AP Chemistry

A 44.6 g of iron ore is treated as follows. The
iron in the sample is all converted by a series
of chemical reactions to Fe2O3. The mass of
Fe2O3 is measured to be 10.1 grams. What
was the percent iron in the sample of ore?
Answer in units of %

  1. 👍 0
  2. 👎 0
  3. 👁 34
asked by Anonymous
  1. What fraction, F, of the mass of a Fe2O3 molecule is FE ?

    total mass of molecule = 2(atomic mass Fe)+3(atomic mass O)

    mass of Fe in that molecule = 2 (atomic mass Fe)
    so
    F = 2(atomic mass Fe)/[ the sum ]

    then
    Mass Fe = 10.1 * F

    and percent = (Mass Fe/44.6)100

    1. 👍 0
    2. 👎 0
    posted by Damon

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    A 39 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 7.9 grams. What was the percent iron in the sample of ore? Answer in

    asked by Alex on September 20, 2015
  2. ap chemistry

    A 25.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 12 grams. What was the percent iron in the sample of ore? Answer

    asked by cheri on September 10, 2012
  3. AP Chemistry

    A 40.3 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.5 grams. What was the percent iron in the sample of ore? Answer

    asked by Gabriella on August 30, 2013
  4. chemistry

    A 46.9 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 11.6 grams. What was the percent iron in the sample of ore? Answer

    asked by Anonymous on August 30, 2011
  5. Chemistry

    I have 3 I don't understand how to do. A 33.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 12.3 grams. What was the

    asked by Brett on September 21, 2012
  6. 11th grade

    A 36.5 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10 grams. What was the percent iron in the sample of ore?

    asked by Anonymous on September 15, 2010
  7. chemistry

    A 28.6 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.1 grams. What was the percent iron in the sample of ore?

    asked by Nick on August 30, 2012
  8. AP Chemistry

    A 33.8 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 20.7 g. What was the mass of iron in the sample of ore?

    asked by Allyson on September 7, 2015
  9. AP chem

    A 37.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 11.1 grams. What was the percent iron in the sample of ore? Answer

    asked by Anonymous on August 25, 2013
  10. chemistry

    A 0.1943g iron ore sample was dissolved in hydrochloric acid and the iron was obtained as Fe 2+ (aq). The iron solution was titrated with Ce 4+ solution according to the balanced chemical reaction shown below.After calculation, it

    asked by matt on October 17, 2010

More Similar Questions