000 moles of NaCl react? 2 NaCl + Pb(NO3)2 PbCl2 + 2 NaNO3
5.000 moles NaCl
2 moles NaCl
1 moles PbCl2 =
2.500 moles PbCl2
In the following reaction how many moles of NH3
are formed if 4.0 moles of H2 react? N2 + 3 H2 => 2 NH3
4.0 moles H2
3 moles H2
2 moles NH3 =
2.7 moles NH3
Complete Problems 1-5 on the practice page.
In the following reaction how many grams of NH3
are formed if 4.00 moles of H2 react? N2 + 3 H2 => 2 NH3
4.00 moles H2
3 moles H2
2 moles NH3 =
45.3 g NH3
1 moles NH3
17 g NH3
Grams A
Moles A Moles B
Grams B
1 1
coefficients
mw mw
In the following reaction how many moles of NH3
are formed if 10.0 grams of H2 react? N2 + 3 H2 => 2 NH3
10.0 grams H2
2.016 g H2
1 moles H2 =
3.31 mol NH3
3 moles H2
2 mole NH3
Complete Problems 6-10 on the practice page.
Grams A
Moles A Moles B
Grams B
1 1
coefficients
mw mw
In the following reaction how many grams of NH3
are formed if 25.0 grams of N2 react? N2 + 3 H2 => 2 NH3
25.0 g N2
28.02 g N2
1 moles N2 =
30.3 g NH3
1 moles N2
2 mole NH3
Grams A
Moles A Moles B
Grams B
1 1
coefficients
mw mw
1 mole NH3 17 g NH3
Complete Problems 10-15 on the practice page.
How many grams of NH3 are formed if 25.0 grams of N2 react with 10.0 g of H2? N2 + 3 H2 => 2 NH3
25.0 g N2
28.02 g N2
1 moles N2 =
30.3 g NH3
1 moles N2
2 mole NH3
1 mole NH3 17 g NH3
10.0 grams H2
2 g H2
1 moles H2
=
3 moles H2
2 mole NH3
1 mole NH3
17 g NH3
56.7 g NH3
(Solve the problem separately with each number)
(The smaller answer is the only correct one)56.7 g NH3
Complete problems 16-20.
How many grams of NH3 are formed if 25.0 grams of N2 react with 10.0 g of H2? N2 + 3 H2 => 2 NH3
25.0 g N2
28.02 g N2
1 moles N2 =
30.3 g NH3
1 moles N2
2 mole NH3
1 mole NH3 17 g NH3
10.0 grams H2
2 g H2
1 moles H2
=
3 moles H2
2 mole NH3
1 mole NH3
17 g NH3
56.7 g NH3 56.7 g NH3
How much of the excess reagent is left over?
How many grams of H2 (the excess reagent) are required to react with 25.0 g of N2 (the limiting reagent) ? N2 + 3 H2 => 2 NH3 25.0 g N2
28 g N2
1 moles N2 =
5.36 g H2
1 moles N2
3 mole H2
1 mole H2 2 g H2
REQUIRED
Left over = Given amount – Required amount = 10.0 g H2 - 5.36 g H2
= 4.64 g H2
How many grams of NH3 are formed if 10.0 grams of N2 react with 15.0 g of H2?
How much of the excess reagent is left over?
N2 + 3 H2 => 2 NH3
Percent Yield Calculations
Terms:
Theoretical Yield = the CALCULATED amount of product expected
Actual Yield = the EXPERIMENTAL amount that was actually obtained
% Yield =
Actual
TheoreticalX 100
What is the percent yield in a reaction where 1.50 mol of NH3 was obtained after reacting 10.0 g of H2 with excess nitrogen? N2 + 3 H2 => 2 NH3
10.0 grams H2
2.016 g H2
1 moles H2 =
3.31 mol NH3
3 moles H2
2 mole NH3
Theoretical Yield
% yield = 1.50
3.31X 100 = 45.3%