U4 One Step Conversions
Download
Report
Transcript U4 One Step Conversions
U4 One Step
Stoichiometry
Problems
Chemistry Ms. Boon 10.10-10.11
Catalyst
Pick up the notes handout and answer the
following question at the top of the page:
10 weeks have passed since the first day of
school. How many days have passed? How
do you know?
7 days = 1 week
10 weeks
X
7 days =
1 week
70 days
Objective
I can perform one-step stoichiometry
conversions using a worksheet, notes, and a
puzzle.
I can show my work and use units in all my
calculations.
Mini Review: What is the mole?
The mole is a number we use to make counting
atoms, ions, and molecules much easier. The
mole allows scientists to count by weighing.
Think, Pair, Share: What is counting by weighing?
Imagine you work at a candy store and a customer asks
for 500 jelly beans. There is a long line and you do not
want to count 500 beans. But you have a scale. What
can you do?
Answer: Find the weight of one bean. Then multiply by
500. Finally, measure this mass of beans and it should
be 500 beans.
Mini Review: What is the mole?
1 mole = 6.02 x 1023 particles. This
does not change.
The number of particles in 1 mole is
called Avogadro’s number
THE MOLE -- Why?
Why is the mole useful to us as chemists??
Make a dot on your paper with your pencil.
Guess how many atoms of Carbon graphite are in
that dot.
25 million atoms in that tiny dot!
Mini Review: What is the mole?
Molar mass and molecular weight are the mass in grams
of one mole of an element or compound.
Different elements and compounds have different molar
masses or molecular weights.
Example 1: What is the
molar mass of aluminum?
Hint: The molar mass is the
same as the atomic mass,
just add “g” for grams.
Example 2: What is the
molecular weight of baking
soda? Hint: First find the
mass of each element, then
multiply by subscripts, then
add up the answers.
Answer 26.98 g/mol
Answer NaHCO3 = 84 g/mol
Mini Review: What is the mole?
Example 2: What is the molecular weight of baking
soda? Hint: First find the mass of each element, then
multiply by subscripts, then add up the answers.
Answer NaHCO3 = 84 g/mol
23 g
x1
23 g
+
1g
x1
1g
+
12 g
x1
12 g
+
16 g
x3
48 g
= 84 g/mol
5 minute - Quick Practice: Choose at least 2 molar
mass/molecular weight problems from your worksheet.
Stoichiometry Conversions Part 1: Grams to
Moles and Moles to Grams.
Calculating the molar mass or molecular weight of a chemical reveals the mass
of one mole of that chemical. What if we are given more than one mole of a
substance? Or some random amount in grams? Use the molar mass or
molecular weight as a conversion factor to move between moles and grams.
Ex 1: Moles to Grams. How
many moles is 24 g of
carbon?
Ex 2: Grams to Moles. How
many grams is 10 moles of
Gold?
Given: 24 g
Given: 10 mol
Unknown: # moles
Unknown: # g
Conversion: 1 mol/12 g
Conversion: 197g/1 mol
Set up: 24 g x 1 mol =
Set up: 10 mol x 197 g =
12 g
1 mol
Answer: 2 mol
Answer: 1970 g
5 minute - Quick Practice: Choose at least 2 gram to mole
or mole to gram problems from your worksheet.
Stoichiometry Conversions Part 2: Particles to
Moles and Moles to Particles.
Avogadro’s number allows us to determine the number of atoms, molecules,
or ions (generally particles) in a given sample. Use 1 mole = 6.02 x 1023 as
a conversion factor to move between moles and particles.
Ex 1: Particles to Moles. How many moles is 1.20 x 1024 atoms
of carbon?
Given: 1.20 x 1024 atoms
Unknown: # moles
Conversion: 1 mol/6.02 x 1023 atoms
Set up: 1.20 x 1024 atoms x 1 mol =
6.02 x 1023 atoms
Answer: 2 mol
Stoichiometry Conversions Part 2: Particles to
Moles and Moles to Particles.
Avogadro’s number allows us to determine the number of atoms, molecules,
or ions (generally particles) in a given sample. Use 1 mole = 6.02 x 1023 as
a conversion factor to move between moles and particles.
Ex 2: Moles to Particles. How many atoms is 10 moles of
Gold?
Given: 10 mol
Unknown: # atoms
Conversion: 6.02 x 1023 /1 mol
Set up: 10 mol x 6.02 x 1023 atoms=
1 mol
Answer: 6.02 x 1024 atoms
5 minute - Quick Practice: Choose at least 2 particle
conversion problems from your worksheet.
Extra Special Bonus: Video Review –
Super Hero Science
How does the law of conservation of mass limit the size
of a super hero?
http://www.youtube.com/watch?v=fpV7DKwcqbk&list=P
LJicmE8fK0EjcBM04Tz0UvUTJ3utyYD1G
More Practice
See textbook p. 224-233
Try the sample problems on p. 228 and 229