Question

1. how many moles of cu(s) form when 3 moles of c(s) reacts with 4 moles of cu₂o according to the following reaction? (4 pts)

c(s) + 2 cu₂o(s) → 4 cu(s) + co₂(g)

Explanation:

Step1: Analyze the reaction stoichiometry

From the balanced chemical equation \(C_{(s)}+2Cu_2O_{(s)}\to4Cu_{(s)} + CO_{2(g)}\), we can see that 1 mole of \(C_{(s)}\) reacts with 2 moles of \(Cu_2O_{(s)}\) to produce 4 moles of \(Cu_{(s)}\).

Step2: Determine the limiting reactant

We have 3 moles of \(C_{(s)}\) and 4 moles of \(Cu_2O_{(s)}\).
For \(C\): If all 3 moles of \(C\) react, based on the ratio \(1:2\) ( \(C:Cu_2O\) ), the moles of \(Cu_2O\) required would be \(3\times2 = 6\) moles. But we have only 4 moles of \(Cu_2O\).
For \(Cu_2O\): Based on the ratio \(2:4\) ( \(Cu_2O:Cu\) ), if we have 4 moles of \(Cu_2O\), the moles of \(Cu\) formed can be calculated.
Using the ratio \(\frac{4\space mol\space Cu}{2\space mol\space Cu_2O}\), when \(n(Cu_2O)=4\space mol\)
\(n(Cu)=\frac{4\space mol\space Cu}{2\space mol\space Cu_2O}\times4\space mol\space Cu_2O\)

Answer:

8 moles of \(Cu_{(s)}\) are formed.