Question

Concentrated hydrogen peroxide solutions are explosively decomposed by traces of transition metal ions (such as Mn or Fe): 2H₂O₂(aq) ---> 2H₂O(l) + O₂(g)

What volume of pure O₂(g), collected at 27°C and 746 torr, would be generated by the decomposition of 125 g of a 50.0% by mass hydrogen peroxide solution?
a. 23.1 L
b. 27.8 L
c. 31.5 L
d. 35.2 L

Answer 1

The volume of pure O2(g) produced by the decomposition of 125g of a 50.0% by mass hydrogen peroxide solution is approximately 0.938 L.

Step-by-step explanation:

To determine the volume of pure O2(g) produced by the decomposition of 125g of a 50.0% by mass hydrogen peroxide solution, we first need to calculate the number of moles of hydrogen peroxide. This can be done using the molar mass of hydrogen peroxide:

Molar mass of H2O2 = 2(1.01) + 2(16.00) = 34.02 g/mol

Now we can calculate the number of moles of H2O2:

Moles of H2O2 = (125g)*(1 mol/34.02g) = 3.675 mol

According to the balanced equation, 2 moles of H2O2 produce 1 mole of O2(g). Therefore, 3.675 moles of H2O2 will produce:

Moles of O2(g) = (3.675 mol)*(1 mol/2 mol) = 1.8375 mol

To convert the moles of O2(g) to volume, we can use the ideal gas law:

Volume of O2(g) = (1.8375 mol)*(0.0821 L/mol*K)*(300K) / (746 torr) = 0.938 L

Therefore, the volume of pure O2(g) produced is approximately 0.938 L.