10) Magnetite, an iron ore with the formula Feyo4, can be reduced by treatment w

Question

10) Magnetite, an iron ore with the formula Feyo4, can be reduced by treatment with hydrogen to yield iron metal and water vapor. This process requires 36 kcal of energy for every 1.00 mol of magnetite reduced. a Write the balanced equation for the reaction, including the value of the heat term. b) How much energy (in kilocalories is required to produce 55 g of iron? c) How many grams of hydrogen are needed to produce 75 g of iron? d) This reaction has a K 2.3 x 10 18 Are the reactants or the products favored? Explain your reasoning.

Explanation / Answer

a)The balanced equation is

Fe3O4 (s) + 4H2 (g) ----------> 3Fe(s) + 4H2O(g) : Delta H = +36Kcal

b) From this stoichiometric equation

1 mole of Fe3O4 produces 3 moles of iron (3x55.845g) and 36 Kcal is needed.

To get 55.0g of iron the energy required = 55.0 x 36 /3x55.845

= 11.81kCal

c)From the equation 4 moles of H2 (4x2g/mol) is need ed to produce 3 moles (3 x55.845g/mol) of iron

to produce 75 g of iron the amount of H2 required = 75g x 4x2g/mol /3x55.845g/mol

= 3.5813 g

d) If the reaction is equilibrium rection then

K = [H2O]/[H2] as the [solids] = 1

Thus if K = 2.3x10-18 , the equilibrium strongly favors the reactants only as it indicates [H2] is 1018 times> [H2O]

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.