One of the reactions that occurs in a blast furnace, in which iron ore is converted to cast iron, is fe2o3 + 3co → 2fe + 3co2 suppose that 1.79 × 103 kg of fe is obtained from a 2.86 × 103 kg sample of fe2o3. assuming that the reaction goes to completion, what is the percent purity of fe2o3 in the original sample?

Answer : The percent purity of in the original sample is 87.94 %

Explanation :

The given balanced chemical reaction is:

First we have to calculate the mass of Fe.

Molar mass of Fe = 55.8 g/mole

Now we have to calculate the moles of

From the balanced chemical reaction we conclude that,

As, 2 moles of Fe produced from 1 mole of

So, of Fe produced from mole of

Now we have to calculate the mass of

Molar mass of = 159.69 g/mole

Now we have to calculate the percent purity of in the original sample.

Mass of original sample =

Therefore, the percent purity of in the original sample is 87.94 %

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.