Answer :
Answer:
You would need 9.00 moles of sulfur to obtain 6.00 moles of Fe2S3.
Explanation:
The balanced chemical equation for the formation of iron(III) sulfide (Fe2S3) is:
4 Fe + 3 S -> 2 Fe2S3
The equation shows that it takes 3 moles of sulfur (S) to produce 2 moles of Fe2S3.
So, to obtain 6.00 moles of Fe2S3, you would need:
(6.00 moles Fe2S3 / 2 moles Fe2S3) * 3 moles S = 9.00 moles of sulfur (S)
Therefore, you would need 9.00 moles of sulfur to obtain 6.00 moles of Fe2S3.
Final answer:
To obtain 6.00 moles of Fe2S3, you would need 9.00 moles of sulfur.
Explanation:
To find the number of moles of sulfur needed to obtain 6.00 moles of Fe2S3, we need to use the balanced equation for the reaction:
FeS + 1.5 S → Fe2S3
From the equation, we can see that 1 mole of Fe2S3 contains 1.5 moles of sulfur. Therefore, to obtain 6.00 moles of Fe2S3, we would need:
6.00 moles Fe2S3 * 1.5 moles S / 1 mole Fe2S3 = 9.00 moles of sulfur.
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