A sample of gas contains 0.1135 mol of
H2(g) and 0.1135 mol
of O2(g) and occupies a volume of
11.3 L. The following reaction takes place:
H2(g) + O2(g)
---->
H2O2(g)
Calculate the volume of the sample after the reaction takes place,
assuming that the temperature and the pressure remain constant.
_____ L
Given reaction :
H2(g) + O2(g) ----> H2O2(g)
NH2 = 0.1135 and NO2 = 0.1135
It is stoichiometrically balanced.
One mol of hydrogen gas reacts with 1 mol of oxygen gas to form 1 mol of hydrogen peroxide gas.
So 0.1135 mol of hydrogen gas reacts with 0.1135 mol of oxygen gas to form 0.1135 mol of hydrogen peroxide gas.
Avogadro's Law states that at constant temperature and pressure volume occupied by a gas is directily proportional to its amount. It also means equal amount of gas will occupy voulume.
Since,
NH2 = NO2 = NH2O2
So, VH2 = VO2 = VH2O2
Also it is given that
VH2 + VO2 = 11.3 L
Hence volume of sample after reaction takes place i.e. volume of H2O2 gas, is 5.65 L.
PLEASE UPVOTE
THANKS
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