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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]



Answer :

GinnyAnswer
Alright, let's analyze the given balanced chemical equation step-by-step to determine the correct answer:

[tex]\[2Cu(s) + O_2(g) \rightarrow 2CuO(s)\][/tex]

1. Balanced Equation: The balanced chemical equation tells us that 2 moles of copper (Cu) react with 1 mole of oxygen (O_2) to produce 2 moles of copper(II) oxide (CuO).

2. Given Information: We are given that there are 8.0 moles of copper (Cu).

3. Stoichiometric Ratios: According to the balanced equation,
- 2 moles of Cu produce 2 moles of CuO.
- This establishes a 1:1 molar ratio between Cu and CuO.

4. Calculating Moles of CuO Produced:
- Since the ratio is 1:1, 8.0 moles of Cu will produce 8.0 moles of CuO.

So, based on the analysis:

- 8.0 moles of Cu will react to produce 8.0 moles of CuO.

Therefore, the correct answer from the given options is:

8.0 moles of Cu produces 8.0 moles of CuO.

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