Question

Given below are the steps for extraction of copper from its ore. The balance reaction involved in -

Roasting of copper(I) sulphide is:

• A. $2C{u}_{2}S\left(s\right)+3O_2\left(g\right)\stackrel{Heat}{\to }2C{u}_{2}O\left(s\right)+2S{O}_2\left(g\right)$
• B. $C{u}_{2}S\left(s\right)+3O_2\left(g\right)\stackrel{Heat}{\to }C{u}_{2}O\left(s\right)+2S{O}_2\left(g\right)$
• C. $2C{u}_{2}S\left(s\right)+2O_2\left(g\right)\stackrel{Heat}{\to }2C{u}_{2}O\left(s\right)+2S{O}_2\left(g\right)$
• D. $C{u}_{2}S\left(s\right)+2O_2\left(g\right)\stackrel{Heat}{\to }C{u}_{2}O\left(s\right)+S{O}_2\left(g\right)$

Answer 1

Answer: (A)

$2C{u}_{2}S\left(s\right)+3O_2\left(g\right)\stackrel{Heat}{\to }2C{u}_{2}O\left(s\right)+2S{O}_2\left(g\right)$

During roasting, the sulfide is converted to an oxide, and sulfur is released as sulfur dioxide, a gas.

For the ores $C{u}_{2}S$ (chalcocite) and $ZnS$ (sphalerite), balanced equations for the roasting are:

$2C{u}_{2}S\left(s\right)+3O_2\left(g\right)\stackrel{Heat}{\to }2C{u}_{2}O\left(s\right)+2S{O}_2\left(g\right)$

Option A is correct.