Suppose 650 mL of hydrogen gas are produced through a displacement reaction involving solid iron and sulfuric acid, H2SO4, at STP. How many grams of iron (II) sulfate are produced? Density H2(g) is on your periodic table.

                     Mass  =  4.415 g of FeSO₄

Explanation:

                   The balance chemical equation for given single replacement reaction is as follow;

                                  Fe + H₂SO₄ → FeSO₄ + H₂

Data Given;

                  Volume =  650 mL  =  0.65 L

                  Density at STP =  0.08988 g/L

                  Mass = Density × Volume = 0.08988 g/L × 0.65 L = 0.0584 g

Step 1: Calculate Moles of H₂ as;  

                  Moles  =  Mass / M.Mass

                  Moles  =  0.0584 g / 2.01 g/mol

                  Moles  =  0.0290 mol of H₂

Step 2: Find out moles of FeSO₄ as;

According to balance chemical equation,

            1 mole of H₂ is produced along with  =  1 mole of FeSO₄

So,

   0.0290 moles of H₂ will be produced along with  =  X moles of FeSO₄

Solving for X.

                     X  =  0.0290 × 1 mol / 1 mol

                     X =  0.0290 moles of FeSO₄

Step 3: Calculate mass of FeSO₄ as;

                   Mass  =  Moles × M.Mass

                   Mass  =  0.0290 mol × 151.90 g/mol

                   Mass  =  4.415 g of FeSO₄

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