How Much Chromium(III) Oxide Is Needed for 439g of Chromium Sulfide?

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SUMMARY

The discussion focuses on the stoichiometric calculation required to determine the amount of Chromium(III) Oxide (Cr2O3) needed to produce 439 grams of Chromium Sulfide (Cr2S3). The balanced chemical equation is Cr2O3(s) + H2S(g) = Cr2S3(s) + H2O(l), indicating a 1:1 mole ratio between Cr2O3 and Cr2S3. To find the moles of Cr2O3 required, participants calculated the moles of Cr2S3 in 439 grams, concluding that the same number of moles of Cr2O3 is necessary. Subsequently, they calculated the grams of Cr2O3 needed based on the moles derived from the first part.

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  • Calculate the molar mass of Chromium(III) Oxide (Cr2O3)
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triplepie
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1. Chromium(III) Oxide reacts with Hydrogen Sulfide(H2S) gas to form Chromium Sulfide and water.

CR2O3(s) + H2S(g) = Cr2S3(s) + H2O (l)

to produce 439g of Cr2S3.

a. How many moles of Cr2O3 are required?

b. How many grams of CR2O3 are required?



2. Not sure how to set this up



3. All I could think of was finding the total grams of CR2O3 and dividing it from 439g's to find part a, but I think I was wrong
 
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Identify the ratios from the written reaction. Calculate the formula weights for the relevant compounds.
 
For part A: Find out how moles of Cr2S3 are in 439 g and the answer is how many moles of Cr2O3 because the mole:mole ratio is 1:1.

For part B: Calculate how many grams of Cr2O3 are in your answer to part a
 

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