Fe3O4 can be reduced by treatment with hydrogen to yield iron metal and water vapor write the balanced equation. this process required 36kcal for every 1.00 mol of Fe3O4 reduced. how much energy in kcal is required to produce 64g of iron. how many grams of hydrogen are needed to produce 71g of iron

Question

Fe3O4 can be reduced by treatment with hydrogen to yield iron metal and water vapor  write the balanced equation.  this process required 36kcal for every 1.00 mol of Fe3O4 reduced.  how much energy in kcal is required to produce 64g of iron.  how many grams of hydrogen are needed to produce 71g of iron

DrBob222 · Accepted Answer

Fe3O4 + 4H2 + 36 kcal ==> 3Fe + 4H2O

36 kcal x 64/3*atomic mass Fe = ? kcal required.

mols Fe needed = grams/atomic mass = ?
Use the coefficients in the balanced equation to convert mols Fe to mols H2.
Now convert g H2 to mols H2. g = mols x molar mass.