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NAME…………………………………………………………………. INDEX NO…………………………………………………………
SCHOOL……………………………………………………………………………………………………………………………………….
SIGN……………………………………………………………………………………………..…DATE ……………………………
233/1
CHEMISTRY
PAPER 2
2 HRS
JULY 2019
CHANIA ZONEJOINT INTER-SCHOOLS EVALUATION TEST
(CZJISET)INSTRUCTIONS TO CANDIDATES
[a]Answer ALL questions in the spaces provided in each question.
[b] Mathematical tables and electronic calculators may be used for calculations.
[c]All working must be clearly shown where necessary.
FOR EXAMINERS ONLY
QUESTION MAXIMUM SCORE CANDIDATES SCORE1 112 113 84 125 126 157 12Total
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1. The diagram below shows spots of pure substance A,B and C on a chromatography paper. Spot D is that of a mixture.
After development ,A,B and C were found to have moved 8cm,3cm and 6cm respectively D was separated into two spots which had moved 6cm and 8cm.
On the diagram
[i][a]Label the baseline (origin). [1mk]
[b]Show the positions of all the spots after development. [3mks]
[ii]Identify the substances present in the mixture D. [2mks]
[b]Describe how solid ammonium chloride can be separated from a solid mixture of ammonium chloride and anhydrous calcium chloride. [2mks]
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[c]The table below shows liquids that are miscible and those that are immiscible.
liquid L3 L4L1 Miscible MiscibleL2 Miscible Immiscible
Use the information given to answer the questions that follow
[i]Name the method that can be used to separate L1 and L3 from the mixture of the two.[1mk]
[ii]Describe how a mixture of L2 and L4 can be separated. [2mks]
2. An ore is suspected to contain mainly iron. Describe a method that can be used to confirm the presence of iron in the ore. [3mks]
[b]Excess carbon (ii) oxide gas was passed over a heated sample of an oxide of iron as shown below. Study the diagram and answer the questions that follow.
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Mass of empty dish=10.98g
Mass of empty dish +oxide of iron=13.30g
Mass of empty dish +residue=12.66g
[i]Determine the formula of the oxide of iron. (Relative formula mass of iron oxide=232, Fe=56.0, O=16.0) [3mks]
[ii]Write an equation for the reaction which took place in the dish. [1mk]
[c]Corrosion is a destructive process in which iron is converted into hydrated iron (III) oxide. State:
[i]Two conditions necessary for rusting to occur. [1mk]
[ii]One method used to protect iron from rusting. [1mk]
[d]Explain why it is not advisable to wash vehicles using sea water. [2mks]
3.[a]State the Hess’s law. [1mk]
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[b]The enthalpies of combustion of calcium, carbon and decomposition of calcium carbonate are indicated below:
C[s]+12O [2][g] → CaO[s]: ∆H =-635KJmol-1
C[S]+O2[g] → CO2[g] ∆H =-394KJmol-1
Enthalpy of decomposition of Ca CO3=+178KJmol-1
[i]Draw an energy cycle diagram that links the enthalpy of formation of calcium carbonate to enthalpies of combustion of calcium, carbon and decomposition of calcium carbonate. [2mks]
[ii]Determine the enthalpy of formation of calcium carbonate. [2mks]
[c]Some average bond energies are given below.
Bond energy in KJmol-1
C-C 348
C-H 414
Cl-Cl 243
C-Cl 432
H-Cl 340
Calculate the energy change for the reaction below. [3mks]
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C2H6(g)+Cl2(g) → CH3CH2Cl(g)+HCl(g)
4. Use the standard electrode potentials for A, B, C, D andF given below to answer the questions that follow.
Eθ (Volts)
A2+[aq] +2e ⇋ A[s] -2.90
B2+[aq]+2e ⇋ B[s] -2.38
C+[aq]+2e ⇋ 1
2C2[g] 0.00
D2+[aq]+2e ⇋ D[s] +0.34
12F2[g]+e- ⇋ F-
[aq] +2.87
[I]Which element is likely to be hydrogen? Give a reason for your answer. [2mks]
[ii]What is Eθfor the strongest reducing agent? [1mk]
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[iii]Calculate the e.m.f of the cell that would be formed when half cells of Band D are combined.[1mk]
[b]Aqueous copper (II) sulphate was electrolysed using the set shown below.
[i]When the switch was closed, a gas was produced at electrode B.Which electrode is the anode?[1mk]
[ii]Write the half equation for the reaction at electrode B. [1mk]
[iii]What happens to the pH of the electrolyte above during electrolysis? Explain. [2mks]
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[i]If carbon electrode were replaced with copper electrodes in the cell above, write the equation for the reaction that would occur at the anode. [1mk]
[c]During electrolysis of copper [II] sulphate using copper electrodes, a current of 0.2 ampheres was passed through the cell for 5 hours. Determine the change in mass of the cathode that occurred as a result of the electrolysis process. (Cu=64, IF=96500C). [3mks]
5. The grid below is part of the periodic table. Letters are not actual symbols. Study it and answer the questions that follow.
[i]Give the letters representing atoms that can form a singly charged ion. [1mk]
[ii]Identify the most electronegative element in the grid. Explain. [2mks]
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[iii]Identify the strongest reducing agent. [1mk]
[iv]Write the formula of the most stable compound formed when J and K react. [1mk]
[v]Give the name of the type of bond in the compound formed in (IV) above. [1mk]
[vi]Give the chemical family name of L and M. [1mk]
[vii]Write the ionic equation for the reaction in which gas L is bubbled through a solution with ions of M. [1mk]
[viii]Element P is an alkaline earth metal and belongs to periodic 2.Indicate its position on the grid.[1mk]
[b]Use the information in the table below to answer the questions that follow.
ELEMENT ATOMIC NUMBER MELTING POINT(°C ¿Q 11 98R 12 650S 14 1410T 17 -102
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U 18 -189V 19 64
Give a reason why the melting point of
[i]Q is higher than of V. [1mk]
[ii]R is higher than Q. [1mk]
[iii]S is the highest [1mk]
6. Study the flow chart below and answer the questions that follow.
[a][i]Name the type of reaction in the following steps.
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I Step III [1mk]
IIstep IV. [1mk]
[ii]Name the important reagents and conditions in
Step1: Reagent [1mk]
Condition [1mk]
Step II: Reagent [1mk]
Condition [1mk]
Step V: Reagent [1mk]
Condition [1mk]
[b][i]Write a balanced equation for the reaction taking place in
Step VI. [1mk]
Step VII [1mk]
[ii]Give the systematic name of liquid X and substance L
Liquid X [1mk]
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Substance L [1mk]
[c][i]If the relative molecular mass of compound formed in step III is 42 000, determine the value of n in the compound. (C=12.0, H=1.0). [2mks]
[ii]State one disadvantage of continued use of items made from the compound formed in d (i) above.[1mk]
7. Use the flow chart below to answer the questions that follow.
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[A]Name:
[i][a]Substance C [12mk]
[b]Compound K [12mk]
[ii]Write the formula of compound K. [1mk]
[B]The following set-up is used to prepare nitric [v] acid in the laboratory.
[i]All the apparatus used during preparation of nitric [v]acid are made by glass. Give a reason.[1mk]
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[ii]Name solid Q. [1mk]
[iii]Give a reason why it is possible to separate nitric (v) acid from the sulphuric (VI) acid used as one of the reagents. [1mk]
[vi]Give 2 uses of Nitric (v) acid [2mks]
[c]In an experiment 1200cm3 of ammonia gas measured at r.t.p reacted completely with copper (ii) oxide. Calculate
[i]The mass of copper formed given the formula of reaction. [3mks]
3CUO[s]+2NH3 [g] → 3CU [s]+3H2O[l]+N2[g]
[ii]The volume of Nitrogen gas formed N=14, H=1.0, O=16.0) [2mks]
CU=64MGV at r.t.p=24 dm3.
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