Question

Concentrated hydrogen peroxide solutions are explosivelydecomposed by traces of transition metal ions

2H2O2(aq) -> 2H2O(l)+O2
what volume of pure O2 collected at 27 C and 764 torr would begenerated by decomposition of 125 grams of a 50% by mass hydrogenperoxide solution?
Ignore any water vapor that may bepresent.

Answer 1

22.52 liters volume of pure oxygen gas will be collected at 27°C and 764 Torr.

Step-by-step explanation:

Mass of hydrogen peroxide solution = 125 g

Mass of hydrogen peroxide in solution = 50% of 125 g ;

`(50)/(100)* 125 g=62.5 g`

Moles of hydrogen peroxide =
`(62.5 g)/(34 g/mol)=1.838 mol`

`2H_2O_2(aq)\rightarrow 2H_2O(l)+O_2(g)`

According to reaction, 2 moles of hydrogen peroxide gives 1 mole of oxygen gas.

Then 1.838 moles of hydrogen peroxide will give:

`(1)/(2)* 1.838 mol=0.919 mol` of oxygen gas .

Moles of oxygen gas = n = 0.919 mol

Pressure of oxygen gas , P= 764 Torr=
`(764)/(760)atm=1.005 atm`

Volume of oxygen gas = V = ?

Gas constant , R= 0.0821 L.atm/mol.K

Temperature of oxygen gas = 27°C=27+273 K=300 K

Using ideal gas equation:

PV = nRT

Putting values in above equation, we get:

`V=(nRT)/(P)`

`=(0.919 mol* 0.0821 atm L/mol K* 300 K)/(1.005 atm)`

V = 22.52 L

22.52 liters volume of pure oxygen gas will be collected at 27°C and 764 Torr.