The mass of 10% hydrogen peroxide solution, which is required

The mass of 10% hydrogen peroxide solution, which is required to obtain the oxygen required for the complete oxidation of 5.6 liters of acetylene.

1. Let’s write down the equations of the proceeding reactions:

2H2O2 = 2H2 + O2;

2C2H2 + 3O2 = 4CO2 + 2H2O;

2.Calculate the chemical amount of oxidizable acetylene:

n (C2H2) = V (C2H2): Vm = 5.6: 22.4 = 0.25 mol;

3. Determine the amount of oxygen that went into the reaction:

n (O2) = n (C2H2) * 3: 2 = 0.25 * 3: 2 = 0.375 mol;

4. find the amount of hydrogen peroxide decomposed:

n (H2O2) = n (O2) * 2 = 0.375 * 2 = 0.75 mol;

5.Calculate the mass of peroxide:

m (H2O2) = n (H2O2) * M (H2O2);

M (H2O2) = 2 + 32 = 34 g / mol;

m (H2O2) = 0.75 * 34 = 25.5 g;

6.Set the mass of the hydrogen peroxide solution:

m (solution) = m (H2O2): w (H2O2) = 25.5: 0.1 = 255 g.

Answer: 255 g.