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Application of Gay-Lussac’s Law of Combining Volumes

Gay Lussac’s of combining volumes states that gases react in simple ratio with one another and to volumes of the products provided that temperature and pressure remain constant. In this article, you will understand how to apply this law in calculation by studying the following examples below: 1.     2H 2 + O 2 → H 2 O In the reaction above, what volume of hydrogen would be left over when 300cm 3 of oxygen and hydrogen are exploded in a sealed tube?   1cm 3 of oxygen = 2cm 3 of hydrogen 300cm 3 of oxygen = 2 x 300 = 600cm 3 Volume of left over = 1000 – 600 = 400cm 3 2.     Calculate the volume of carbon (II) oxide required to react with 40cm 3 of oxygen. 2CO + O 2 → 2CO 2 1cm 3 of oxygen = 2cm 3 of CO 40cm 3 of oxygen = 2 x 40 = 80cm 3 3.     Calculate the volume of residual gases that would be produced when 100cm 3 of sulphur (IV) oxide reacts with 20cm 3 of oxygen    2SO 2 + O 2 → 2SO 3 1cm 3 of O 2 = 2cm 3 20cm 3 of O 2 = 2 x 20 = 40cm 3

Analysis of two unknown inorganic compounds

 

Question

C and D are samples of two different simple salts. Carry out the following exercises on them. Record your observations and identify any gases evolved. State the conclusion you draw from the result of each test.

A)    Heat about one half of C in dry test tube until no further change is observed. Allow to cool

B)     (I)  to the cooled residue from (a) above, add about 5 cm3 of dilute hydrochloric acid and warm.

(II)  to about 2cm3 of the clear solution from (b)(I) above, add aqueous ammonia in drops until it is excess.

C)    Put all D in a boiling tube and add about 10 cm3 of distilled water. Shake thoroughly and divide into two portions.

D)    (I) to the first portion from (C) above, add about 2 cm3 of barium chloride solution, followed by dilute hydrochloric acid in excess. Warm the mixture.

(II) to the second portion from ( C) above, add 2 to 3 drops  of acidified  potassium tetraoxomanganate (VII) solution and shake. (The question is credit to West Africa Senior Secondary Certificate Examination)

 Answer

C is Copper trioxocarbonate (IV) and D is sodium trioxosulphate (IV)

 

S\n

Test

Observation

Inference

A (I)

C  + heat

Colourless ,odourless gas which is acidic to litmus paper and turned lime water milky

CO2, present, CO32-,HCO3- present

(II)

On cooling

green colour turned to black

Oxide of Cu, sulphide of Cu, Pb and carbon likely present

B(I)

Black residue + dil.HCl + heat.

No gas evolved,  dissolved to give a blue solution

Sulphide absent, carbon absent, soluble chloride present

(II)

Solution from (b)(I) +aqueous ammonia in drops till excess

Pale blue precipitate in drops but soluble in excess to form a deep blue solution

Cu2+ confirmed

C(I)

D + water divide into two portions

Dissolved and formed a colourless solution

Soluble salts Na+,K+,NH4+ likely present

D(I)

To the first portion of solution from (C) above + dil. Barium chloride + dil. HCl +heat

White precipitate formed which dissolved in dil. HCl and produced a colourless gas with irritating smell

SO42- absent, CO32-     and HCO3- absent, SO32- and SO2 likely present

(II)

To the second portion add acidified KMnO4 solution and shake

It decolourized KMnO4 ,purple colour turned colourless)

SO2, SO32- confirmed

 

Explanation of the result\inference

A.    In test (a)(I) C liberated a gas which turned lime water milky. this  means that carbon (IV)oxide is present and this gas can only come from Trioxocarbonates or hydrogen carbonates

B.      In test (a)(II)the black residue can be one of the following compounds, CuO, Cus, PbS, or carbon which are common black compounds.

C.    In test (b)(I) the black residue dissolved in warm dil. HCl without giving off gas suggested that sulphide, and lead ions are likely to be absent. This is because lead has insoluble chloride while sulphide liberates hydrogen sulphide gas when heated with dil. HCl.

D.     In test (b)(II) the solution from b(I) formed pale blue precipitate which was soluble in excess aqueous ammonia to form deep blue solution. This shows that copper ions are present.

E.      In test (c)(I)D dissolved in water and it gave colourless solution. This means that insoluble salts are not present. The possible ions might be sodium ions, potassium ions and ammonia ions. This is because they are always soluble in every case.

F.       In test (d)(I) the solution plus barium chloride and dil. Hydrochloric acid plus heating. The white precipitate formed became soluble and produced a gas which has an irritating smell. This means that SO42- and carbonate are absent. Trioxosulphate (IV) and SO2 likely present.

G.    In test (d)(II) the solution decolorized KMnO4. This means that SO2 and trioxosulphate (IV) are present. Note hydrogen sulphide can do the same but with yellow deposit of sulphur.

 

 

 

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