Messages posted by WrenchR

10 c.c of a mixture of hydrogen , carbon monoxide, and carbon dioxide mixed with 15cc of oxygen and exploded. The resulting mixture of gases was cooled to the original room temperature and pressure and measured 19 cc. On shaking with potash a further contraction to 12cc took place. Deduce the composition of mixture.

solution:

Let x cc = volume of hydrogen

ycc = volume of CO

z cc = Volume of CO2 [10-(x+y)]

On explosion, the following reactions occur:

2H_{2 +} O₂ = 2H₂O

x cc (x/2) cc (condensed to occuppy a negligible volume)

2CO + O₂= 2CO₂

ycc (y/2)cc y cc

Since the contraction on shaking with potash is due solely to the absorption of CO_2,

y+10-(x+y)=7

x = 3

The equations can now be written as :

2H_{2 +} O₂ = 2H₂O

3cc + 3/2 cc (condensed)

2CO + O₂= 2CO₂

_{ycc y/2 cc ycc}

So volume of oxygen required for complete combustion = (3/2 + y/2) cc and since 15 cc of oxygen were originally present and 12 cc of oxygen remain

so 3/2 + y/2 = 3 ------- (1)

y=3 and z=4

Now somebody please explain how 12cc of oxygen remains. I didn't understand eqn (1).

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