1- In an experiment, 18 g of silver nitrate was dissolved in enough water to for

Question

1- In an experiment, 18 g of silver nitrate was dissolved in enough water to form 100.0 mL of solution. This aquesous silver nitrate solution was then mixed with 400.0mL of aqueous 0.50 M iron(III) chloride solution and a white precipiate formed. After filtiration and drying, 13.2 g of white solid was obtained .

(A) write a balanced chemical equation for the reaction that occures in the experiment

(B)Give the net ionic equation for this reaction

(C)What i the percent yield for the reaction?

(D) What is the concentration of chloride ion in the reaction solution after the reaction (concentration of chloride ion remaning after complete precipitation of the solid product of the reaction.

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2- Liquid iron is made from Fe2O3 in the following three-step chmical process in a blast furance

3 Fe2O3 (s) + CO (g) --> 2 Fe3O4 (s) + CO2 (g)

Fe3O4 (s) + CO (g) --> 3 FeO (s) + CO2 (g)

FeO (s) + CO (g) --> Fe (l) + CO2 (g)

What is the maximm mass of iron that could be produced from 250.0 g of Fe2O by this process?

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3- Acetic Acid (HC2H3O2) is the major ingredient of vinegar. A 12.5 mL sample of vinegar was titrated using 0.504 M aqueous NaOH solution. the titration required 20.65 mL of the base to reach the equivalence point.

Assuming the density of the vinegar is 1.01 g/mL, what is the mass precent acetic acid in this sample of vinegar?

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Solve one of them and you get 3 points solve all of them and you get 5

Explanation / Answer

a.) 3AgNO3 + FeCl3 ---> 3AgCl + Fe(NO3)3

b) Fe --> Fe3+ + 3e-

NO3 + e- --> NO3-

Ag --> Ag+ + e-

3Cl + 3e- --> 3Cl-

c) 0.1 moles of AgNO3 reacting with 0.2 moles of FeCl3

3 :1 ratio they react generally...0.1 moles of AgNO3 gives 0.1 moles AgCl.. 13.2 gms of white ppt, of 0.2 moles of FeCl3 only 1/6th reacts to form salts.. remaining is left out so

% yield with resp to Fecl3 = 16.66%

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