Unit 6 Note Packet
What is a mole?
What is a mole?
Why does it need to be so big?
-Atoms are
How do we measure a mole?
By the ____________,
It is still ________________________ atoms though
Summary
Calculating Molar Mass
What is Molar mass?
-The mass of ____________ of a substance
-It will be _____________ for _________ compound and element
-Is measured in ________________
-Calculated by adding the mass of each up in a compound or substance
What is the molar mass of Iron (III) Oxide
What is the molar mass of aluminum sulfate?
What is the molar mass of copper (II) sulfate pentahydrate?
Summary
Molar Conversions, 1-step
What are the conversion factors of the mole?
Convert 6.3 grams of carbon dioxide to moles
Convert 3.2 x 10-6 mol of diphosphorus pentoxide to grams
Convert 6.92 x 10 25 atoms of Iron to moles
Convert 0.025 moles of chickens to particles
Convert 16 liters of carbon dioxide to moles at STP
Convert 5.3 x 10 -4 moles of Oxygen gas to liters at STP
Summary
Molar Conversions, 2-step
Conversion Factors
- x grams=1 mol
-6.02 x 10 23 particles= 1 mol
-22.4 Liters=1 mol
When doing these conversions you will go through the mole
Convert 4.6 grams of chlorine gas to liters
Convert 35.1 L of Helium to atoms of Helium
Convert 1 molecule of dinitrogen pentoxide to grams
Summary
Percent Composition
What is the Percent composition?
What is the formula for percent composition?
Find the percent composition of copper (I) sulfide
Find the percent of calcium in calcium phosphate
How many grams of copper do you have when you have 28 grams of copper (I)
sulfide?
Summary
Empirical Formula
What is an empirical formula?
How to get an empirical formula?
1) % to mass
2) Mass to mole
3)Divide by small
4) Times til whole
Find the empirical formula for a sample of 25.9% N and 74.1% O
What is the empirical formula when you have 6.256 grams of
Carbon, 1.392 grams of Hydrogen, and 8.352 grams of Oxygen
Summary
Molecular Formula
What is the molecular formula?
How do you get the molecular formula?
1. Find the empirical formula.
2. Find the empirical formula mass.
3. Divide the molecular mass by the empirical mass.
4. Multiply each subscript by the answer from step 3
Which of the following molecular formulas are also empirical formulas?
What is the empirical formula if not?
C5H10O5
C6H12O2
C55H72MgN4O5
C12H17ON
Determine the molecular formula for a compound that has a molar mass of 34
grams and is and is 94.1% Oxygen and 5.9%Hydrogen
A Chemical contains 43.64% P and 56.36% O. The compound has a molar
mass of 283.9 g/mol. What is the empirical formula and molecular formula?
Summary