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# Answer to Question #183483 in General Chemistry for Krissy

Question #183483

c. If 9.63g of FeS is formed what is the % yield?                           /2

1. Calculate the percent yield for the reaction:   P4 (s) + 6 Cl2 (g) → 4 PCl3 (l)

2. if 75.0 g of phosphorus reacts with excess chlorine gas to produce 111.0 g of phosphorus trichloride. /5

3. When iron (II) hydroxide is mixed with phosphoric acid, iron (II) phosphate precipitate results.

4. Balance the following equation:   Fe(OH)2 (aq) + H3PO4 (aq)  →  Fe3(PO4)2 (s) + H2O (l)   /1

1
2021-04-21T06:09:28-0400

Perform the standard mass to mass (3 step) stoichiometry calculation to find the amount of product for each of the two reactants assuming the other one is in excess. Whichever one produces the lesser amount of product is the limiting reactant and you have found the theoretical yield.

To find the percent yield: 100 (actual yield given)/theoretical yield) in per cent.

Three molecules of Fe(OH)2 reacts with two molecules of H3PO4 to precipitate one molecule of Fe3(PO4)2 and six molecules of H2O.

Balanced equation ;

"3 Fe(OH)_2 + 2 H_3PO_4 \u2192 Fe_3(PO_4)_2 + 6 H_2O"

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