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Limiting Reactant, Theoretical Yield and Percent Yield

Chemistry
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When 56.1g Fe2O3 reacts with 64.2g HCl, 89.9g of FeCl3 form. What is the limiting reactant, theoretical yield and percent yield. How much of the excess reactant remains? 

The formula is: Fe2O3 + 6 HCl --> 2 FeCl3 + 3H2O

Mar 23rd, 2015

Fe2O3 +6 HCl ---> 2 FeCl3+3H2O

(2*55.85+48)  6*36.45  2*(55.85+35.45*3) 

111.7       218.7                 324.4

56.1g FeO3 needs 218.7/111.7*56.1 = 109.84 g of HCl to complete react with it, so 56.1 is limit reactant. 

the theorectial yield of FeCl3 is 324.4/111.7*56.1 = 162.93 g, percentage yield is 89.9/162.93 x100% =55.2%   

Mar 23rd, 2015

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