Question

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 565 g of Cr2S3,

(a) how many moles of Cr2O3 are required

Answer 1

Answer and Explanation:

The balanced chemical equation for the reaction is:

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

From the equation, we can see that one mole of Cr2O3 reacts with three moles of H2S to produce one mole of Cr2S3.

The molar mass of Cr2S3 is (2 x atomic mass of Cr) + (3 x atomic mass of S) = (2 x 52 g/mol) + (3 x 32 g/mol) = 152 g/mol.

So, to produce 565 g of Cr2S3, we need (565 g) / (152 g/mol) = 3.72 moles of Cr2S3.

Since one mole of Cr2O3 produces one mole of Cr2S3, we need 3.72 moles of Cr2O3 to produce 565 g of Cr2S3.

So, the answer to your question is that 3.72 moles of Cr2O3 are required to produce 565 g of Cr2S3.