5. The reaction which produces iron metal from iron ore, Fe-Os, in a blast furna

Question

5. The reaction which produces iron metal from iron ore, Fe-Os, in a blast furnace is represented by the balanced equation: Fe2O3(s) 3 CO (g) 2 Fe (s) + 3CO2 (g) + A small blast furnace is filled with 7.24 kg of iron ore. A. What volume of iron ore is used if its density is 7.34 g/cm? 1.24 7.34 91C B. What volume of carbon monoxide, measured at STP, is required theoretically to react with all the iron ore? C. If the actual yield of iron metal was 68.2 moles, what was the percent yield of this reaction?

Explanation / Answer

A) Density = mass / volume

Volume = mass / density

Volume = 7.24 x 10^3 g / 7.34 g/cm^3 => 986 cm^3 or mL

Volume = 0.986 L

B) 1 eq Fe2O3 ore required 3 eq of CO

Molar mass of Fe2O3 = 159.69 g/mol or 0.15969 kg/mol

so 7.24 kg / 0.15969 kg/mol => 45.33 moles

Therefore moles of CO required = 45.33 x 3 => 136 moles

at STP

V = nRT / P

V = 136 moles x 0.082 L atm/mol.K x 298 K / 1 atm

V = 3.32 x 10^3 L

C) 1 eq of Fe2O3 produces 2 eq of Fe

So theoretically Fe = 2 x 45.33 => 90.66 moles

% Yield = ( 68.2 / 90.66) x 100 => 75.2 %

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