Alright, let's look carefully at the chemical equation provided and break it down step by step.
The given chemical equation is:
[tex]\[2 \text{Cu}_{(s)} + \text{O}_2{(g)} \rightarrow 2 \text{CuO}_{(s)}\][/tex]
Here’s the step-by-step analysis:
1. Identify Reactants and Products:
- The reactants are [tex]\(2 \text{Cu}_{(s)}\)[/tex] (Copper in solid form) and [tex]\(\text{O}_2{(g)}\)[/tex] (Oxygen gas).
- The product is [tex]\(2 \text{CuO}_{(s)}\)[/tex] (Copper(II) oxide in solid form).
2. Balance the Equation:
- The equation provided is balanced as the number of atoms for each element is equal on both sides.
- For Copper (Cu): There are 2 Cu atoms on the reactant side and 2 Cu atoms on the product side.
- For Oxygen (O): There are 2 O atoms on the reactant side (in [tex]\(\text{O}_2\)[/tex] molecule) and 2 O atoms on the product side (in 2 moles of [tex]\(\text{CuO}\)[/tex]).
3. Interpretation of the Reaction:
- This is a synthesis reaction where oxygen gas reacts with solid copper to form copper(II) oxide.
- The reaction shows that 2 moles of solid copper react with 1 mole of oxygen gas to produce 2 moles of copper(II) oxide.
4. Understanding Context:
- This chemical equation represents an oxidation reaction where Copper (Cu) is oxidized by oxygen ([tex]\(\text{O}_2\)[/tex]) to form Copper(II) oxide (CuO).
Based on this detailed breakdown of the given chemical equation, we confirm that the reaction information is accurately balanced and represented. The solution reflects an understanding of chemical balancing principles, stoichiometry, and the nature of the reaction without needing any numerical or further calculations.
