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0.1 Faraday of electricity was passed through a solution of copper (II) sulphate. The maximum weight of copper deposited on the cathode would be ______ (Cu = 64) 

A. 3.2 g   B. 32.0 g    C. 16.0 g    D. 6.4

If the change in free energy of a system is -899 Jmol-1 and the entropy change is 10 Jmol-1k-1 at 25°C, calculate the enthalpy change.

A. +2081 Jmol-1   B. -2081 Jmol-1   C. -649 Jmol-1   D. +649 Jmol-1


On oxidizing anhydrous iron (II) sulphate, in addition to producing iron (III) oxide, which of the following is produced?  

A. SO2(g) + FeS(s).     B. SO3(g) + FeS(s).    C. SO2(g) + SO3(g)     D. SO2(g) + H2S(g)

Which of the following statements applies during the electrolysis of sodium hydroxide solution using platinum electrodes?  

A. Na+ ions are discharged at the cathode
B. Hydrogen ions are discharged at the anode
C. The concentration of sodium hydroxide decreases at both electrode compartments
D. The concentration of sodium hydroxide increases at the cathode only

A compound contains 40.0% C, 6.7% H and 53.3% O. If the molecular mass of the
compound is 180, its molecular formula is _______ [C = 12, H = 1, O = 16]

A. CH2O    B. C3H6O3    C. C6H6O3    D. C6H12O6.


Fehling’s solution can be used to distinguish between

(a) CH3CHO and C2H5OH
(b) CH3COCH3 and CH3COOCH3
(c) CH3CHO and CH3COCH3
(d) C2H5OH and CH2CH2COOH


The general formula of haloalkanes where X represents the halide is

A. CnH2n-1X.     B. CnH2nX.       C. CnH2n+2X.     D. CnH2n+1X.


The constituent of baking powder that makes the dough to rise is ________

A. NaHCO3    B. NaOH    C. Na2CO3    D. NaCI.


Which of the following is a deliquescent compound?

A. Na2CO3    B. CaCl2     C. CuO .    D. Na2CO3. 10H2O


The periodic classification of the element is an arrangement of the elements ¡n order of their ____ 

A. atomic weights    B. isotopic weights    C. molecular weights    D. atomic numbers

Five compounds R, T, W, X, and Y form the following compounds:  

i. a basic hydride R.H,
ii. anacidic hydride YH,
iii. amphoteric oxide W2O3, XO2.

Which of the elements is an alkali?  

A. R    B. T   C. W   D. X

Which of the following questions is correct about the periodic table?

A. The non-metallic properties of the elements tend to decrease across each period.
B. The valence electrons of the elements increase progressively across the period.
C. Elements in the same group have the same number of electron shells.
D. Elements in the same period have the same number of valence electrons.


An element X has electron configuration 1s2 2s2 2p6 3s2 3p5. Which of the following statements is correct about the element?

A. It has a completely filled p-orbital.
B. It has 5 electrons in its outermost shell
C. It belongs to group II on the periodic table.
D. It is a halogen.



The IUPAC nomenclature of the compound above is ______

A. 2-bromo-3-chlorobutanol.
B. 3-bromo-2-chlorobutanol.
C. 3-chloro-2-bromobutanol.
D. 2-chloro-3-bromobutanol.



In the reaction above, an ¡increase in temperature will

A. increase the value of the equilibrium constant
B. decrease the value of the equilibrium constant
C. increase the reactant production
D. shift the equilibrium to the left.


Which of the following metals cannot replace hydrogen from water or steam?  

A. Sodium      B. Magnesium      C. Copper      D. Calcium

Weighed salts Y and Z were left exposed in the laboratory overnight. In the morning Y had gained weight, and Z had become liquid. What conclusion could be drawn about the nature of the two salts?

A. Z is efflorescent
B. Y and Z are efflorescent
C. Y and Z are deliquescent.
D. Y and Z are hygroscopic

Polystyrene is widely used as packaging materials for fragile objects during transportation because of its

A. lightness.   B. low density.   C. high density.   D. high compressibility.


Which of the following will produce a solution with pH less than 7 at equivalent point?

A. HNO3 + NaOH.    B. H2SO4 + KOH.    C. HCI + Mg(OH)2.    D. HNO + KOH.


2Na2O2(s) + 2H2O(l) → 4NaOH(s) + O2(g)

The substance that is oxidized in the reaction above is ______

A. 2Na2O2(s)    B. NaOH(aq)     C. H2O(l)    D. O2(g)



The compound above exhibits

A. geometric isomerism    B. optical isomerism    C. structural isomerism    D. positional isomerism.


Beryllium and aluminium have similar properties because they _______

A. are both metals.
B. belong to the same group.
C. belong to the same period.
D. are positioned diagonally to each other.


Bronze is preferred to copper in the making of medals because it ______

A. is stronger    B. can withstand low temperature     C. is lighter     D. has low tensile strength.


By means of filtration, one component can be obtained pure from an aqueous mixture of sodium chloride and ______ 

A. potassium nitrate    B. sand    C. lead nitrate    D. sugar (glucose)

How many cations will be produced from a solution of potassium aluminium tetraoxosulphate (VI)?

A. 3    B. 4   C. 1   D. 2


When carbon dioxide is bubbled into limewater a white precipitate ¡s formed. If the passage of the gas is continued the precipitate disappears. The reason for this is ______ 

A. calcium carbonates formed which on reaction dissolves
B. calcium hydrogen carbonate is precipitated and then dissolves
C. calcium carbonate is formed which on reaction with further carbon dioxide forms soluble calcium hydrogen carbonate
D. concentration of the solution has occurred with the deposition of calcium hydroxide

The main product of the reaction between phosphorus(V) chloride and ethanol is

(a) chloroethane    (b) chloromethane    (c) dichloromethane    (d) chloroethene


Given that M is the mass of a substance deposited during electrolysis and Q is the quantity of electricity consumed, then Faraday’s first law can be written as _________

The structural formula of ethanoic acid is ______


Water is said to be temporarily hard when it contains ________

A. Ca(HCO3)2 and Mg(HCO3)3 salts.
B. Ca(HCO3)2 and CaCO3 salts.
C. Mg(HCO3)2 and CaSO4 salts.
D. CaSO4 and Ca(HCO3)2 salts


In the deduction of ethyl ethanoate with LiAlH4, the product obtained is ______

(a) ethanol    (b) ethane    (c) ethanoic acid    (d) ethane


The vapour density of a gas may be defined as _______

A. the mass of a unit volume of the gas compared to an equal volume of water vapour
B. the mass of a unit volume of the gas compared to an equal volume of hydrogen
C. the mass of a unit volume of the gas compared to an equal volume of oxygen
D. the mass of a unit volume of the gas minus the vapour pressure of water

If excess zinc is added to a bluish green solution of copper (II) sulphate, and the excess zinc filtered off after completion of reaction, a colourless solution is obtained because ______

A. both zinc and copper are metals
B. the sulphate radical and the zinc ion are divalent
C. zinc is more electropositive than copper
D. both zinc and copper form depositive ions in solution

The final oxidation product of alkanol, alkanal and alkanones is _______

A. alkanoic acid     B. alkanoyl halide     C. alkanoate      D. alkanamide



The diagram above best illustrates the effect of decrease in ______

A. concentration   B. temperature    C. surface area    D. pressure.


The molecular lattice of iodine is held together by _______

A. dative bond     B. metallic bond    C. hydrogen bond    D. van der Waal’s forces.


The mathematical expression of pH is _______


An organic compound has an empirical formula CH2O and vapour density of 45. What is its molecular formula? [C=12, H=1, 0=16]

A. C3H7OH    B. C2H5OH    C. C3H5O3    D. C2H4O2


The IUPAC name for

  is _______

A. 2-methylbut-3-ene    B. 2-methylbut-4-ene   C. 3-methylbut-2-ene    D. 3-methylbut-1-ene

An experimental test of the Law of Conservation of Mass is illustrated in the diagram.  


In practice, the flask is weighed before and after reaction between solutions X and Y. Which of the following pairs of solutions will be unsuitable for the experiment?  

A. X = hydrochloric acid; Y = silver nitrate
B. X = barium chloride; Y = dilute sulphuric acid
C. X = hydrochloric acid; Y = sodium carbonate
D. X = hydrochloric acid; Y = lead nitrate

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