The reduction of iron(III) oxide () to pure iron during the first step of steelmaking, ()()() is driven by the high-temperature

Question

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The reduction of iron(III) oxide () to pure iron during the first step of steelmaking, ()()() is driven by the high-temperature

combustion of coke, a purified form of coal: ()()() Suppose at the temperature of a blast furnace the Gibbs free energies of formation of and are and , respectively. Calculate the maximum mass of pure iron that can be produced by the combustion of of coke. Round your answer to significant digits.

Chemistry

1 answer:

notsponge [240] · Answer 1 · 2022-12-10T09:33:10+03:00

Answer:

hello your question is incomplete attached below is the complete question

answer : To 2 significant digits = 5500 kg

Explanation:

Given

C(s) + O2 (g) ----------> CO2 ( g )

mass of CO2 = 8.9 * 10^6 g

number of moles = 8.9 * 10^6 / 12 = 7.416 * 10 ^5 mol

same amount of moles is needed by O2 hence

attached below is the detailed solution