Problem: Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water: Cr2O3(s) + 3H2S(g) ⟶Cr2S3(s) + 3H2O(l) To produce 421 g of Cr2S3, how many moles of Cr2O3 are required?

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We’re being asked to calculate the moles of Cr2Orequired to produce 421 g of Cr2S3 for the following reaction:


Cr2O3(s) + 3 H2S(g) ⟶ Cr2S3(s) + 3 H2O(l) 


The flow for this problem will be like this:


Mass of Cr2S3 (molar mass of  Cr2S3) → Moles of Cr2S3 (mole-to-mole comparison)  Moles of Cr2O3


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Problem Details

Chromium(III) oxide reacts with hydrogen sulfide (H2S) gas to form chromium(III) sulfide and water: 

Cr2O3(s) + 3H2S(g) ⟶Cr2S3(s) + 3H2O(l) 

To produce 421 g of Cr2S3, how many moles of Cr2Oare required?

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.