Examine the statement and balanced equation.

pure elemental iron undergoes a single replacement reaction with sulfuric acid (h2so4) to produce iron(iii) sulfate (fe2(so4)3) and hydrogen gas.

2fe + 3h2so4 → fe2(so4)3 + 3h2
(m fe = 55.8 g/mol, m h2so4 = 98.1 g/mol, m fe2(so4)3 = 399.9 g/mol, m h2 = 2.0 g/mol)

if 3.21 x 1012 mol of iron(iii) sulfate are formed, how many g of it will be produced?

The answer to your question is:   1.28 x 10 ¹⁵ g of Fe₂(SO₄)₃

Explanation:

Single replacement reaction:

                                  2Fe   +    3H₂SO₄    →    Fe₂(SO₄)₃   +   3H₂

M Fe = 55.8 g/mol

M H₂SO₄ = 98.1 g/mol

M Fe₂(SO₄)₃ = 399.9 g/mol

M H₂ = 2.0 g/mol

Fe₂(SO₄)₃ = 3.21 x 10¹² mol

Fe₂(SO₄)₃ =  ? g

                          1 mol of Fe₂(SO₄)₃  399.9 g/mol of Fe₂(SO₄)₃

                          3.21 x 10¹² mol Fe₂(SO₄)₃    x

                         x = (3.21 x 10¹² x 399.9 ) / 1

                         x = 1.28 x 10 ¹⁵ g of Fe₂(SO₄)₃

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