Question

In the conversion of 0.01 mole of PbS PbSO4; the volume of 10 volume hydrogen peroxide required is

Answer 1

The reaction is
4H2O2 + PbS →→→ 4H2O + PbSO4

Thus 0.01 mole PbS reacts with 0.01*4 i.e. 0.04 moles of H2O2

Thus volume of H2O2 needed
= 0.04*11.2/10 = 0.0448 L or 44.8mL

Answer 2

To convert Lead Sulphide (PbS) to Lead Sulphate $\left(\mathrm{PbSO}_{4}\right)$ four molecules of Hydrogen Peroxide is reacted with one molecule of Lead Sulphide (PbS) to produce 4 molecules of water and one molecule of Lead Sulphate $\left(\mathrm{PbSO}_{4}\right)$.

The ratio of Lead Sulphide (PbS) and Hydrogen Peroxide $\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)$ used is 1 : 4. Therefore, 0.01 mole of PbS reacts with 0.04 mole of $\mathrm{H}_{2} \mathrm{O}_{2}$. Therefore, the volume of “10 Volume”.  

$\begin{array}{l}{\mathrm{H}_{2} \mathrm{O}_{2} \text { required }=\frac{(0.04 \times 11.2)}{10}} \\ {=0.0448 \mathrm{L} |}\end{array}$

= 44.8 mL.