The reduction of iron(III) oxide to iron during steel-making can be summarized by this sequence of reactions: 2C(s) +02 (g) > 2CO (g) K1Fe2O3 (s) + 3CO(lg) > 2Fe(l)+3CO2 (g) K2The net reaction is: 2Fe2O3(s) + 6C(s) + 3O2(g) ---> 4Fe(I) + 6CO2 (g) Kwrite an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2· If you need to include any physical constants be sure you use their standard symbols, which you'll find in the ALEKS Calculator.

K = [Fe]4×[CO2] / [Fe2O3]2 × [C]6 × [O2]3

Explanation: the over all reaction is

2Fe2O3(s) + 6C(s) + 3O2(g) ---> 4Fe(I) + 6CO2 (g)

So equilibrium constant equals, product concentration/ reactant concentration.

K = [Fe]4×[CO2] / [Fe2O3]2 × [C]6 × [O2]3

the potential energy of the reactants is 200j.

from the energy diagram, the energy of the product formed is 350j; this means that, this reaction is an endothermic reaction, because it absorbs energy from its environment.

i do not get it   at all