ch 2 matter & atoms
DESCRIPTION
Ch 2 Matter & Atoms. Natural Approach to Chemistry Lab Aids Condensed. 2.1 Frames 2-282.2 Frames 29-62 2.3 Fr. 63-106. 2.1 Matter & the Elements. Standards: SC.912.P.8.5 relate properties of atoms & their position in the periodic table to the arrangement of their electrons - PowerPoint PPT PresentationTRANSCRIPT
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Ch 2 Matter & Atoms
Natural Approach to ChemistryLab Aids
Condensed
2.1 Frames 2-28 2.2 Frames 29-62 2.3 Fr. 63-106
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2.1 Matter & the Elements
• Standards:• SC.912.P.8.5 relate properties of atoms & their
position in the periodic table to the arrangement of their electrons
• SC.912.P.8.9 apply the mole concept and the law of conservation of mass to calculate quantities of chemicals participating in reactions
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The “stuff” that we are made of is called matter.
Chemistry tells us how one kind of matter can be changed into a completely different kind of matter.
What are things made of?
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substance: a kind of matter that can’t be separated into other substances by physical means such as heating, cooling, filtering, drying, sorting, or dissolving.
Corn oil is a pure substance
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mixture: matter that contains more than one substance.
Corn oil is a pure substance
Oil and vinegar dressing is a mixture of substances
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Examples: MassDensityColor
Physical properties can be measured or seen through direct observations.
Physical properties
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Physical changes include changes in shape, phase or temperature.
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Chemical properties are observed when a substance changes into a different substance.
Iron RustChemical change
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Signs that a
chemical change has occurred
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Each element is a unique type of atom.
All oxygen atoms are identical.
An oxygen atom is different from a silicon atom or a potassium atom.
element: a substance that cannot be separated into simpler substances by chemical means.
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1 grain of rice = 0.01 gram
1 hydrogen atom = 1.678 x 10–24 grams
= 0.000000000000000000000001678 grams
How small is an atom?
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The periodic table
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The periodic table organizes elements according to how they combine with other elements (based on their chemical properties).
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HydrogenLightest elementAtomic number: 1
UraniumHeaviest naturally occurring elementAtomic number: 92
Increasing atomic number
Incr
easin
g at
omic
num
ber
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Elements that belong to the same group (column) have similar chemical properties.
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Reminder
1 atomic mass unit (amu) = 1.66 x 10-24 g
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The atomic mass is the mass of:
1) a single atom in amu.
2) a mole of atoms in grams.
One single hydrogen atom weighs 1.01 amu.
One mole of hydrogen atoms weighs 1.01 g.
What does that mean?
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The atomic mass is the mass of:
1) a single atom in amu.
2) a mole of atoms in grams.
One single carbon atom weighs 12.0 amu.
One mole of carbon atoms weighs 12.0 g.
What does that mean?
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One mole contains 6.02 x 1023 atoms
Avogadro’s number
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How many moles are in 100 g of sulfur (S)?
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How many moles are in 100 g of sulfur (S)?
Asked: The number of molesGiven: The element is sulfur and there are 100 gRelationships: One mole of sulfur has a mass of 32.065 g
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How many moles are in 100 g of sulfur (S)?
Asked: The number of molesGiven: The element is sulfur and there are 100 gRelationships: One mole of sulfur has a mass of 32.065 g
Solve:
Answer: 100 g of sulfur contains 3.12 moles of sulfur atoms.
110032.065
3.12mole Sg Sg S
moles S
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How many grams of calcium (Ca) do you need to have 2.50 moles of calcium?
Asked: The number of gramsGiven: The element is calcium and there are 2.50 molesRelationships: One mole of calcium has a mass of 40.078 g
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How many grams of calcium (Ca) do you need to have 2.50 moles of calcium?
Asked: The number of gramsGiven: The element is calcium and there are 2.50 molesRelationships: One mole of calcium has a mass of 40.078 g
Solve:
Answer: 2.50 moles of calcium has a mass of 100. g.
40.0782.501
100.2g Camoles Camole Ca
g Ca
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Physical properties can be seen and measured
Chemical properties are observed when one substance is changed into another
Elements are organized in a periodic table This allows to convert
grams to moles and vice versa.
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2.2 Molecules and Compounds
Sc.912.P.8.7 interpret formula representations of molecules and compounds in terms of composition and structure.Sc.912.P.8.9 mole concept and law of conservation of mass
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One H2 moleculeOne O2 molecule
molecule: a group of atoms chemically bonded together.
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molecule: a group of atoms chemically bonded together.
compound: a substance containing more than one element in which atoms of different elements are chemically bonded together.
One H2O moleculeOne H2 moleculeOne O2 molecule
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What do all these have in common?
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What do all these have in common?
They are made up of only 3 types of atoms: carbon, oxygen and hydrogen.
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More than 200,000 words in the English language
Trillions of substances that make up the universe
The alphabet of chemistry
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The chemical formula
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The chemical formula
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Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N).
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Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N).
Asked: Chemical formulaGiven: 3 hydrogen (H) and 1 nitrogen (N)Relationships: The subscript tells the number of each element in the
compound.
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Write a chemical formula for a compound that has three hydrogen (H) atoms for each atom of nitrogen (N).
Asked: Chemical formulaGiven: 3 hydrogen (H) and 1 nitrogen (N)Relationships: The subscript tells the number of each element in the
compound.Answer: NH3
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The properties of a compound depend more on the exact structure of the molecule
than on the individual elements from which it is made.
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F
U
N
E
RA
L
F U N E R A L F U NER A L
The arrangement of letters matters!
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The arrangement of atoms matters!
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Representation
There are many ways of representing the same thing.
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Representation
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Ionic compounds
Salt (NaCl) is not a molecule!
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ionic compound: a compound such as a salt in which positive and negative ions attract each other to keep matter together.
ion: an atom or small molecule with an overall positive or negative chare as a result of an imbalance of protons and electrons.
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Formula mass
The formula mass of water (H2O) is 18 g.
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What is the mass of 1 mole of methane (CH4)?
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What is the mass of 1 mole of methane (CH4)?
Asked: The mass of 1 mole of methane
Given: Methane (CH4) contains 1 carbon (C) and 4 hydrogen (H) atoms
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound
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What is the mass of 1 mole of methane (CH4)?
Asked: The mass of 1 mole of methane
Given: Methane (CH4) contains 1 carbon (C) and 4 hydrogen (H) atoms
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound
Solve:
Answer: One mole of methane (CH4) has a mass of 16.04 g. 44 4 1.0079 12.0 16.0411 g CH
moH
eC
l
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How many moles are in 100 grams of water (H2O)?
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How many moles are in 100 grams of water (H2O)?
Asked: The moles in 100 g of water
Given: Water (H2O) contains 2 hydrogen (H) atoms and 1 oxygen (O)
atom.
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.
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How many moles are in 100 grams of water (H2O)?
Asked: The moles in 100 g of water
Given: Water (H2O) contains 2 hydrogen (H) atoms and 1 oxygen (O)
atom.
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.
Solve:
Answer: 100 g of water (H2O) contains 5.55 moles.
2
5
2 2 1.0079 15.999 18.015
110018.01
55
. 5
gH O H Omole
molegg
moles
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How many grams are in 2.300 moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter.
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How many grams are in 2.300 moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter.
Asked: The mass in grams of 2.300 moles of butane
Given: 2.300 moles of C4H10
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.
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How many grams are in 2.300 moles of butane (C4H10)? Butane is used as a lighter fluid in disposal lighter.
Asked: The mass in grams of 2.300 moles of butane
Given: 2.300 moles of C4H10
Relationships: The formula mass is the sum of the atomic masses for each atom in the compound.
Solve:
Answer: 133.7 g are in 2.300 moles of butane (C4H10).
4 1
2
4 10
00
4 1
4 10 4 12.011 10 1.0079 58.12
133.7
3
58.1232.300
1
gH O H Omole
g C Hgmo
gle mole C
C HH
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How many oxygen atoms are in 200.0 g of glucose (C6H12O6)?
Asked: Number of oxygen atoms
Given: 200.0 g of C6H12O6
Relationships: Formula mass of glucose:
6 12 6
6 12.011 12 1.0079 6 15.9 19 80.159
C Og
m e
H
ol
Remember: Avogadro’s number indicates that one mole contains 6.02 x 1023 atoms
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Solve: First we find how many moles are in 200.0 g of glucose:
6 12 66 12 6
6 16 12 6
2 6
1200.0
180.1.11
150
mole C molesH O Cg C H Og H
H OC O
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Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose:
6 12 66 12 6 6 12 6
6 12 6
1200.0 1.110
180.15mole C H Og C H O moles C H O
g C H O
236 12
2
66 12 6
6 12 6
36 12 6
6.022 101.110
1
6.684 10
molecules C H Omoles C H
molecules
O
C
mole C
O
H O
H
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Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose:
Then we find how many O atoms are contained in 6.684 x 1023 molecules of glucose:
6 12 66 12 6 6 12 6
6 12 6
1200.0 1.110
180.15mole C H Og C H O moles C H O
g C H O
236 12 6
6 12 66 12 6
236 12 6
6.022 101.110
1
6.684 10
molecules C H Omoles C H Omole C H O
molecules C H O
236 12 6
6 1 6
24
2
4.66.684 101
010 10O atomsmolecules C H Omolecule C H O
O atoms
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Solve: First we find how many moles are in 200.0 g of glucose:
Next we find how many molecules are contained in 1.11 moles of glucose:
Then we find how many O atoms are contained in 6.684 x 1023 molecules of glucose:
Answer: There are 4.010 x 1024 atoms of O in 200.0 g of glucose (C6H12O6).
6 12 66 12 6 6 12 6
6 12 6
1200.0 1.110
180.15mole C H Og C H O moles C H O
g C H O
236 12 6
6 12 66 12 6
236 12 6
6.022 101.110
1
6.684 10
molecules C H Omoles C H Omole C H O
molecules C H O
236 12 6
6 1 6
24
2
4.66.684 101
010 10O atomsmolecules C H Omolecule C H O
O atoms
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We can build compounds using atoms- The type of atom matters
- The arrangement of atoms also matters
We can calculate the formula mass of compounds:
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2.3 Mixtures and Solutions
Sc.912.P.8.9 mole concept and law of conservation of massSc.912.P.12.12 explain how various factors such as concentration, temperature, and presence of a catalyst affect the rate of a chemical reaction
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CHAPTER 2
Matter and Atoms
2.3 Mixtures and Solutions
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A recipe calls for you to “mix until homogeneous.”
What does that mean?
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A mixture that is uniform throughout.
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A mixture that is uniform throughout. Different samples may have different compositions.
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What happens when sugar is added to water?
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What happens when sugar is added to water?
A solution is obtained.
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Is orange juice a solution?
Hint: Are things dissolved in orange juice?
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Is orange juice a solution?
It is partially a solution because some chemicals are dissolved in water, but some bits (like pulp) are not.
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These four solutions contain the same solvent and solute.
Which one is the most concentrated solution?Which one is the most dilute solution?
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concentration: the amount of each solute compared to the total solution.
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• Can you dissolve salt in water?
VariablesAmount of saltAmount of water
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• Can you dissolve salt in water?
• Can you continue adding more and more salt, and still get a solution?
Variables
Amount of saltAmount of water
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• Can you dissolve salt in water?
• Can you continue adding more and more salt, and still get a solution?
• Can you dissolve more salt when you increase the temperature?
Variables
Amount of saltAmount of water
Amount of saltAmount of waterTemperature
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solubility: the amount of a solute that will dissolve in a particular solvent at a particular temperature and pressure.
Solubility of common substances in water at 25oC
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If the concentration of a sugar solution is 75 g/L, how much solution do you need if you want 10 g of sugar?
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If the concentration of a sugar solution is 75 g/L, how much solution do you need if you want 10 g of sugar?
Asked: Volume of solution
Given: 10 g of solute and concentration of 75 g/L
Relationships:mass of soluteLiters of solution
concentration in g L
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If the concentration of a sugar solution is 75 g/L, how much solution do you need if you want 10 g of sugar?
Asked: Volume of solution
Given: 10 g of solute and concentration of 75 g/L
Relationships:
Solve:
mass of soluteLiters of solutionconcentration in g L
10 0.1 1333375
g L org
LL
m
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How much menthol do you need to make 10 kg of mouthwash if the concentration of menthol must be 0.05%?
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How much menthol do you need to make 10 kg of mouthwash if the concentration of menthol must be 0.05%?
Asked: Mass of solute
Given: 10 kg of solution, solute concentration of 0.05%
Relationships: %100
concentration inmass of solute mass of solution
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How much menthol do you need to make 10 kg of mouthwash if the concentration of menthol must be 0.05%?
Asked: Mass of solute
Given: 10 kg of solution, solute concentration of 0.05%
Relationships:
Solve:
%100
concentration inmass of solute mass of solution
0.05%10 0.00510
50
kg kg or g
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molarity: the number of moles of solute per liter of solution.
( )( )
amount of solute moles molesmolarityvolume of solvent liters L
moles ML
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If 10.0 g of citric acid (C6H8O7) is added to 500 mL of water, what is the molarity of the resulting solution?
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Asked: The molarity of a solution
Given: The amount of solute (citric acid) and the volume of solution
Relationships:
moles solutemolarityvolume of solution L
If 10.0 g of citric acid (C6H8O7) is added to 500 mL of water, what is the molarity of the resulting solution?
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Asked: The molarity of a solution
Given: The amount of solute (citric acid) and the volume of solution
Relationships:
Solve: Start by calculating the formula mass of C6H8O7:
moles solutemolarity
volume of solution L
6 12.011 8 1.0079 7 1 192.5. 12999 g mole
If 10.0 g of citric acid (C6H8O7) is added to 500 mL of water, what is the molarity of the resulting solution?
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Asked: The molarity of a solution
Given: The amount of solute (citric acid) and the volume of solution
Relationships:
Solve: Start by calculating the formula mass of C6H8O7:
Next we calculate the number of moles in 10.0 g of C6H8O7:
moles solutemolarity
volume of solution L
6 12.011 8 1.0079 7 15.999 192.12 g mole
1# 10.0192.12
0.0521molemoles gg
moles
If 10.0 g of citric acid (C6H8O7) is added to 500 mL of water, what is the molarity of the resulting solution?
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If 10.0 g of citric acid (C6H8O7) is added to 500 mL of water, what is the molarity of the resulting solution?
Asked: The molarity of a solution
Given: The amount of solute (citric acid) and the volume of solution
Relationships:
Solve: Start by calculating the formula mass of C6H8O7:
Next we calculate the number of moles in 10.0 g of C6H8O7:
Answer:
moles solutemolarity
volume of solution L
6 12.011 8 1.0079 7 15.999 192.12 g mole
1# 10.0 0.0521192.12molemoles g moles
g
0.05210.500
0.104molesmolarityL
M
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Ascorbic acid = Vitamin C
Vitamin C acts as a food preservative by reacting with oxygen (O2)Ascorbic acid
C6H8O6
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How much (volume) of a 1 M ascorbic acid solution will completely react with 0.02 moles of oxygen (O2)?
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Asked: Volume of solution
Given: Concentration (1M) and balanced reaction
Relationships:
According to the balanced reaction we need 2 moles of ascorbic acid for every mole of O2.
moles solutemolarity
volume of solution L
How much (volume) of a 1 M ascorbic acid solution will completely react with 0.02 moles of oxygen (O2)?
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Asked: Volume of solution
Given: Concentration (1M) and balanced reaction
Relationships:
According to the balanced reaction we need 2 moles of ascorbic acid for every mole of O2.
Solve: That means we need 0.04 moles of ascorbic acid:
0.04 0 41
0.04moles solute molesvolume L L ormolarit
LM
my
moles solutemolarity
volume of solution L
How much (volume) of a 1 M ascorbic acid solution will completely react with 0.02 moles of oxygen (O2)?
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Asked: Volume of solution
Given: Concentration (1M) and balanced reaction
Relationships:
According to the balanced reaction we need 2 moles of ascorbic acid for every mole of O2.
Solve: That means we need 0.04 moles of ascorbic acid:
Answer: 40 mL of the solution contains 0.04 moles of ascorbic acid, which is enough to react with 0.02 moles of oxygen (O2).
0.04 0 41
0.04moles solute molesvolume L L ormolarit
LM
my
moles solutemolarity
volume of solution L
How much (volume) of a 1 M ascorbic acid solution will completely react with 0.02 moles of oxygen (O2)?
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The air you breathe is a mixture!
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Air takes up less space under high pressure.
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Standard
Temperature and
Pressure
molar volume: the amount of space occupied by a mole of gas at STP. It is equal to 22.4 L.
0oC
1 atm
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Partial pressures
The total pressure in a mixture of gases is the sum of
the partial pressures of each individual gas
in the mixture.
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Gas A
Gas BGas C
Gas A Gas B
Gas CTotal pressure
=
+
+
Partial pressure of A
Partial pressure of C
Partial pressure of B
Partial pressures
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If 1 L of helium (75%) and neon (25%) is at STP, what is the partial pressure of helium?
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Asked: Partial pressure of helium
Given: 75% He and 25% Ne at STP conditionsStandard pressure is 101,325 Pa or 1 atm
Relationships: The total pressure is the sum of the partial pressures of each gas.
If 1 L of helium (75%) and neon (25%) is at STP, what is the partial pressure of helium?
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Asked: Partial pressure of helium
Given: 75% He and 25% Ne at STP conditionsStandard pressure is 101,325 Pa or 1 atm
Relationships: The total pressure is the sum of the partial pressures of each gas.
Solve: 75,9940.75 101,30.75
250.75 1
Paor
Paatmatm
or
If 1 L of helium (75%) and neon (25%) is at STP, what is the partial pressure of helium?
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Asked: Partial pressure of helium
Given: 75% He and 25% Ne at STP conditionsStandard pressure is 101,325 Pa or 1 atm
Relationships: The total pressure is the sum of the partial pressures of each gas.
Solve:
Answer: The partial pressure of helium is 75,994 Pa or 0.75 atm.
75,9940.75 101,30.75
250.75 1
Paor
Paatmatm
or
If 1 L of helium (75%) and neon (25%) is at STP, what is the partial pressure of helium?
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STP conditions:
Standard
Temperature (0oC)
Pressure (1 atm)
Air is a mixture of gases. Based on Dalton’s law of partial pressures:
2 2...air N O ArP P P P
Concentration of a solution can be expressed in:mass per volumemass percentmolarity
moles of solutemolarity Mliters of solvent