Transcript Mole-Mass and Mole-Volume Relationships


Section 10.2
Mole-Mass & Mole-Volume
Relationships
Last time we talked about..
What is a Mole?
Last time we talked about..
What is Avogadro’s number?
Last time we talked about..
What are representative particles?
Last time we talked about..
Count-Mole Relationship
Convert number of particles
NA
moles
Different definitions for masses
•
Gram atomic mass (gam)
looking at the mass of individual atoms eg. Fe, Mg
•
Gram molecular mass (gmm)
Looking at the mass of molecular compounds eg. CO2, N2, C3H8
•
Gram formula mass (gfm)
Looking at the mass of ionic compounds eg. NaCl, KBr
Last time we talked about..
To simplify (yay!) we have a term that combines all 3:
Molar mass – the mass (in grams) of one mole of a substance
Because this term is broad, we need to be specific in what we are talking
about:
Ex. What is the molar mass of oxygen?
Are we talking about molecular oxygen ( O2 )? or atomic Oxygen (O)?
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1 mole Oxygen atoms = 16.00 g O
1 mole O2 molecules = 2 (16.00g) = 32.00g O
We will use (gam) (gmm) or (gfm) instead of molar mass only if we have
a situation like this
Mass – Mole Relationship
Mass is an easy way to measure quantity of matter, but in chemical
reactions, it is often important to consider the number of atoms of
each element present in a sample.
Demo Problem
How many grams are in 9.45 mol of dinitrogen trioxide?
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Is this compound ionic, molecular, or an acid?
 Molecular (you can tell by the prefixes)
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What is the formula?
 N2 O 3
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List the Knowns & Unknowns in your problem
 Known: 9.45 moles N2 O3
 Molar mass of N2 O3 = ?
 1 mol N2O3 = 2(14.01 g N) + 3 (16.00 g O) = 76.02g N2 O3
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Solve for the unknown (use dimensional analysis)
• 9.45 mol N2 O3 (76.02g N2 O3 /1.00 mol N2 O3) = 718.389 g N2O3
• 718 g N2 O3
Practice Problem
How many moles are in 92.2 g of Iron (III) Oxide?
 Is this a molecular compound, ionic compound, or acid?
 Ionic compound with a transition metal cation
 What is the formula?
 Fe2 O3
 List the knowns and unknowns in your problem
 Given mass Fe2 O3 = 92.2 g
 1.00 mole Fe2 O3 = 2(55.85g Fe) + 3(16.00gO) = 159.70 g Fe2 O3
 Solve for the Unknown
 92.2 g Fe2 O3 (1.00 mol Fe2 O3 /159.70 g Fe2 O3 )
 = 0.57733 mol Fe2 O3 = 0.577 mol Fe2 O3
Volume – Mole Relationship
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The volumes of one mole of different solids and liquids are not
the same
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1 mole glucose molecules = 180.18 g glucose
1 mole water molecules = 18.02 g water
1 mole paradichlorobenzene molecules = 147.00 g
paradichlorobenzene
The volumes of moles of gas are much more predictable if they
are under the same conditions
Standard temperature and pressure (STP)
 The volume of a gas changes with
temperature and pressure – so we
need a standard reference
 Standard temperature and
pressure (STP)
◦ Temperature = 0o C
◦ Standard Pressure = 101.3 kPa = 1
atmosphere(atm)
 At STP: 1 mole of any gas occupies
a volume of 22.4 L
 This is known as the molar volume
of a gas and is measured at STP
Recall..
1 mol of any substance contains 6.02 x 1023 representative particles
So…
22.4 L of any gas contains 6.02 x 1023 representative particles of that gas.
Does this mean 22.4 L of all gases at STP should have the same mass?
NO. Mass is still measured using molar mass, and 1 mole of each substance
has a different mass.
Demo Problem
What is the volume (in Liters) of 0.60 mol SO2 gas at STP?
 List the knowns and unknowns
 0.60 mol SO2
 1 mol SO2 = 22.4 L SO2
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volume = ? L
 Solve for the unknown
 0.60 mol SO2 (22.4 L SO2 )/1 mol SO2
 13.44 L SO2 = 13 L SO2
Density of gas
 The density of gas is usually measured in grams per Liter (g/L)
 If you are given the density of a gas at STP, you can calculate the
molar mass of that gas using the conversion factor
1 mol = 22.4 L
Demo Problem
The density of a gaseous compound containing Carbon and Oxygen is
1.964 g/L at STP. Determine the molar mass of the compound.
 Density = 1.964 g/L
 1 mol (gas at STP) = 22.4 L
 Convert g/L to g/mol
 1.964 g/1.00L (22.4 L/1.00 mol)
 = 43.9936 g/mol = 44.0 g/mol
The mole road map
We can use the mole to convert between particles, mass, and
volume of gas at STP.
The mole is the mediator between any of these.
So what is the mole road map?
Mole Road Map
Using the Mole Map..
Find the following..
1.
2.
3.
The mass, in grams of
1.
3.32 mol K
2.
2.50 mol iron (II) hydroxide
The number of moles in
1.
3.70 x 10-1 g TiO2
2.
75.0 g Nitrogen gas
What is the volume at STP of these gases?
1.
3.20 x 10-3 mol CO2
Practice Problem
What is the density of krypton gas at STP?
(hint: assume you have one mole of the gas!)