6th Year
Chemistry
Higher Level
Sinéad Nolan
Stoichiometry
No part of this publication may be copied, reproduced or transmitted in any form or by any means,
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The Dublin School of Grinds.
Ref: 6/che/h/sn/stoichiometry
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Stoichiometry
A mole (also known as Avogadro's Number) is the number that is
used in making calculations involving atoms and molecules. Given
the relatively microscopic size of the particles, it would be rather
difficult to calculate amounts in terms of numbers of atoms. So, we
use the mole.
A mole, (mol for short) is equal to 6.022 x 1023 atoms or molecules,
(which is equal to the same number of atoms found in 12.000 grams of carbon-12).
The Atomic mass given for an element on the periodic table measured out in grams is
equal to one mole of atoms of that element.
Thus, the Molecular mass (Mr) of elements and compounds is the mass, in grams, equal
to the atomic and formula masses of those elements and compounds. The unit of
Molecular mass is grams per mole, g/mol or gmol-1.
Calculate the molecular masses for each of the following
1. CO2
6. NH4OH
2. NO3-
7. Cu(NO3)2
3. CCl4
8. (NH4)3PO4
4. Na2SO4
9. CH3COOH
5. C12H22O11
10.Na2CO3.10H2O
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Sinéad Nolan
nop
mass
n
Mr
n
cm3
n
6x1023
cm3
22400
n
@ STP
24000
@RTP
n
cM
@ The Dublin School of Grinds
vL
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Sinéad Nolan
Need to know the following conversions:
mass  mols, mols  mass, nop  mols, mols  nop, mass  nop & nop  mass…etc
 Mr
mass
mols
x Mr
 6x1023
nop
mols
x 6x1023
x 6x1023
 Mr
nop
mols
mass
x Mr
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nop
 6x1023
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Sinéad Nolan
Example 1
Calculate the mass of 0.125 moles of calcium chloride, CaCl2
Example 2
How many mols of sulphuric acid, H2SO4 are there in 12.25 g of sulphuric acid?
Example 3
How many atoms of sodium are present in 1.25 mols of the metal?
Example 4
How many (a) molecules, (b) atoms of hydrogen and (c) atoms of oxygen are present in
0.75 moles of water, H2O?
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Sinéad Nolan
Example 5
What is the mass in grams of 3x1023 molecules of ethanol, C2H5OH?
Example 6
How many (a) molecules, (b) atoms of carbon and (c) atoms of oxygen are present in 150
g of carbon dioxide, CO2?
Example 7
How many moles of gas are present in a sample containing 1.8 x 10 24 atoms of chlorine
at s.t.p.?
LCH 2009 10 (a)
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Sinéad Nolan
Need to know the following conversions:
cm3  mols, mols  cm3, cm3  nop & nop  cm3…etc
 22400
@ STP
cm3
mols
x 22400
@ RTP
 24000
cm3
Notes:
mols
x 24000

1 mol of any gas occupies 22,400 cm3 at STP or 24,000 cm3 at RTP

Make sure you read the question carefully to determine whether to use 22,400 cm3
(STP) or 24,000 cm3 (RTP)!

Remember there are 1000 cm3 in 1 litre
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Sinéad Nolan
Example 1
Calculate the volume occupied by 1.68 moles of chlorine gas, Cl2 at STP.
Example 2
How many mols of sulphur dioxide, SO2 are there in 680 cm3 of the gas measured at STP.
Example 3
Calculate the volume occupied by 1.68 moles of chlorine gas, Cl2 at RTP.
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Sinéad Nolan
Example 4
How many mols of sulphur dioxide, SO2 are there in 680 cm3 of the gas measured at RTP.
Example 5
What is the volume in cm3 of 9 x 1023 molecules of nitrogen, N2 measured at RTP?
Example 6
How many (a) molecules, (b) atoms of carbon and (c) atoms of oxygen are present in 720
cm3 of carbon dioxide, CO2 measured at STP?
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Sinéad Nolan
Example 7
What is the volume in cm3 of 9 x 1023 molecules of chlorine, Cl2 measured at STP?
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Sinéad Nolan
Calculate the % by mass of an element in a compound
%X
total mass of X
MR
Example 1
Calculate the percentage by mass of oxygen in ethanoic acid, CH3COOH.
Example 2
What is the percentage by mass of nitrogen in ammonium nitrate, NH4NO3
LCH 2003 4 (g)
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Sinéad Nolan
Calculate the Empirical Formula of a compound from its % composition
There is more than one kind of chemical formula, namely they are empirical and
molecular formulas. Empirical formulas give the lowest whole number ratio of the atoms
in a compound, whereas the molecular formula gives the exact composition of one
molecule.
Empirical
Molecular
HO
H2O2
CH
C 2H 2
CH
C 6H 6
NO
NO
NO2
N2O4
Step 1: Convert mass percents to mass in grams
Step 2: Convert the mass of each element to moles of that element by dividing by the Ar
Step 3: Divide each mole value by the smallest number of mols to convert to mol ratios
Step 4: You can also be asked to determine the chemical formula of the compound
when given its Mr
Example 1
An oxide of copper contains 88.8% by mass of the metal. What is the empirical formula
of the oxide?
LCH 1998
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Example 2
A compound containing only carbon, hydrogen and oxygen was found to conatin
52.17% carbon, 13.04% hydrogen and 34.79% oxygen. What is the empirical formula of
the compound? Using a mass spectrometer, it was found that the relative molecular
mass of the compound was 184. What is the molecular formula?
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Calculate the Empirical Formula of a compound given the masses of reactants and
products
Step 1: Calculate the masses of all reactants and products by subtraction – Law of
Conservation of Mass
Step 2: Convert the mass of each element to moles of that element by dividing by the Ar
Step 3: Divide each mole value by the smallest number of mols to convert to mol ratios
Example 1
When 4.10 g of hydrated magnesium sulfate, MgSO4.xH2O, were heated strongly, 2.00
g of anhydrous magnesium sulfate were obtained.
Calculate the value of x, the degree of hydration of the crystals.
LCH 2011 4(e)
Example 2
When 3.175 g of copper reacts with chlorine gas 6.725 g of copper chloride is formed.
Find by calculation the empirical formula of the chloride.
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Sinéad Nolan
Calculate masses of reactants and products from a balanced equation
Step 1: Calculate the number of mols ( Mr,  22,400 cm3,  24,000 cm3…etc) of reactants
required or products produced
Step 2: Using a balanced equation and ratio, calculate the number of mols of product
produced or reactants required
Step 3: Convert back to the units requested in the question (x Mr, x 22,400 cm3,
x
24,000 cm3…etc)
Example 1
The fermentation of glucose results in the formation of ethanol and carbon dioxide,
according to the equation:
C6H12O6 = 2C2H5OH + 2CO2.
If 126 g of glucose are consumed
(i) how many moles of glucose does this represent?
(ii) assuming complete conversion of glucose to ethanol. How many moles of ethanol are
produced?
(iii) what volume of carbon dioxide measured at S.T.P. is produced?
(iv) how many molecules of carbon dioxide does this volume contain?
When the carbon dioxide is bubbled through limewater (calcium hydroxide solution) the
solution first turns a milky colour due to the formation of calcium carbonate. It then goes
clear again, due to the formation of calcium hydrogencarbonate. The overall reaction
may be represented by the equation:
Ca(OH)2 + 2CO2 = Ca(HCO3)2
If the carbon dioxide produced in the fermentation above were passed through
limewater, calculate the maximum mass of hydrogencarbonate that could be formed.
SQ
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Sinéad Nolan
Example 2
In a reaction 14.7 g of potassium dichromate(VI) reacted completely with concentrated
hydrochloric acid according to the equation:
K2Cr2O7 + 14 HCl = 2KCl + 2CrCl3 + 7H2O + 3Cl2
(i) How many moles of potassium dichromate(VI) were used?
(ii) How many moles of water were produced?
(iii) What volume of chlorine, measured at s.t.p was produced?
(iv) How many molecules of chlorine did this volume contain?
(v) If the chlorine produced in the reaction were bubbled through a solution containing
excess sodium bromide, calculate the mass of bromine liberated according to the
equation according to the equation:
Cl2 + 2NaBr = 2NaCl + Br2
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Example 3
When crystalline copper (II) nitrate is heated the following reaction takes place:
2Cu(NO3)2.3H2O = 2CuO + 4NO2 + O2 + 6H2O
If 4.83 g of crystalline copper (II) nitrate were heated, calculate
(i) the mass of copper (II) oxide
(ii) the volume of nitrogen dioxide (at S.T.P.)
(iii) the number of molecules of oxygen, that would be produced according to the above
equation.
LC 1999
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Expressing the concentrations of solutions
M = mol per litre of solution (Molarity)
e.g. 1.25 M H2SO4 = 1.25 mols of H2SO4 per litre
% w/v = number of grams per 100 cm3 of solution
e.g. 15 % w/v Mg(OH)2 = 15 grams of Mg(OH)2 per 100 cm3 of solution
% v/v= number of cm3 per 100 cm3 of solution
e.g. 4.5 % v/v C2H5OH = 4.5 cm3 of C2H5OH per 100 cm3 of solution
% w/w = number of grams per 100 grams of solution
e.g. 10 % w/w NaCl = 10 grams of NaCl per 100 grams of solution
ppm = parts per million = milligrams per litre of solution
e.g. 50 ppm of dissolved O2 in a water sample = 50 mg O2 per litre of water
Need to be able to do all inter-conversions, but especially be able to convert to M (mol/L)
Example 1
What is the molarity of a solution that contains 3.68 g of NaOH per 250 cm3 of solution?
Example 2
Calculate the concentration in grams per litre of a H 2SO4 solution whose concentration
is 2.5 M.
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Sinéad Nolan
Example 3
A 500 cm3 can of beer contains 21.5 cm3 of ethanol. Calculate its % alcohol, i.e. the
concentration of alcohol in the beer as a % (v/v).
LCH 2007 4 (h)
Example 4
On analysing a sample of water, a chemist finds that 50 cm3 of it contains 0.007 g of
calcium carbonate, CaCO3. What is the concentration of CaCO3 in ppm.
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Sinéad Nolan
Calculating the number of moles given a volume and molarity
n
cM
vL
Notes:
 Concentration must be in M (mols per litre – remember how to convert)
 Volume must be in Litres (1000cm3 in 1 Litre)
Example 1
How many moles of NaOH are present in 50 cm3 of 0.68 M NaOH?
Example 2
What volume of 0.65 M H2SO4 solution will contain 5 grams of sulphuric acid?
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Example 4
Hydrochloric acid is severely corrosive to skin and eyes and toxic by inhalation or
ingestion. It should be handled carefully and stored safely. The entire contents of a
bottle containing 2.5 litres of concentrated hydrochloric acid were accidentallyspilled in
a laboratory. The spilled acid was neutralised by adding solid powdered sodium
carbonate.
The neutralisation reaction is described by the following equation.
Na2CO3 + 2HCl = 2NaCl + H2O + CO2
The spilled acid was a 36% (w/v) solution of hydrogen chloride in water.
(i) Calculate the number of moles of hydrochloric acid spilled.
(ii) What was the minimum mass of anhydrous sodium carbonate required to completely
neutralise all of the spilled hydrochloric acid?
(iii) What volume of carbon dioxide in litres, at room temperature and pressure, was
LCH 2004 10 (a)
produced in this neutralisation reaction?
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Example 4
An indigestion tablet contains a mass of 0.30 g of magnesium hydroxide [Mg(OH)2] as
its only basic ingredient. The balanced chemical equation for the reaction between
magnesium hydroxide and hydrochloric acid (HCl(aq)), the acid produced in the
stomach, is as follows:
Mg(OH)2 + 2HCl = MgCl2 + 2H2O
(i) Calculate the volume of 1.0 M HCl neutralised by two of these indigestion tablets. Give
your answer correct to the nearest cm3.
(ii) What mass of salt is formed in this neutralisation?
(iii) How many magnesium ions are present in this amount of the salt?
(iv) Another indigestion remedy consists of a suspension of magnesium hydroxide
[Mg(OH)2] in water and is marked 6% (w/v).
What volume of this second indigestion remedy would have the same neutralising effect
on stomach acid as two of the indigestion tablets mentioned earlier?
LCH 2005 10 (a)
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Past Exam Short Questions related to this topic
LC 2015 – Question 4 (a)
Solution
LC 2015 – Question 4 (e)
Solution
LC 2014 – Question 4 (f)
Solution
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LC 2014 – Question 4 (g)
Solution
LC 2014 – Question 4 (h)
Solution
LC 2013 – Question 4 (c)
Solution
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LC 2013 – Question 4 (e)
Solution
LC 2011 – Question 4 (e)
Solution
LC 2010 – Question 4 (d)
Solution
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LC 2007 – Question 4 (e)
Solution
LC 2007 – Question 4 (h)
Solution
LC 2006 – Question 4 (d)
Solution
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LC 2005 – Question 4 (h)
Solution
LC 2004 – Question 4 (h)
Solution
LC 2003 – Question 4 (b)
Solution
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LC 2003 – Question 4 (g)
Solution
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Past Exam Short Solutions related to this topic
LC 2014 – Question 4 (f) Solution
LC 2014 – Question 4 (g) Solution
LC 2014 – Question 4 (h) Solution
LC 2013 – Question 4 (c) Solution
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LC 2013 – Question 4 (e) Solution
LC 2011 – Question 4 (e) Solution
LC 2010 – Question 4 (d) Solution
LC 2007 – Question 4 (e) Solution
LC 2007 – Question 4 (h) Solution
LC 2006 – Question 4 (d) Solution
LC 2005 – Question 4 (h) Solution
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LC 2004 – Question 4 (h) Solution
LC 2003 – Question 4 (b) Solution
LC 2003 – Question 4 (g) Solution
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Past Exam Long Questions related to this topic
LC 2015 – Question 10 (c)
Solution
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LC 2014 – Question 11 (b)
Solution
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LC 2013 – Question 10 (b) (ii)
Solution
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LC 2012 – Question 10 (c) (ii – iv)
Solution
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LC 2011 – Question 10 (b)
Solution
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LC 2008 – Question 11 (b)
Solution
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LC 2005 – Question 10 (a)
Solution
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LC 2004 – Question 10 (a)
Solution
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LC 2002 – Question 11 (a) (ii – iv)
Solution
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Past Exam Long Solutions related to this topic
LC 2014 – Question 11 (b)
Solution
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LC 2013 – Question 10 (b) (ii) Solution
LC 2012 – Question 10 (c) (ii – iv) Solution
LC 2011 – Question 10 (b) Solution
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LC 2008 – Question 11 (b) Solution
LC 2005 – Question 10 (a) Solution
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LC 2004 – Question 10 (a) Solution
LC 2002 – Question 11 (a) (ii – iv) Solution
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