To determine the correct options to represent the reaction of zinc oxide with carbon to produce zinc and carbon dioxide, we can start with the balanced chemical equation for the reaction.
The reaction can be represented by the following balanced equation:
\[ \text{C (s)} + 2 \text{ZnO (s)} \rightarrow 2 \text{Zn (s)} + \text{CO}_2 \text{(g)} \]
From the stoichiometry of the reaction:
- 1 mole of carbon reacts with 2 moles of zinc oxide to produce 2 moles of zinc and 1 mole of carbon dioxide.
If you have 5.00 moles of carbon, you would need: \[ 5.00 , \text{moles C} \times \frac{2 , \text{moles ZnO}}{1 , \text{mole C}} = 10.00 , \text{moles ZnO} \]
Now, we will look at the choices provided:
-
Carbon + Zinc oxide → Zinc + Carbon dioxide (this is a general representation of the reaction and is correct)
-
C (s) + 2 ZnO (s) → 2 Zn (s) + CO2 (g) (this is the correctly balanced chemical equation and is correct)
The other options either have incorrect stoichiometry or incorrect products. Thus, the two correct responses based on your given options are:
- C (s) + 2 ZnO (s) → 2 Zn (s) + CO2 (g)
- Carbon + Zinc oxide → Zinc + Carbon dioxide
These two responses accurately represent the scenario described in the problem.