Question

10 grams of a sample of potassium chlorate gave on complete decomposition, 2.24 litre of oxygen at S.T.P. Calculate the mass of KCl formed and volume of ${\text{O}}_{\text{2}}$ liberated at same time? (KClO${}_3\to$KCl + O${}_2$)

Answer 1

$2KCl{O}_3⟶2KCl+3O_2$ (Volume of $O_2$ liberated $=2.24$ Litres)

Moles of $O_2$ liberated $=\frac{2.24}{22.4}=0.1$ $mole$

Moles of $KCl$ formed $=\frac{2}{3}\times 0.1=0.067$

Mass of $KCl$ formed $=0.067\times 74.5=5$ $gm$