At given temperature and pressure the
volumes of all gaseous reactants and products bear a simple whole number ratio
to each other.
For example:
I.e. one volume of hydrogen reacts
with one volume of chlorine to form two volumes of HCl gas. I.e. the ratio by
volume which gases bears is 1:1:2 which is a simple whole number ratio.
Similarly other examples are:
ILLUSTRATIVE EXAMPLE (14): In the reaction
the ratio of volumes of nitrogen, hydrogen
and ammonia is 1: 3 : 2. These figures illustrate the law of:
(A) Constant proportions (B) Gay-Lussac
(C)
Multiple proportions (D)
reciprocal proportions
SOLUTION: The above ratio of 1: 3: 2 illustrates the
Gay-Lussac law of combining volume.
Hence
(B) is correct.
ILLUSTRATIVE EXAMPLE (15): How much volume of oxygen will be required for
complete combustion of 40 ml of acetylene (C2H2) and how
much volume of carbon dioxide will be formed? All volumes are measured at NTP.
SOLUTION:
So for complete combustion of 40 ml of
acetylene, 100 ml of oxygen are required and 80 ml of CO2 is formed.
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