10) Magnetite, an iron ore with the formula Fe 04, can be reduced by treatment w

Question

10) Magnetite, an iron ore with the formula Fe 04, can be reduced by treatment with hydrogen to yield iron mctal 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 iror? c) How many grams of hydrogen are needed to produce 75 g of iron? d) This reaction has a K-2.3 x 1018. Are the reactants or the products favored? Explain your reasoning 9.4

Explanation / Answer

Fe3O4(s) + H2(g) + 36 kcal = Fe(s) + H2O(g)

balance

Fe3O4(s) + 4H2(g) + 36 kcal = 3Fe(s) + 4H2O(g)

b)

energy for m = 55 g of Iron

mol = mass/MW = 55/55.8 = 0.999 mol of Fe

3 mol of Fe = 36 kcal

1 mol of Fe = 36/3 = 12 kcal required

c)

mass of H2 for

m = 75 g of Fe

mol = mass/M W= 75/55.8 = 1.344

now

3 mol of Fe = 4 mol of H2

1.344 mol of Fe = x mol of H2

x = 4/3*1.344 = 1.792 mol of H2

mass = )mol*MW = 1.792*2 = 3.584 g o fH2

d)

since K <<1

clearly, only reactants will be favoured, therefore, expect mostly reactants in the mix

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