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)
a. 2
b. 3
c. 8
d. 12
e. 20

Explanation:

Step1: Analyze the stoichiometry of the reaction

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 to form 4 moles of \(Cu_{(s)}\).

Step2: Calculate the moles of \(Cu_{(s)}\) formed

If we have 3 moles of \(C_{(s)}\), using the mole - ratio from the balanced equation. The ratio of \(n(C):n(Cu)=1:4\). So if \(n(C) = 3\space mol\), then \(n(Cu)=4\times n(C)\)

$$n(Cu)=4\times3\space mol = 12\space mol$$

Answer:

d. 12