Chemistry

Problem

A vessel of 2.50 litre was filled with 0.01 mole of

\text{Sb}_2\text{S}_3

and 0.01 mole of

\text{H}_2

to attain the equilibrium at

440^\circ\text{C}

as :

\text{Sb}_2\text{S}_3(\text{s}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{Sb}(\text{s}) + 3\text{H}_2\text{S}(\text{g})

After equilibrium the

\text{H}_2\text{S}

formed was analysed by dissolving it in water and treating with excess of

\text{Pb}^{2+}

to give 1.029 g of

\text{PbS}

as precipitate. What is value of

K_C

of the reaction at

440^\circ\text{C}

? (Atomic mass of

\text{Pb} = 206

)