From Part A Mass of K x Fe(C 2 O 4 ) y zH 2 O prepared 5 100 g Mas...

From Part A: Mass of KxFe(C2O4)y Â· zH2O prepared : 5.100 g Mass of FeCl3 : 1.60 g From...

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Chemistry

From Part A:
Mass of K_xFe(C₂O₄)_yÂ· zH₂O prepared : 5.100 g
Mass of FeCl₃ : 1.60 g
From Part B:
% Potassium in compound : 17.95 %
% Iron (from ion exchange & titration vs. NaOH) : 8.35 %
From Part C:
% Oxlate : 43.97 %
Calculate the % water of hydration :
Calculate the following for Fe³⁺:
g in 100 g sample mol in 100 g sample mol/mol Fe
(3 sig figs) mol/mol Fe
(whole number)
Calculate the following for K⁺:
g in 100 g sample mol in 100 g sample mol/mol Fe
(3 sig figs) mol/mol Fe
(whole number)
Calculate the following forC₂O₄^2-:
g in 100 g sample mol in 100 g sample mol/mol Fe
(3 sig figs) mol/mol Fe
(whole number)
Calculate the following for H₂O
g in 100 g sample mol in 100 g sample mol/mol Fe
(3 sig figs) mol/mol Fe
(whole number)
Using your chemical knowledge and literature references (donâ€™tforget to include the references in your lab report and discusspossible sources of errors) answer the questions below:
Enter the simplest formula of the Iron Oxalate Complex Salt:
K Fe(C₂O₄) Â· H₂O
Now that the formula of the complex salt is known, thepercent yield can be determined.
Calculate the moles of FeCl₃ used in preparation:
Calculate the theoretical moles ofK_xFe(C₂O₄)_y Â·zH₂O:
Calculate the actual moles ofK_xFe(C₂O₄)_y Â·zH₂O synthesized:
Calculate the percent yield:

Answer & Explanation Solved by verified expert

3.8 Ratings (395 Votes)

Given mass of FeCl3 taken 16 g mass of complex formed 51 g Fe 835 K 1795 C2O4 4397 Total 7027 H2O 100 7027 2973 Therefore water of hydration 2973 For Fe3 g 100 g of sample 835 g mole 100g of sample 835 5585 015 mole mole of See Answer

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g in 100 g sample	mol in 100 g sample	mol/mol Fe (3 sig figs)	mol/mol Fe (whole number)