This page contains the detailed and easy notes for Edexcel IGCSE Chemistry Chemical Formulae,Equation and Calculation for revision and understanding.
Edexcel IGCSE Paper 1: Complete Revision Summary
Quantitative Chemistry
- a) Calculating Formulas Mass
- b) Calculating Moles from Masses
- c) Calculating Moles from Volume
- d) Calculating Moles from Concentration
- e) Calculations from Balanced Chemical equations
- f) Percentage Yield
- g) Atom Economy
- h) Titrations
RELATIVE FORMUALE MASS
It is the sum of relative atomic mass of all the atoms present in a compound.
The ratio of the average mass of one atom compared to 1/12th of the mass of C-12
Eg – CO2 = Mass of C + 2(mass of O)
= 12+ (2× 16)
= 44g
CaCO3 = Mass of Ca + Mass of C + 3(mass of O)
= 40+12+ (3× 16)
= 100g
Ca(PO4)3 = Mass of C + 3 × mass of P+ 12(mass of O)
= 310g
MOLES – Amount of substance.
Chemical Formulae,Equation and Calculation
Edexcel IGCSE Chemistry Chemical formulae, equations and calculations
Send download link to:
Edexcel IGCSE Chemistry Chemical formulae, equations and calculations
Send download link to:
Examples
Q1 Calculate the moles of following
- 22g of CO2 Moles = Mass/Mr = 22/44 = 0.5 moles
- 17g of NH3 Mass/Mr = 24/17 =2 moles
- 48dm3 of O2 Volume/24 = 48/24 = 2 moles
- 24000cm3 of CO2 24000/1000dm3 = 24dm3 = 24/24 = 1 mole
- 20g of NaOH dissolved in 50cm3 of Solution Moles = 20/40 = 0.5 moles
Q2 Calculate the mass of :-
- a) 2 moles of calcium carbonate Mass = Moles × Mr =Mr CaCO3 =100 = 2 × 100g= 200g
- b) 0.1 moles of hydrochloric acid Mr of Hcl = 36.5 = 36.5×0.1 = 0.365g
Q3 Calculate the concentration of the following
- a) 2 moles of NaOH dissolved in 10 dm3 of solution = Concentration = Moles/V(dm)3 = 2/10 = 0.2 mol dm-3
- b) 20 g of NaOH dissolved in 50 cm3 of solution = Moles of NaOH = 20/40 = 0.5 moles
C = 0.5/0.05 moldm-3 = 10moldm-3
V= 50/1000 = 0.05dm3
Avogadros Constant
1 mole = 6.02 x 1023 atoms
Q1 Calculate the number of molecules in the following :
- 49 g of sulphuric acid
Mr of H2SO4 = 98g
=98/49 =0.5 moles
= 0.5 x 6.02 x 1023 atoms
= 3.01 x 1023 atoms
- 8 g of oxygen gas
Mr of O2 = 32g
=8/32 =0.25 moles
= 0.25 x 6.02 x 1023 atoms
= 1.50 x 1023 atoms
- 48 dm3 of Nitrogen
Mr of N2 =48/24 = 2 moles
= 2 x 6.02 x 1023 atoms
= 1.20 x 1024 atoms
- d) 50 cm3 of 0.1 mol dm3 of sodium hydroxide
Moles = C x V = 0.1 x 50/1000 = 5 x 10-3 moles
=5 x 10-3 x 6.02 x 1023 atoms
= 3.01 x 1021 atoms
Balanced Chemical Equations
C + O2 CO2
One mole of carbon is reacting with one mole of oxygen to form one mole of carbon dioxide.
2Al + 3O2 2Al2O3
2 moles aluminium reacts with 3 moles of oxygen to form 2 moles of aluminium oxide.
Mg + 2HCl MgCl2 + H2
One mole of magnesium is reacting with 2 moles of hydrochloric acid to form one moles of magnesium chloride and one mole of hydrogen gas.
CALCULATIONS FROM EQUATIONS
Calculate the mass of Magnesium oxide produced from 6 g of Magnesium when burned complete y in air ?
STEP 1: Write the balanced chemical equation.
2Mg + O2 2MgO
STEP2: Write known to the left and unknown to the right
Mg = MgO
STEP3: Write the moles relationship from the balanced chemical equation
2moles = 2 moles
STEP4: Convert moles into mass
48g = 80g
STEP5: Do the Maths.
48/48 = 1g 80/48 = 1.66g
1g× 6 = 6g 1.66g × 6 = 10g
Calculate the mass of alumium needs to produce 306 g of Aluminium Oxide ?
STEP 1: Write the balanced chemical equation.
4Al + 3O2 2Al2O3
STEP2: Write known to the left and unknown to the right
2Al2O3 Al
STEP3: Write the moles relationship from the balanced chemical equation
2moles = 4 moles
STEP4: Convert moles into mass
204g = 108
STEP5: Do the Maths.
306g 108/204 x 306 = 162g
LIMITING REAGENTS
To work out the limiting reagent work out moles of all the reagents and then work from the balanced chemical equation which reagent is in excess and which is in limiting
The reactant that get all used up completely is the limiting reagent. The other reagent which is present in greater quantity than required is in excess.
13.5 gm Aluminium reacts which 32 g of Oxygen
- a) Work out the moles of Aluminium and Oxygen
- b) Which reagent is limiting and which is in excess
- c) Calculation the mass of aluminium oxide produced ?
4Al + 3O2 2Al2O3
- Moles of Al = 13.5/27 = 0.5 moles
Moles of O2 = 32/32 = 1 moles
- 4 moles of Alumunium = 3 moles of oxygen
1 moles of alumnum = ¾ O2
0.5 mol of aluminium = ¾ x 0.5 = 0.375
So 0.375 moles oxygen is required hence oxygen is in excess and alumunium is limiting
- Al = A2O3
4 moles = 2 moles
- 2/4
0.5 – 2/4 x 0.5
=0.25 x 102
=25.5g
PERCENTAGE YIELD
% yield = observed mass/expected mass x 100
= Actual yield/Theoretical yield x 100
When 28 g of nitrogen combined with hydrogen 30 g of ammonia is made ? Calculate the percentage yield ?
N2 + 3H2 2NH3
N2 = NH3
1mole = 2moles of ammonia
28g = 32g of ammonia
Expected = 32g
Observed = 30g
% yield = 30/32 x 100 = 93.75%
When 80 g of iron oxide reacts with carbon, 20 g of iron is produced. Calculate the % yield ?
2Fe2O3 + 3C Fe + 3CO2
Fe2O3 = Fe
2 moles = 4 moles
320g = 224 g
1g =224/320
80g = 224/320 x 80 = 56g
20/56 x 100 = 35.71%
WHY PERCENTAGE YEILD IS NOT 100 %
The percentage yield can never by greater than 100%. It is very difficult to get 100% percentage yield but scientist always look for that route that gives maximum percentage yield.
- Reason for not getting 100% yield
- The reaction does not go to completion so complete products are not formed.
- Some of the reaction can start moving to the reverse direction if they are reversible
- Some of the reaction can go and form alterative or unwanted product.
- During the reaction some of the reactants can get lost or stick to the reaction vessel so do not react.
- If the reaction involves gaseous reactants they can escape.
- Some of the products can also get lost in the reaction vessel. If the reaction involves gaseous products they can also escape.
- The reagent might not be pure therefore did not react completely to give the desired yield.
Atom Economy
Atom economy = Mr of desired product/Total Mr of all the Products x 100
Calcium Oxide is produced using the following reaction
CaCO3 CaO + CO2
Calculate the atom economy
Desired Product = CaO =56g
Mass of reactants = CaCO3 = 100g
Atom Economy = 56/100 x 100 = 56%
Iron oxide is reduced by carbon to form iron and carbon monoxide
Fe203 + 3C 2Fe +3CO
Calculate the atom economy
Desired Product = 2Fe =56 x 2 = 112g
Mass of reactants = Mass of Fe2CO3 + 3(Mass of C) = 196g
% Yield = 112/196 x 100 = 57%
REACTIONS WITH 100 % ATOM ECONOMY
- Addition reaction
- Reactions with only one product have 100 atom economy
- How to increase atom economy?
- Chemist should look for reaction that produce single product
- If the by products are produced they should look for recycling the byproducts or use them in some other reactions to increase the atom economy.
Titration
It is the technique used to determine the exact volume of acid and base to carry out a neutralization reaction.
TITRATION PROCEDURE
- Known Concentration solution either acid or base is measured by the pipette and is added into the conical flask. For this solution both concentration and volume is known.
- The indicator is also added in the conical flask. When the indicator changes colour the end point is reached i.e the solution gets completely neutralised.
- The unknown concentration solution is added into the burette. The starting volume is noted from the burette. The tap is then opened and the unknown solution is added dropwise into the conical flask with regular mixing.
- As soon as the indicator changes colour, the tap is closed and the final reading from the burette is noted.
- The entire process is repeated three times and the values are noted in the following format.
- The concordont reading are taken. The anamolous results are not taken into account.
- The means of the concordont readings are noted and used in the calculation
Titration Example
10 cm3 of 0.5 mol dm3 of sulphuric acid is titrated with sodium hydroxide. The results are given in the table.
2NaOH + H2SO4 Na2SO4 + H20
Calculate the concentration of sodium hydroxide required to completely neutralize the acid ?
Steps
- Write the balanced chemical equation
2NaOH + H2SO4 2NaOH + H20
- Underneath each equation write the numerical value given for each
Moles = 5 x 10-3 x 2 = 10-2 moles
- The quantity that has two value use the concentration triangle to find the moles
V = 10cm3
= 0.01dm3
C = 0.5 mol dm-3
Moles = C x V
0.01 x 0.5=5 x 10-3 moles
- Use the molar ratio to find the moles of unknown quantity
- Use titration volume and find the concentration
Mean Titre = 25.24+25.34+ 25.29/3
= 25.29cm3
Q1 In a Titration 50 cm3 of 0.1 mol dm3 of potasisum hydroxide is neutralized by 20 cm3 of sulphuric Acid.
Calculate the concentration of sulphuric acid.
- a) Write the balanced chemical equation
2KOH + H2SO4 K2SO4 + 2H2O
- b) Underneath each equation write the numerical value given for each
- c) The quantity that has two value use the concentration triangle to find the moles
- d) Use the molar ratio to find the moles of unknown quantity
- e) Use titration volume and find the concentration
V = 0.05dm3 V = 0.02 dm3
C = 0.1 mol dm-3
= 0.005 moles
m = 0.0025 mole
C = 0.125 mol dm-3
Key Terms
- Relative atomic mass — It is the ratio of the average mass of an atom compared to one twelfth of the mass of carbon-12
- Relative formula mass — It is the sum of relative atomic masses of all the atoms present in a formulae
- Moles – It is the amount of substance that has the same number of particles found in 12 g of carbon-12.
- Avogadros Constant —Number of particles present in one mole of the substance.
- 1mole = 6.02 x 1023 atoms
- Limiting Reagent – It is the reagent that is completely used up in the reaction
- Yield— The mass of desired product obtained in a chemical reaction
- Percentage yield = Actual yeild /Theoretical Yield x 100
- Atom Economy = Mass of the desired product/total mass of all the reactants x 100
Concentration = Mass of Solute(g)/Volume of Solution(dm3)
Titration — It is the technique used to determine the exact volume of acids and alkali required to carry out complete neutralization.
Neutralization Reaction Reaction in which acid and base react to form salt and water.
Acids—Substance that has pH less than T
Alkali — Soluble bases that has pH greater than 7
Pipette – It is a glass tube with a bulge in the middle that is used to take out the exact volume of known concentration solutiom
Burette— It is a long tube with the.tap at the bottom that is used to measure the titre
Concordant – Values which are in the range of difference 0.1 to 0.2 cm3
TEST YOURSELF
Q1 Calculate the number of moles in the following
- 10 g of calcium carbonate
Mr = CaCO3 = 100g = 10/100 = 0.1 moles
- 98 g of sulphuric acid
Mr = H2SO4 =98/98 = 1 mole
- 18 g glucose
C6H1206
Mr = 180
18/180 = 0.1 moles
- 90 cm3 of oxygen gas
Firstly convert 90cm3 in to dm3
90/1000 = 0.09 dm3
0.09/24 = 0.00375 moles
- 10 cm3 of 0.2 mol dm3 sodium hydroxide solution
0.2 x 10/1000 = 0.002 moles
Q2 What is the mass of magnesium required to form 160 g of magnesium oxide ?
MgO = Mg
Mg + O2 2MgO
MgO = Mg
Moles 1 1
Mass 4Og 24g
160g 96g
= 96g
Q3 Hydrogen react with chlorine to form hydrogen chloride gas. When 71 g of chlorine reacts 70 g of hydrogen chloride is obtained. Calculate the percentage yield.
H2 + Cl2 2HCl
Cl2 HCl
Cl2 = HCl
Moles 1 2
Mass 71g 73g
160g 96g
% yield = 70/73 x 100 = 95.8%
Q4 Calculate the atom economy of both of these reactions:-
N2 + 3H2 2NH3
34/28+6 x 100 = 100%
CaCO3 CaO + CO2
40+16/100 x100 = 56%
Q5 50 cm3 of 0.2 mol dm3 of HCI reacts with 10 cm3 of NaOH. Determine the concentration of NaOH ?
NaOH + HCl NaCl + H2O
V = 50/1000 = 0.05dm3
C = 0.2
Moles = 0.1
NaOH V = 10/1000 = 0.01dm3
Moles = 0.1 moles
C = 10 moldm-3
DISCLAIMER
Disclaimer: I have tried by level best to provide the answers and video explanations to the best of my knowledge. All the answers and notes are written by me and if there is any similarity in the content then it is purely coincidental. But this is not an alternative to the textbook. You should cover the specification or the textbook thoroughly. This is the quick revision to help you cover the gist of everything. In case you spot any errors then do let us know and we will rectify it.
References:
BBC Bitesize
AQA GCSE Science Kerboodle textbook
Wikipedia
Wikimedia Commons
Make sure you have watched the above videos and are familiar with the key definations before trying these questions. It is also good to time yourself while doing these questions so that you can work on the speed as well.
Analytical Chemistry
- Amount of Substance 1 MS
- Amount of Substance 1 QP
- Amount of Substance 2 MS
- Amount of Substance 2 QP
- of Mass, Chemical Measurements & Eqns 1 MS
- of Mass, Chemical Measurements & Eqns 1 QP
- of Mass, Chemical Measurements & Eqns 2 MS
- of Mass, Chemical Measurements & Eqns 2 QP
- of Mass, Chemical Measurements & Eqns 3 MS
- of Mass, Chemical Measurements & Eqns 3 QP
- Using Conc. of Solutions in mol(dm)-3 MS
- Using Conc. of Solutions in mol(dm)-3 QP
- Yield & Atom Economy MS
- Yield & Atom Economy QP
This page contains the detailed and easy notes for Edexcel IGCSE Chemistry Chemical Formulae,Equation and Calculation for revision and understanding.
Edexcel IGCSE Paper 1: Complete Revision Summary
Quantitative Chemistry
- a) Calculating Formulas Mass
- b) Calculating Moles from Masses
- c) Calculating Moles from Volume
- d) Calculating Moles from Concentration
- e) Calculations from Balanced Chemical equations
- f) Percentage Yield
- g) Atom Economy
- h) Titrations
RELATIVE FORMUALE MASS
It is the sum of relative atomic mass of all the atoms present in a compound.
The ratio of the average mass of one atom compared to 1/12th of the mass of C-12
Eg – CO2 = Mass of C + 2(mass of O)
= 12+ (2× 16)
= 44g
CaCO3 = Mass of Ca + Mass of C + 3(mass of O)
= 40+12+ (3× 16)
= 100g
Ca(PO4)3 = Mass of C + 3 × mass of P+ 12(mass of O)
= 310g
MOLES – Amount of substance.
Chemical Formulae,Equation and Calculation
Edexcel IGCSE Chemistry Chemical formulae, equations and calculations
Send download link to:
Edexcel IGCSE Chemistry Chemical formulae, equations and calculations
Send download link to:
Examples
Q1 Calculate the moles of following
- 22g of CO2 Moles = Mass/Mr = 22/44 = 0.5 moles
- 17g of NH3 Mass/Mr = 24/17 =2 moles
- 48dm3 of O2 Volume/24 = 48/24 = 2 moles
- 24000cm3 of CO2 24000/1000dm3 = 24dm3 = 24/24 = 1 mole
- 20g of NaOH dissolved in 50cm3 of Solution Moles = 20/40 = 0.5 moles
Q2 Calculate the mass of :-
- a) 2 moles of calcium carbonate Mass = Moles × Mr =Mr CaCO3 =100 = 2 × 100g= 200g
- b) 0.1 moles of hydrochloric acid Mr of Hcl = 36.5 = 36.5×0.1 = 0.365g
Q3 Calculate the concentration of the following
- a) 2 moles of NaOH dissolved in 10 dm3 of solution = Concentration = Moles/V(dm)3 = 2/10 = 0.2 mol dm-3
- b) 20 g of NaOH dissolved in 50 cm3 of solution = Moles of NaOH = 20/40 = 0.5 moles
C = 0.5/0.05 moldm-3 = 10moldm-3
V= 50/1000 = 0.05dm3
Avogadros Constant
1 mole = 6.02 x 1023 atoms
Q1 Calculate the number of molecules in the following :
- 49 g of sulphuric acid
Mr of H2SO4 = 98g
=98/49 =0.5 moles
= 0.5 x 6.02 x 1023 atoms
= 3.01 x 1023 atoms
- 8 g of oxygen gas
Mr of O2 = 32g
=8/32 =0.25 moles
= 0.25 x 6.02 x 1023 atoms
= 1.50 x 1023 atoms
- 48 dm3 of Nitrogen
Mr of N2 =48/24 = 2 moles
= 2 x 6.02 x 1023 atoms
= 1.20 x 1024 atoms
- d) 50 cm3 of 0.1 mol dm3 of sodium hydroxide
Moles = C x V = 0.1 x 50/1000 = 5 x 10-3 moles
=5 x 10-3 x 6.02 x 1023 atoms
= 3.01 x 1021 atoms
Balanced Chemical Equations
C + O2 CO2
One mole of carbon is reacting with one mole of oxygen to form one mole of carbon dioxide.
2Al + 3O2 2Al2O3
2 moles aluminium reacts with 3 moles of oxygen to form 2 moles of aluminium oxide.
Mg + 2HCl MgCl2 + H2
One mole of magnesium is reacting with 2 moles of hydrochloric acid to form one moles of magnesium chloride and one mole of hydrogen gas.
CALCULATIONS FROM EQUATIONS
Calculate the mass of Magnesium oxide produced from 6 g of Magnesium when burned complete y in air ?
STEP 1: Write the balanced chemical equation.
2Mg + O2 2MgO
STEP2: Write known to the left and unknown to the right
Mg = MgO
STEP3: Write the moles relationship from the balanced chemical equation
2moles = 2 moles
STEP4: Convert moles into mass
48g = 80g
STEP5: Do the Maths.
48/48 = 1g 80/48 = 1.66g
1g× 6 = 6g 1.66g × 6 = 10g
Calculate the mass of alumium needs to produce 306 g of Aluminium Oxide ?
STEP 1: Write the balanced chemical equation.
4Al + 3O2 2Al2O3
STEP2: Write known to the left and unknown to the right
2Al2O3 Al
STEP3: Write the moles relationship from the balanced chemical equation
2moles = 4 moles
STEP4: Convert moles into mass
204g = 108
STEP5: Do the Maths.
306g 108/204 x 306 = 162g
LIMITING REAGENTS
To work out the limiting reagent work out moles of all the reagents and then work from the balanced chemical equation which reagent is in excess and which is in limiting
The reactant that get all used up completely is the limiting reagent. The other reagent which is present in greater quantity than required is in excess.
13.5 gm Aluminium reacts which 32 g of Oxygen
- a) Work out the moles of Aluminium and Oxygen
- b) Which reagent is limiting and which is in excess
- c) Calculation the mass of aluminium oxide produced ?
4Al + 3O2 2Al2O3
- Moles of Al = 13.5/27 = 0.5 moles
Moles of O2 = 32/32 = 1 moles
- 4 moles of Alumunium = 3 moles of oxygen
1 moles of alumnum = ¾ O2
0.5 mol of aluminium = ¾ x 0.5 = 0.375
So 0.375 moles oxygen is required hence oxygen is in excess and alumunium is limiting
- Al = A2O3
4 moles = 2 moles
- 2/4
0.5 – 2/4 x 0.5
=0.25 x 102
=25.5g
PERCENTAGE YIELD
% yield = observed mass/expected mass x 100
= Actual yield/Theoretical yield x 100
When 28 g of nitrogen combined with hydrogen 30 g of ammonia is made ? Calculate the percentage yield ?
N2 + 3H2 2NH3
N2 = NH3
1mole = 2moles of ammonia
28g = 32g of ammonia
Expected = 32g
Observed = 30g
% yield = 30/32 x 100 = 93.75%
When 80 g of iron oxide reacts with carbon, 20 g of iron is produced. Calculate the % yield ?
2Fe2O3 + 3C Fe + 3CO2
Fe2O3 = Fe
2 moles = 4 moles
320g = 224 g
1g =224/320
80g = 224/320 x 80 = 56g
20/56 x 100 = 35.71%
WHY PERCENTAGE YEILD IS NOT 100 %
The percentage yield can never by greater than 100%. It is very difficult to get 100% percentage yield but scientist always look for that route that gives maximum percentage yield.
- Reason for not getting 100% yield
- The reaction does not go to completion so complete products are not formed.
- Some of the reaction can start moving to the reverse direction if they are reversible
- Some of the reaction can go and form alterative or unwanted product.
- During the reaction some of the reactants can get lost or stick to the reaction vessel so do not react.
- If the reaction involves gaseous reactants they can escape.
- Some of the products can also get lost in the reaction vessel. If the reaction involves gaseous products they can also escape.
- The reagent might not be pure therefore did not react completely to give the desired yield.
Atom Economy
Atom economy = Mr of desired product/Total Mr of all the Products x 100
Calcium Oxide is produced using the following reaction
CaCO3 CaO + CO2
Calculate the atom economy
Desired Product = CaO =56g
Mass of reactants = CaCO3 = 100g
Atom Economy = 56/100 x 100 = 56%
Iron oxide is reduced by carbon to form iron and carbon monoxide
Fe203 + 3C 2Fe +3CO
Calculate the atom economy
Desired Product = 2Fe =56 x 2 = 112g
Mass of reactants = Mass of Fe2CO3 + 3(Mass of C) = 196g
% Yield = 112/196 x 100 = 57%
REACTIONS WITH 100 % ATOM ECONOMY
- Addition reaction
- Reactions with only one product have 100 atom economy
- How to increase atom economy?
- Chemist should look for reaction that produce single product
- If the by products are produced they should look for recycling the byproducts or use them in some other reactions to increase the atom economy.
Titration
It is the technique used to determine the exact volume of acid and base to carry out a neutralization reaction.
TITRATION PROCEDURE
- Known Concentration solution either acid or base is measured by the pipette and is added into the conical flask. For this solution both concentration and volume is known.
- The indicator is also added in the conical flask. When the indicator changes colour the end point is reached i.e the solution gets completely neutralised.
- The unknown concentration solution is added into the burette. The starting volume is noted from the burette. The tap is then opened and the unknown solution is added dropwise into the conical flask with regular mixing.
- As soon as the indicator changes colour, the tap is closed and the final reading from the burette is noted.
- The entire process is repeated three times and the values are noted in the following format.
- The concordont reading are taken. The anamolous results are not taken into account.
- The means of the concordont readings are noted and used in the calculation
Titration Example
10 cm3 of 0.5 mol dm3 of sulphuric acid is titrated with sodium hydroxide. The results are given in the table.
2NaOH + H2SO4 Na2SO4 + H20
Calculate the concentration of sodium hydroxide required to completely neutralize the acid ?
Steps
- Write the balanced chemical equation
2NaOH + H2SO4 2NaOH + H20
- Underneath each equation write the numerical value given for each
Moles = 5 x 10-3 x 2 = 10-2 moles
- The quantity that has two value use the concentration triangle to find the moles
V = 10cm3
= 0.01dm3
C = 0.5 mol dm-3
Moles = C x V
0.01 x 0.5=5 x 10-3 moles
- Use the molar ratio to find the moles of unknown quantity
- Use titration volume and find the concentration
Mean Titre = 25.24+25.34+ 25.29/3
= 25.29cm3
Q1 In a Titration 50 cm3 of 0.1 mol dm3 of potasisum hydroxide is neutralized by 20 cm3 of sulphuric Acid.
Calculate the concentration of sulphuric acid.
- a) Write the balanced chemical equation
2KOH + H2SO4 K2SO4 + 2H2O
- b) Underneath each equation write the numerical value given for each
- c) The quantity that has two value use the concentration triangle to find the moles
- d) Use the molar ratio to find the moles of unknown quantity
- e) Use titration volume and find the concentration
V = 0.05dm3 V = 0.02 dm3
C = 0.1 mol dm-3
= 0.005 moles
m = 0.0025 mole
C = 0.125 mol dm-3
Key Terms
- Relative atomic mass — It is the ratio of the average mass of an atom compared to one twelfth of the mass of carbon-12
- Relative formula mass — It is the sum of relative atomic masses of all the atoms present in a formulae
- Moles – It is the amount of substance that has the same number of particles found in 12 g of carbon-12.
- Avogadros Constant —Number of particles present in one mole of the substance.
- 1mole = 6.02 x 1023 atoms
- Limiting Reagent – It is the reagent that is completely used up in the reaction
- Yield— The mass of desired product obtained in a chemical reaction
- Percentage yield = Actual yeild /Theoretical Yield x 100
- Atom Economy = Mass of the desired product/total mass of all the reactants x 100
Concentration = Mass of Solute(g)/Volume of Solution(dm3)
Titration — It is the technique used to determine the exact volume of acids and alkali required to carry out complete neutralization.
Neutralization Reaction Reaction in which acid and base react to form salt and water.
Acids—Substance that has pH less than T
Alkali — Soluble bases that has pH greater than 7
Pipette – It is a glass tube with a bulge in the middle that is used to take out the exact volume of known concentration solutiom
Burette— It is a long tube with the.tap at the bottom that is used to measure the titre
Concordant – Values which are in the range of difference 0.1 to 0.2 cm3
TEST YOURSELF
Q1 Calculate the number of moles in the following
- 10 g of calcium carbonate
Mr = CaCO3 = 100g = 10/100 = 0.1 moles
- 98 g of sulphuric acid
Mr = H2SO4 =98/98 = 1 mole
- 18 g glucose
C6H1206
Mr = 180
18/180 = 0.1 moles
- 90 cm3 of oxygen gas
Firstly convert 90cm3 in to dm3
90/1000 = 0.09 dm3
0.09/24 = 0.00375 moles
- 10 cm3 of 0.2 mol dm3 sodium hydroxide solution
0.2 x 10/1000 = 0.002 moles
Q2 What is the mass of magnesium required to form 160 g of magnesium oxide ?
MgO = Mg
Mg + O2 2MgO
MgO = Mg
Moles 1 1
Mass 4Og 24g
160g 96g
= 96g
Q3 Hydrogen react with chlorine to form hydrogen chloride gas. When 71 g of chlorine reacts 70 g of hydrogen chloride is obtained. Calculate the percentage yield.
H2 + Cl2 2HCl
Cl2 HCl
Cl2 = HCl
Moles 1 2
Mass 71g 73g
160g 96g
% yield = 70/73 x 100 = 95.8%
Q4 Calculate the atom economy of both of these reactions:-
N2 + 3H2 2NH3
34/28+6 x 100 = 100%
CaCO3 CaO + CO2
40+16/100 x100 = 56%
Q5 50 cm3 of 0.2 mol dm3 of HCI reacts with 10 cm3 of NaOH. Determine the concentration of NaOH ?
NaOH + HCl NaCl + H2O
V = 50/1000 = 0.05dm3
C = 0.2
Moles = 0.1
NaOH V = 10/1000 = 0.01dm3
Moles = 0.1 moles
C = 10 moldm-3
DISCLAIMER
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References:
BBC Bitesize
AQA GCSE Science Kerboodle textbook
Wikipedia
Wikimedia Commons
