ANSWERS:
1. 11. (a) (i) Partition law:
“When a solute is dissolved in a mixture of two immiscible solvents, it distributes itself in a constant ratio of concentration”.
(ii) Conditions
1.The two solvents must be completely immiscible.
2. Temperature should be constant.
3. There should be no change in molecular state of the solute i.e. should not dissociate or associate in any of the solvents.
(b) (i) Standard molar enthalpy of formation:
Is the heat change when 1 mole of a substance is formed from its elements in their standard states?
(g) + (g) N (g)
Heat of solution of a substance:
Is the enthalpy change when 1 mole of a substance is added to so much water that further addition of water produces no farther change.
Ionization energy:
Is the energy required to remove the most loosely held electron from the shell of an atom or ion.
(c) (i) Hess’s law:
The enthalpy change for a particular reaction is same whether the reaction takes place in one step or in a series of steps.
(ii) Solution:
Applying Hess’s law
HC = -393 KJ mol-1
HC = +285 KJ mol-1
K.D =
0.0243a = 10-4 -a
1.0243a = 10-4
a = 9.76×10-5 moles
Fraction of Iodine extracted by C will be
= 9.76 x 10-5
1 x 10-4
= 0.976
(iii) Solution:
12.(a) (i) Nucleophilic addition reaction is the reaction in which nucleophile is added
First followed by electrophile.
Elimination reaction is the reaction whereby an atom or group of atoms are removed from a compound
e.g: C C Cl + NaOH C + NaCl + O
C C and C CC OH
By Lucas Test
Propanol will not form cloudness when it undergoes Lucas test but propan -2-ol will form cloudness after 5 minutes upon Lucas test.
(ii) C CH – C and C C C Cl
Using KOH followed by AgN in the presence of HN, yellow ppt will be observed for C C CCl while there is
Cl
No reaction for C CH C
(iii) C C CHO and C C – C C
C C CHO will react with Tollen’s reagent [Ag (N]OH to form a white ppt of silver at the bottom of the test-tube while
CC C – C C will not react.
(c) (i) Propanoic acid from ethane
C CN + O 4
C C – N CH3 C– OH
Propanoic acid
(ii) Propan-2-ol from propan-1-ol
CC C OH + S C CH = C
(iii) Propyne from Ethyne
λ m =
= 133 S cm3 mol
= 6.4×10-3 g cm-1
C = 5 X 10 -2 M
=
1 dm3 = 10 3 cm3
x =1cm3
= 10-3
= =
= =
= 128 S cm-2 mol-1
∝ = O.96
13. Salt hydrolysis is the reaction between salt and water to form an acidic or alkaline solution:
Order of reaction: Molecularity:
– It cannot be determined – Can be determined from the equation
From equation (determined experimentally).
– It can be a whole number or fraction . – It can only be a whole number
– It is the sum of concentrations terms on – It is the number of ions atoms or
Which the rate of reaction actually depends molecules that must collide so as to
(It is sum of exponents of the concentrations results in a chemical reaction.
in the rate law).
– It cannot be obtained from the stoichiometry – It can be obtained from the
Of an unbalanced equation. Stoichiometry of the equation.
= 30 x 60 = 1800s at 27
= 10×60 = 600s at 47
Log =
n log =
log = – 1.088 x 10-5 Ea
= Ea = 4.3833
K =
K =
K = 3.85×10-4
Tollen’s reagent (silver mirror test)
Acyl halides (Acid halide)
Derivatives of carboxylic acids upon hydrolysis go back to carboxylic acids
Transesterification is the reaction between ester and alcohol to form another ester
Conditions for a chemical reaction to take place
i. The collision of the molecules must be energetic enough to break the bonds between the molecule
ii. The colliding molecule must have right orientation (geometry)
Log K1 = log A –
Log K2 = log A –
Log K1 –log K2 = –
Log =
In = Kt =
– = Kt =
Homolytic bond cleavage.
Is the type of bond cleavage in which the covalent bond breaks symmetrically so that are electron moves to each end.
Heterolytic bond cleavage.
Here the covalent bond breaks unsymmetrical and all bonding electrons are taken by the more electronegative atom
(g) + → 2N Slow
R= [] [] this slow step will determine rate law
= [NO] [NO]
= [NO
= []
At equilibrium =
[NO] 2 = []
[NO] 2 = []
R= [NO]2 []
R= K [NO]2 []
The slow step will determine the rate law
R = [Br] []
Consider the equilibrium reaction
= [B]
= [Br] 2
At equation:
=
[B] = [Br]2
[B] =[ Br]2
[Br] = [Br]1/2
R= K0Br1/2
R= K [Br []
Kh =
CCOONa → CCO + N
Start 0.1 0 0
0.1 – x x x
Kh =
α = × 100
[H COONa] =
Let added volume be x
[H COONa] =
0.1=
n=0.1x
[H COONa] =
[HCOOH] =
14. Explain the meaning and significance of colloids
15. Discuss the properties of soil colloids
– Surface area
– Electric charge
– Ion exchange (diagram)
16. Explain the mechanism of ion exchange in soil
17. Calculation of percentage base saturation of a soil sample. With worked examples (how to calculate)
18. Aluminum has high polarizing power hence the compound formed between Al and carbon will be unstable therefore it will decompose immediately after formation.
The chloride outside is not part of the complex meaning that it is ionization. Therefore Ag will react. In [ p(NH3)2 cL4)] the chloride is part of the complex hence there is no ionizable chloride ion and there no reaction
19. (a)(i) CH3 – C-CH3 + CH3 Mg CL CH3 –C- CH3
(ii) CH3 –C- C-CH3 +NaOH + I2 CHI3 + NaOOC – CONa + NaI
(iii) CH3 CH2 C – NH2
CH3 CH2 NH2 + KBr +CO2 +H2O
(iv) CH3 CH2 NH2 + CHcL3
CH3 CH2 N =C + HCL
20. Distinguish between
When Br2/H2O is added to phenol, white ppt is formed
When Br2/H2O is added, no reaction
(iv) CH3 CH2 OH +I2 + NaOH No reaction
22. With the aid of chemical equations explain the following
(i) Mercury(ii) iodide solution but not in potassium iodide solution but in water
(ii) The pink solution of cobalt (ii) chloride turns blue when conc. HCL is added gelatinous ppf of
(iii) Copper (ii) hydroxide turns deep blue in excess ammonia
(iv) ZnO and Pbo dissolves in hot conc sodium hydroxide solution
23. using relevant balanced chemical equation describe the process of extracting copper from copper pyrite under the following heading.
(i) Concentration
(ii) Roasting
(iii) Removal of ion impurities
(iv) Self- reduction reaction
24. Cobalt copper, Iron and manganese are d-block elements
a. What is meant by the term d- block element
b. Write E.C of Cu, Fe2+, Mn2+
(i) Explain in terms of E.C why Fe2+ ions are readily oxidized to Fe3+ ions but manganese (ii) ions are not readily oxidized to Mn3+
25. 2.5 x 10-3 moles of a compound with a formula was dissolved in 0.1M a silver nitrate solution. 50 cm3 were required for complete precipitation of the chloride ions present.
(i) Deduce the ionic formula of the compound
(ii) Draw the structure of the complex ion present and name it
26. Write the formula of the following complexes
(i) Tetra ammine copper(ii) Sulphate mono hydrate
(ii)Potassium
27. Write down a balanced chemical equation for the following
(i) Adding of excess ammonia solution to aluminium ion
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