Hydrogen gas can be produced from a reaction of steam with iron metal according to the equation below:3Fe (s) + 4H2O (g) ⟶4 H2 (g) + Fe3O4 (s)What mass of hydrogen can be produced from the reaction of 568.2 g of steam with excess iron? Express your answer in the correct number of significant figures.

To solve this problem, we need to use stoichiometry, which is a method in chemistry that uses balanced chemical equations to calculate quantities of reactants or products.

Step 1: Balance the chemical equation The given chemical equation is already balanced: 3Fe (s) + 4H2O (g) ⟶ 4H2 (g) + Fe3O4 (s)

Step 2: Convert the mass of steam (H2O) to moles We know that the molar mass of H2O is approximately 18.015 g/mol. So, we can convert the mass of steam to moles using the formula: moles = mass / molar mass moles of H2O = 568.2 g / 18.015 g/mol = 31.54 mol

Step 3: Use the stoichiometry of the reaction to find the moles of hydrogen (H2) From the balanced chemical equation, we can see that 4 moles of H2O produce 4 moles of H2. Therefore, the moles of H2 produced will be the same as the moles of H2O used. moles of H2 = 31.54 mol

Step 4: Convert the moles of hydrogen (H2) to mass The molar mass of H2 is approximately 2.016 g/mol. So, we can convert the moles of H2 to mass using the formula: mass = moles * molar mass mass of H2 = 31.54 mol * 2.016 g/mol = 63.6 g

So, the mass of hydrogen that can be produced from the reaction of 568.2 g of steam with excess iron is approximately 63.6 g. This answer is expressed in the correct number of significant figures.