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10 a(1)
but-1-ene
but-2-ene

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QUESTION 7 (A)
Type of reaction of substance A is exothermic reaction while substance B is endothermic reaction. Temperature change in substance A increases while temperature change in substance B decreases. Change in the total energy of reactant substance A decreases and the total energy content of product is lower. While change in the total energy of reactant substance B increases and the total energy content of product is higher. Reaction occur in substance A is formation bond while substance B is breaking bond. The example of reaction of substance A is neutralization while substance B is frying egg.

QUESTION 7 (B)
Number of mole of CuSO4
= (100*0.5)/1000
= 0.05
Number of mole of MgSO4 = 0.05
Mg + CuSO₄→MgSO4 + Cu

ΔH = -mcδ/n
-105000 = (100*4.2*δ)/0.05
5250 = 420δ
δ = 12.5 ℃
Temperature increased by 12.5 ℃.

QUESTION 7 (C) i.
Acid X = Ethanoic Acid
Acid Y = Hydrochloric Acid

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aii) C4H8+6O2->4CO2+4H2O
no. of mol of C4H8
=8.4/4(12)+8
=0.15 mol
From eqn,
1 mol of C4H8 produce 4 mol of CO2
0.15 mol of C4H8 produce 0.6 mol of CO
bi) process I is dehydration,
process ll is esterification
compound Q is propanoic acid
cIII)

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ai)average rate of reaction for experiment 1=40/60=0.667cm3/s average rate of reaction for experiment2 =40/45=0.889cm3/s
b)page 30-33

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a)i. The process is called rusting.The iron is placed below the zinc in electrochemistry series.Thus zinc is more electropositive than iron and zinc is more reactive than iron.Zn will inhibit the rusting of Fe.

a)ii. Magnesium is more electropositive than zinc.Thus, the magnesium is more reactive to surrounding to form other compound.This makes Mg cannot protect iron from rusting.

b) Experiment I : not redox reaction because there are not change in oxidation number in both AgNO3 and  NaCl.
Experiment II : Redox reaction.The oxidation number of Zinc is increase from 0 -> +2 and the oxidation number of copper is decrease from +2 -> 0
So,both of the oxidation and reduction occured in this experiment.
c)
A)Changing of iron (II). Fe² ions to iron (III), Fe³ and vice versa.

Experiment :

To investigate the conversion of iron (II) ions to iron (III) ions and vice versa.

Apparatus : test tubes, boiling tube, dropper,. Test tube holder, filter funnel, Bunsen burner,

matches , spatula.

Materials : FeSO4 solution, FeCl3 solution, acidified KMnO4

solution, Zn powder, filter paper,

NaOH solution, potassium hexacyanoferrate (II) solution, potassium hexacyanoferrate (III) solution, potassium thiocyanate solution.

Procedure of Changing iron (II) ions, Fe2+ to iron (III) ions, Fe3+

1. Pour 4 cm³ of FeSO4 solution into a test tube.

2. Add acidified KMnO4

solution drop by drop until a yellow solution or brown solution is obtained.

3.Divide the solution obtained equally into 3 separate test tubes.

4.Test the solution with :

i.Sodium hydroxide solution

ii Potassium hexacyanoferrate (II) solution

iii.Potassium thiocyanate solution.

5.Record all the observations.

Data & observation :

II.Changing iron (III) ions, Fe3+

to iron (II) ions, Fe2+.

1.Pour 4 cm³ of FeCl3

solution into a boiling tube.

2.Add half a spatula of zinc powder and warm the mixture gently.

3.Cool the mixture and then filter it.

4.Divide the filtrate equally into 3 separate test tubes.

5.Test the solutions with :

i NaOH solution

ii Potassium hexacyanoferrate (II) solution

iii Potassium hexacyanoferrate (III) solution.

6.Record all the observations

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