Topic 1.3 chemical reactions and related calculations
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Transcript of Topic 1.3 chemical reactions and related calculations
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Topic 1.3 Chemical reactions and related calculations
file://localhost/Users/carter.j/Movies/iSkysoft Free Video Downloader Videos/Chemistry - A Volatile History (Episode 1)(Part 2-6).flv
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Topic 1.3: Chemical reactions and related calculations
When elements react, their atoms join with other atoms to form compounds
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04/13/2023
The reaction of Iron and Sulfur
Fe + S FeS
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Relative formula mass (Mr)
The relative formula mass is the sum of the masses of the atoms in the numbers shown in the formula.
E.g.
The relative atomic mass (Ar) of Hydrogen is 1.0
There are two hydrogen atoms in a molecule of H2 so the Mr of H2 is 1.0 + 1.0 = 2.0
The decimal points are really important, if it is 1.0 on the
periodic table then that is the number you use, and you must quote your answer to the same
number of decimal places!
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From yesterday’s practical
Iron reacts with sulfur to form iron sulfide with a formula of FeS
Fe has an Ar of 55.8
S has an Ar of 32.1
Therefore the Mr of FeS is 55.8 + 32.1 =
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Calculate the relative formula mass (Mr) of:
A) Cl2
B) Ne
C) NH3
D) CH4
E) MgBr2
F) S8
G) Ca(OH)2
H) K2SO4
I) NH4NO3
J) Ca(NO3)2
K) Al2(SO4)3
L) H2C2O4.2H2O
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Calculate the relative formula mass (Mr) of:
A) Cl2 71.0
B) Ne 20.2
C) NH3 15.0
D) CH4 16.0
E) MgBr2 184.1
F) S8 256.8
G) Ca(OH)2
74.1
H) K2SO4
174.3
I) NH4NO3
80
J) Ca(NO3)2
164.1
K) Al2(SO4)3
342.3
L) H2C2O4.2H2O 126
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The reaction of Magnesium and Oxygen
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Avogadro’s number & the mole
A mole is the amount of a substance in grams which has the same number of particles as there are atoms in 12 g of 12C.
Italian physicist Amedeo Avogadro was investigating the number of molecules in different volumes of gases, and found that, under the same conditions, one mole of a gas always contained the same number of particles. So, one mole of CO2 has the same number of particles as one mole of helium or one mole of methane, or any other gas. The symbol for the Avogadro constant is L after the Austrian Loschmidt, who originally calculated the value for the constant, which is 6.023 x 1023, (602,300,000,000,000,000,000,000,000).
You do not need to learn this!
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The Avogadro constant is given the symbol L.
L = 6.023 x 1023 particles mol-1
The mole is a quantity of particles.
1 mol is 6.023 x 1023 particles
The mass of a 12C atom is 1.992 x 10-23 g. If a mole contains 6.023 x 1023 of these atoms, then a mole of 12C has a mass of:
6.023 x 1023 x 1.992 x 10-23 = 11.998 g
Avogadro’s number is the number of atoms in 12 g of carbon
You do not need to learn this!
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The relative formula mass of a substance, in grams, is known as one mole of that substance
Candidates are expected to use the relative formula mass of a substance to calculate the number of moles in a given mass of that substance and vice versa.
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Moles and masses:
To convert the mass of a substance to moles use:
Number of moles of an element = mass
Ar
Number of moles of a compound = mass
Mr
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Balanced equations
Chemical reactions can be represented by word equations or symbol equations.
Candidates should be able to write word and balanced symbol equations for reactions in the specification.
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Some common anion names:
F Fluoride
Cl Chloride
I Iodide
Br Bromide
O Oxide
OH Hydroxide
CO3 Carbonate
SO4 Sulfate
NO3/NO2 Nitrate
PO4 Phosphate
The –ate at the end of some anion names means that they contain oxygen, eg sulfate contains sulfur and oxygen, sulfide is just sulfur on its own.
Make a copy of this table in your book!
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Balancing equations - 1
From the worksheet, first try to balance the equation, then try to write a word equation for the reaction
E.g. H2 + Cl2 HCl
H2 + Cl2 2HCl Balanced
Hydrogen + Chlorine Hydrogen chloride
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States: (s), (l), (g), (aq)
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In a chemical equation the states are shown for the elements of compound at room temperature.
E.g.
Sodium + water sodium hydroxide + hydrogen
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
It tells us that solid sodium reacts with liquid water to produce a solution of sodium hydroxide and hydrogen
gas
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Homework
Complete worksheet:
Equations and Molar Ratios
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Percentage mass
The percentage mass of an element in a formula can be calculated by dividing the the relative mass of the compound by the relative atomic mass of the element in the formula:
E.g. The percentage mass of H in CH4
There are 4 x 1.0 = 4.0
4.0/16.0 = 0.25 or 25%
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Calculate the percentage mass in the following
a) C in CH4 e) N in Ca(NO3)2
b) Br in MgBr2 f) O in Ca(NO3)2
c) S in K2SO4 g) O in Ca(OH)2
d) N in NH4NO3 h) O in Fe(NO3)3
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Calculate the percentage mass in the following
a) C in CH4 e) N in Ca(NO3)2
75.0% 17.1%
b) Br in MgBr2 f) O in Ca(NO3)2
86.8% 58.5`%
c) S in K2SO4 g) O in Ca(OH)2
18.4% 43.2%
d) N in NH4NO3 h) O in Fe(NO3)3
35.0% 59.6%
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Calculating reacting masses
The masses of reactants and products can be calculated from balanced symbol equations
Candidates should be able to calculate the mass of a reactant or product from information about the mass of the other reactants and products in the reaction and the balanced symbol equation
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The reaction of a iodine with zinc
Intention – to carry out a reaction that will allow us to apply all the skills we have been learning this week (balancing equations, calculating Mr values and working out numbers of moles)
Take photos of each stage, you will need them to produce a flow diagram of the investigation.
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Mole calculations
1. Calculate the number of moles that you have using the mass you are given in the question and the Mr
Number of moles of ______ = _____ / _____ = ____
Find the ratio (stoichiometry) of the reaction equation
If I have ____ moles of _____, then I must have ____ moles of _____.
Find the mass of the unknown:
Mass of _____ = moles x Mr = _____ x _____ = ______g
Mass
Moles Mr
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Finding the value of X in CuSO4.XH2O
Intention – to carry out a reaction that will allow us to further develop all the skills we have been learning (balancing equations, calculating Mr values and working out numbers of moles)
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Irreversible reactions
The combustion of methane (CH4) to make CO2 and H2O is an irreversible reaction:
CH4 + 2O2 CO2 + 2H2O
What this means is that we cannot react CO2 and H2O together to make CH4 and O2
CO2 + 2H2O CH4 + 2O2
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Reversible reactions
A reversible reaction is a chemical change in which the products can be converted back to the reactants under suitable conditions.
A reversible reaction can be shown by the sign
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Revision materials
Task, in pairs, produce revision material(s) on one of the following topics:
Balancing equations
The mole
Relative molecular mass
Conservation of mass in a reaction
Yield
Reversible reactions
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Revision materials
Key words Clear explanations
Colourful and attractive to look at
Include test questions
Include model answers
Use diagrams