Certainly! Let's analyze the balanced chemical equation step-by-step:
[tex]\[ 2 \text{Cu}_{(s)} + \text{O}_2 \cdots 2 \text{CuO}_{(s)} \][/tex]
1. Identify the Reactants and Products:
- Reactants: Copper (Cu) in the solid state and Oxygen (O₂) in the gaseous state.
- Products: Copper Oxide (CuO) in the solid state.
2. Stoichiometric Coefficients:
- The coefficients in the balanced equation tell us the ratio in which the reactants combine and the products are formed.
- 2 moles of Copper (Cu) react with 1 mole of Oxygen (O₂) to produce 2 moles of Copper Oxide (CuO).
3. Interpret the Coefficients:
- For every 2 moles of Copper used, 1 mole of Oxygen is consumed, and 2 moles of Copper Oxide are produced.
4. Given Data:
- From the balanced chemical equation, we start with:
- 2 moles of Copper (Cu).
- 1 mole of Oxygen (O₂).
- These react completely to form:
- 2 moles of Copper Oxide (CuO).
5. Molecular Interaction:
- When the reaction occurs, the copper atoms and oxygen molecules interact in the ratio specified by the coefficients.
- Specifically, 2 copper atoms combine with 1 molecule of oxygen (O₂) to form 2 units of copper oxide (CuO).
6. Summary:
- Initial moles of copper (Cu): 2 moles.
- Initial moles of oxygen (O₂): 1 mole.
- Moles of copper oxide (CuO) produced: 2 moles.
So, the reaction starts with 2 moles of Copper and 1 mole of Oxygen and results in the formation of 2 moles of Copper Oxide.
Therefore, the moles of the reactants and products are as follows:
- Moles of Copper (Cu) initially = 2
- Moles of Oxygen (O₂) initially = 1
- Moles of Copper Oxide (CuO) produced = 2
