Question

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

Answer 1

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.

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