Blister copper is produced by reaction of copper oxide with copper sulphide.
2Cu2O + Cu2S $\to$ 6Cu + SO2
When 2.86 $\times$ 103 g of Cu2O and 4.77 $\times$ 103 g of Cu2S are used for reaction, the mass of copper produced is _____________ g. (nearest integer)
(Atomic mass of Cu = 63.5 a.m. u, S = 32.0 a.m. u, O = 16.0 a.m. u)
Answer (integer)
3810
Solution
moles of $\mathrm{Cu}_{2} \mathrm{O}=\frac{2.86 \times 10^{3}}{143}=20$
<br/><br/>
moles of $\mathrm{Cu}_{2} \mathrm{S}=\frac{4.77 \times 10^{3}}{159}=30$
<br/><br/>
$\mathrm{Cu}_{2} \mathrm{O}$ is limiting reagent
<br/><br/>
$$
\begin{array}{lccc}
2 \mathrm{Cu}_{2} \mathrm{O} & + & \mathrm{Cu}_{2} \mathrm{~S} \longrightarrow & 6 \mathrm{Cu} & + & \mathrm{SO}_{2} \\
20 && 30 & - & & - \\
- & &20 & 60 & & 10
\end{array}
$$
<br/><br/>
Mass of copper $=60 \times 63.5=3810 \mathrm{~g}$
About this question
Subject: Chemistry · Chapter: Some Basic Concepts of Chemistry · Topic: Mole Concept
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