When steam (hot water) is passed over iron, hydrogen gas and iron (lll) oxide are formed. What mass of steam would be needed to react completely with 100.0 g of iron?

Question

Peyton Adams · Accepted Answer

The reaction requires 48.4 g of steam.

First, write the equation that is balanced. #"2Fe" + "3H"_2"O" → "Fe"_2"O"_3 + "3H"_2# Step 2: Determine the iron moles. #100 cancel("g Fe") × "1 mol Fe"/(55.84 cancel("g Fe")) = "1.791 mol Fe"# Step 3. Calculate the moles of #"H"_2"O"#. #1.791 cancel("mol Fe") × ("3 mol H"_2"O")/(2 cancel("mol Fe")) = "2.686 mol H"_2"O"# Step 4. Calculate the mass of #"H"_2"O"#. #2.686 cancel("mol H"_2"O") × ("18.02 g H"_2"O")/(1 cancel("mol H_2"O"")) = "48.4 g H"_2"O"#

Noah Aldrich · Answer

undefined To determine the mass of steam needed to react completely with 100.0 g of iron, we first need to write and balance the chemical equation for the reaction:

3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g)

From the balanced equation, we can see that 4 moles of water (H2O) are required to react with 3 moles of iron (Fe).

The molar mass of iron (Fe) is approximately 55.85 g/mol, and the molar mass of water (H2O) is approximately 18.015 g/mol.

Using stoichiometry:

1. Calculate the number of moles of iron in 100.0 g:
   Moles of iron = Mass of iron / Molar mass of iron

2. Use the mole ratio from the balanced equation to find the moles of water needed:
   Moles of water = Moles of iron × (4 moles H2O / 3 moles Fe)

3. Convert moles of water to grams:
   Mass of water = Moles of water × Molar mass of water

4. Perform the calculations to find the mass of steam needed.