The following balanced equation tells us that [tex]$8.0 \, \text{mol}$[/tex] of [tex]$Cu$[/tex]
[tex]\[
2 \, \text{Cu (s)} + \text{O}_2 \, (\text{g}) \rightarrow 2 \, \text{CuO (s)}
\][/tex]
A. reacts with [tex]$4.0 \, \text{mol}$[/tex] of [tex]$\text{O}_2$[/tex]
B. produces [tex]$8.0 \, \text{mol}$[/tex] of [tex]$\text{CuO}$[/tex]
C. cannot react with oxygen
D. produces [tex]$16.0 \, \text{mol}$[/tex] of [tex]$\text{CuO}$[/tex]