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

for step 7 table c on the lab "newtons law of action"   the average time it took the car to travel .25 meters   was 1.92 seconds.

the average time it took the car to travel 0.50 meters was 2.61 seconds

hope this : )