The Iron salt is made according to the formula given in your lab manual. FeCl3(aq) +...
The Iron salt is made according to the formula given in your lab manual.
FeCl3(aq) + K2C2O4(aq) → KxFe(C2O4)y·zH2O(s)
16.26 mL of a 0.367 g/mL FeCl3 solution is combined with 13.52 g of K2C2O4·H2O. (Water is part of the compound.)
How many moles of product (KxFe(C2O4)y·zH2O(s)) could be obtained assuming that the K2C2O4·H2O is in excess and that all of the Fe originally in FeCl3 ends up in the product?
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The Iron salt is made according to the formula given in your lab
manual.
FeCl3(aq) +...
With the completion of the determinations of % potassium, % iron, and % oxalate in the...
With the completion of the determinations of % potassium, % iron, and % oxalate in the crystals, you may calculate the % water. The percentage compositionof the crystals, KxFe(C2O4)y · zH2O, has then been completely determined experimentally. The simplest formula (x,y,z) can now be calculated from the the percentage composition. Once the formula is know it is then possible to calculate the percent yield of product that was obtained in the preparation and purification of the crystals. From Part A:...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 4.200 g Mass of FeCl3 :...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 4.200 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 22.00 % % Iron (from ion exchange & titration vs. NaOH) : 9.10 % From Part C: % Oxlate : 36.96 % - 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)...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 6.000 g Mass of FeCl3 :...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 6.000 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 11.50 % % Iron (from ion exchange & titration vs. NaOH) : 14.70 % From Part C: % Oxlate : 40.56 % Calculate the % water of hydration : 33.24 1.Enter the simplest formula of the Iron Oxalate Complex Salt: K Fe(C2O4) · H2O Now that the formula of the complex salt is known,...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 4.359 g Mass of FeCl3 : 1.60 g From Part B: % ...
From Part A: Mass of KxFe(C2O4)y · zH2O prepared : 4.359 g Mass of FeCl3 : 1.60 g From Part B: % Potassium in compound : 22.70 % % Iron (from ion exchange & titration vs. NaOH) : 10.60 % From Part C: % Oxlate : 55.69 % Now, let's finish the calculation and the determination of the formula of the iron compound: Calculate the % water of hydration : Tries 0/3 Calculate the following for Fe3+: g in 100...
Equation given in lab manual Fe(C2O4)y-x + 3OH - ---> Fe(OH)3 + yC2O4-2 1. Moles of...
Equation given in lab manual Fe(C2O4)y-x + 3OH - ---> Fe(OH)3 + yC2O4-2 1. Moles of NaOh used to complete the reaction 2. Moles of iron(III) oxalate reacted 3. Moles of Fe+3 reacted 4. Grams of Fe+3 reacted 5. Percentage of Fe+3 in the KxFe(C2O4)y * zH2O green salt complex 6. Calculate the actual percentage of Fe+3 in K3(C2O4)3 * 3H2O 7. Percent error? Data: Mass of crystals 0.177g 40ml of distilled water used to dissolve the crystals Total volume...
With the completion of the determinations of % potassium, % iron, and % oxalate in the...
With the completion of the determinations of % potassium, %
iron, and % oxalate in the crystals, you may calculate the % water.
The percentage compositionof the crystals,
KxFe(C2O4)y ·
zH2O, has then been completely determined
experimentally. The simplest formula (x,y,z) can now be calculated
from the the percentage composition. Once the formula is know it is
then possible to calculate the percent yield of product that was
obtained in the preparation and purification of the crystals.
From Part A:...
BACKGROUND: Synthesis of Potassium Iron (III) Oxalate Hydrate Salt The iron(II) ions from Fe(NH4)2(SO4)2•6H2O will be precipitated as iron(II) oxalate. Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s) The su...
BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
Take-Home Assignment This assignment is due on Friday, January 31st. How many grams of FeCl3 could...
Take-Home Assignment This assignment is due on Friday, January 31st. How many grams of FeCl3 could be made by reacting 165 mL of a 0.180 M HCl solution with excess iron? (5) → 2 FeCl3(aq) + 3 H2(g) 2 Fe(s) + 6 HCl(aq) =.165. 15mL IL T1000mL HG/ 0165L HCL .180 moles a moles Feclz 162. 2049 IL T6 moles Hell Imol FeCl3 mass of FeCl3 (g):
16. How many grams of steam and iron must react to produce 375 g of magnetic...
16. How many grams of steam and iron must react to produce 375 g of magnetic iron oxide, Fe3O4? 3 Fe(s) + 4 H2O(g) Fe3O4(s) + 4 H2(g) 18. Mercury can be isolated from its ore by the reaction 4 HgS + 4 CaO → 4 Hg + 3 CaS + CaSO4 (a) How many moles of CaS are produced from 2.5 mol CaO? (b) How many grams of Hg are produced along with 9.75 mol of CaSO4? (c) How many...
You analyze a sample of unknown metal using the procedure n the lab manual. Your sample...
You analyze a sample of unknown metal using the procedure n the lab manual. Your sample of metal has a mass of 0.0714 g, and you determine that 0.00506 moles of hydrogen gas were generated in the experiment. What is the atomic mass of this unknown metal? Assume the stoichiometry given in equation 1 works for this unknown metal. Be sure to enter the correct number of significant figures in your answer. g/mol The objective of this experiment is to...
With the completion of the determinations of % potassium, %
iron, and % oxalate in the crystals, you may calculate the % water.
The percentage compositionof the crystals,
KxFe(C2O4)y ·
zH2O, has then been completely determined
experimentally. The simplest formula (x,y,z) can now be calculated
from the the percentage composition. Once the formula is know it is
then possible to calculate the percent yield of product that was
obtained in the preparation and purification of the crystals.
From Part A:...
BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
Take-Home Assignment This assignment is due on Friday, January 31st. How many grams of FeCl3 could be made by reacting 165 mL of a 0.180 M HCl solution with excess iron? (5) → 2 FeCl3(aq) + 3 H2(g) 2 Fe(s) + 6 HCl(aq) =.165. 15mL IL T1000mL HG/ 0165L HCL .180 moles a moles Feclz 162. 2049 IL T6 moles Hell Imol FeCl3 mass of FeCl3 (g):
You analyze a sample of unknown metal using the procedure n the lab manual. Your sample of metal has a mass of 0.0714 g, and you determine that 0.00506 moles of hydrogen gas were generated in the experiment. What is the atomic mass of this unknown metal? Assume the stoichiometry given in equation 1 works for this unknown metal. Be sure to enter the correct number of significant figures in your answer. g/mol The objective of this experiment is to...
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