Chemistry

posted by .

Hi, could someone please take a look at my solution to this problem and let me know if it's correct? I would really appreciate some help.

Calculate the theoretical yield for K3[Fe(C2O4)3]*3H2O; 491.258 g/mol

Mass of Ferrous Ammonium Sulfate Hexahyrdreate: 4.01 g, 392.17 g/mol

[1] FeSO4∙(NH4)2SO4∙ 6H2O + H2C2O4∙ 2H2O ---> FeC2O4 + (NH4)2SO4 + H2SO4 + 8H2O

[2] 6 FeC2O4 + 3H2O2 + 6K2C2O4∙ H2O --->
4K3[Fe(C2O4)3]∙ 3 H2O + 2 Fe(OH)3 + 6 H2O

[3] 2 Fe(OH)3 + 3 H2C2O4∙ 2H2O + 3 K2C2O4∙ H2O ----> 2 K3[Fe(C2O4)3]∙ 3H2O + 9 H2O


4.01g * 1mol/392.17g = 0.01 mol FeSO4∙(NH4)2SO4∙ 6H2O

0.01 mol * 1/1 = 0.01 mol FeC2O4

0.01 mol * 4/6 = 0.00667 mol K3[Fe(C2O4)3]*3H2O

0.00667 mol * 491.258g/1mol = 3.28 g K3[Fe(C2O4)3]*3H2O

0.01 mol * 2/6 = 0.0033 mol Fe(OH)3

0.0033 * 2/2 = 0.0033 mol K3[Fe(C2O4)3]*3H2O

0.0033 mol * 491.258g/1mol = 1.62 g K3[Fe(C2O4)3]*3H2O

3.28 + 1.62 = 4.9 g K3[Fe(C2O4)3]*3H2O

  • Chemistry -

    The method looks ok to me but I disagree slightly with the numbers. I think most of that is that you threw away some significant figures here and there. For example, the first calculation of 0.01 should be 0.0102. The 0.0033 should be recalculated for three s.f. etc.

  • Chemistry -

    Thank you Dr. Bob

  • Chemistry -

    Why did you add 3.28???

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. math

    how do you calculate theoretical yield of something?
  2. Chemistry

    4.0 g of ferrous ammonium sulphate, FeS04(NH4)2 SO4 6H20, is used. The oxalate is in excess, calculate the theoretical yield of the iron complex. Can someone please show me how to calculate a question like this please?
  3. chemistry - DrBob222

    For this question can u please explain steps 3 and 4 4.0 g of ferrous ammonium sulphate, FeS04(NH4)2 SO4 6H20, is used. The oxalate is in excess, calculate the theoretical yield of the iron complex. Can someone please show me how to …
  4. Chemistry

    4.0 gram of ferrous ammonium sulphate, FeSO4*(NH4)2SO4 * 6H2O, is used. Since the oxalate is in excess , Calculate the theoretical yield of the iron complex FeSO4•NH4)2SO4•6H2O + H2C2O4•2H20 --> FeC2O4 + (NH4)2SO4 + H2SO4 …
  5. chemistry

    can someone please help me with this question: mass of ferrous ammonium sulfate = 4g mass of k3(fe(c204)3)*3h2o = 4.25 g 1) using the above mass of ferrous ammonium sulfate calculate the theoretical yield of k3(fe(c204)3)*3h2o?
  6. Chem

    4.0 gram of ferrous ammonium sulphate, FeSO4*(NH4)2SO4 * 6H2O, is used. Since the oxalate is in excess , Calculate the theoretical yield of the iron complex. FeSO4•NH4)2SO4•6H2O + H2C2O4•2H20 --> FeC2O4 + (NH4)2SO4 + H2SO4 …
  7. chemistry

    Really need help on figuring out the formula for Iron Complex. The question was: 4.0 g of ferrous ammonium sulphate, FeS04(NH4)2*SO4*6H20, is used. The oxalate is in excess, calculate the theoretical yield of the iron complex. I got …
  8. Science

    If .275 moles of ferrous ammonium sulfate (Fe(NH4)2(SO4)2. 6H2O) and an excess of all other reagents are used in a synthesis of K3[Fe(C2O4)3].3H2O, how many grams of product will be obtained if the reaction gives a 100% yield?
  9. Chemistry

    If 0.273 moles of ferrous ammonium sulfate (Fe(NH4)2(SO4)2 . 6H2O) and an excess of all other reagents are used in a synthesis of K2[Fe(C2O4)3] . 3H2O, how many grams of product will be obtained if the reaction gives a 100% yield?
  10. Chemistry

    Dr. Bob222, Yesterday I posted a question and you answered me with how to calculate it.. Can you tell me if I'm doing this correctly?

More Similar Questions