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Copper reacts with sulfur to form copper(I) sulfide, according to the balanced equation:

[tex]\[ 2 \text{Cu} + \text{S} \rightarrow \text{Cu}_2 \text{S} \][/tex]

Given that there are [tex]\(40.2 \text{g Cu}\)[/tex] and [tex]\(14.1 \text{g S}\)[/tex], complete the steps below to determine the limiting and excess reactants.

1. How many moles are in [tex]\(40.2 \text{g Cu}\)[/tex]?
[tex]\[ \square \text{ mol Cu} \][/tex]

2. How many moles are in [tex]\(14.1 \text{g S}\)[/tex]?
[tex]\[ \square \text{ mol S} \][/tex]



Answer :

GinnyAnswer
To determine the moles of each substance given their respective masses and molar masses, follow these steps:

1. Molar masses:
- The molar mass of copper (Cu) is [tex]\( 63.55 \, \text{g/mol} \)[/tex].
- The molar mass of sulfur (S) is [tex]\( 32.07 \, \text{g/mol} \)[/tex].

2. Calculate the number of moles of copper:
- Given mass of copper: [tex]\( 40.2 \, \text{g} \)[/tex].
- The formula to calculate moles is:
[tex]\[ \text{moles of Cu} = \frac{\text{mass of Cu}}{\text{molar mass of Cu}} \][/tex]
- Substituting the values:
[tex]\[ \text{moles of Cu} = \frac{40.2 \, \text{g}}{63.55 \, \text{g/mol}} \approx 0.632 \, \text{moles Cu} \][/tex]

3. Calculate the number of moles of sulfur:
- Given mass of sulfur: [tex]\( 14.1 \, \text{g} \)[/tex].
- The formula to calculate moles is:
[tex]\[ \text{moles of S} = \frac{\text{mass of S}}{\text{molar mass of S}} \][/tex]
- Substituting the values:
[tex]\[ \text{moles of S} = \frac{14.1 \, \text{g}}{32.07 \, \text{g/mol}} \approx 0.440 \, \text{moles S} \][/tex]

To summarize:
- There are approximately [tex]\( 0.632 \, \text{moles Cu} \)[/tex] in [tex]\( 40.2 \, \text{g} \)[/tex] of copper.
- There are approximately [tex]\( 0.440 \, \text{moles S} \)[/tex] in [tex]\( 14.1 \, \text{g} \)[/tex] of sulfur.

These values will be used to determine the limiting and excess reactants in the reaction.

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