*Please show how you got the calculations. In a reactor scenario, 20.000 g Fe3O4 was reacted,...

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Chemistry

*Please show how you got the calculations.
In a reactor scenario, 20.000 g Fe3O4 was reacted, at 1450 K,with NO having an initial pressure of 3.000 atm. At equilibrium,the mass of the solid-phase product (Fe2O3) was calculated to be8.0742 g. 2Fe3O4(s) + 2NO(g) <=> 3Fe2O3(s) + N2O(g)
1. Calculate the mass of each gas-phase species atequilibrium.
2. Calculate the mass of Fe3O4 remaining at equilibrium from themass of Fe2O3 calculated to exist at equilibrium.
3. Calculate the total mass of all species at equilibrium andprove that it equals the initial total mass of the reactants, tothe .1 g place.

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4.2 Ratings (532 Votes)

20000 g Fe3O4 was reacted at 1450 K with NO having an initial pressure of 3000 atm At equilibrium the mass of the solidphase product Fe2O3 was calculated to be 80742 g 2Fe3O4s 2NOg 3Fe2O3s N2Og Solution Mass of Fe3O4 20g so moles of Fe3O4 mass molecular wt 20 2315 0086 moles Mass of Fe2O3 See Answer

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