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How many grams of FeS are formed from 7.62g of Fe reacted with excess S?

User Hendekagon
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2 Answers

23 votes
23 votes

Final answer:

0.136 moles of FeS will be formed from 7.62g of Fe.

Step-by-step explanation:

To determine how many grams of FeS are formed from 7.62g of Fe reacted with excess S, we need to use the balanced chemical equation for the reaction. The balanced equation is:

Fe + S → FeS

From the equation, we can see that the mole ratio between Fe and FeS is 1:1. Therefore, the number of moles of FeS formed will be the same as the number of moles of Fe.

To calculate the number of moles of FeS, we divide the mass of Fe by its molar mass:

moles of Fe = mass of Fe / molar mass of Fe = 7.62g / 55.85g/mol = 0.136 mol

Therefore, 0.136 moles of FeS will be formed from 7.62g of Fe.

User Chol Nhial
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2.7k points
14 votes
14 votes

Answer:

12.2g

Step-by-step explanation:

I took the quiz :)

User Jon Cahill
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2.9k points