One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron, is below. fe2o3 + 3 co → 2 fe + 3 co2 suppose that 1.92 ✕ 103 kg of fe are obtained from a 5.13 ✕ 103 kg sample of fe2o3. assuming that the reaction goes to completion, what is the percent purity of fe2o3 in the original sample?

The answer to your question is: 53.46 % pure

Explanation:

data

Fe = 1.92 ✕ 103 kg   produced    = 1920 kg

Fe2O3 = 5.13 ✕ 103 kg    sample   = 5130 kg

MW Fe2O3 = (56x2)+(16x3) = 160 kg

% of purity = ?

                   Fe2O3 + 3 CO → 2 Fe + 3 CO2

Convert mass to moles

Fe

      56 kg   1 mol

  1920 kg   x moles       x = 34.28 moles

From the reaction

   1 mol of Fe2O3  2 moles of Fe

      x moles of Fe2O3 34.28 moles

  x = 34.28/2 = 17.14 moles of Fe2O3

       160 kg of FE2O3  1 mol

             x kg of Fe2O3  17.14 moles

x = 17.14 x 160/1 = 2742,4 kg of Fe2O3  It's supposed to be the amount of Fe if it was 100% pure.

                             2742.4 kg of Fe2O3  100%

                              5130 kg of Fe2O3   x

x = (2742.4x100)/5130 = 53.46 pure

the ratio of the conjugate base to the acid required to attain the desired ph.