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Percent_Purity_Yield_WS_answers

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					Percent Purity, Percent Yield                                         Name: __________________________
                                                                      Date: _________________


 1. The roasting of siderite ore, FeCO3, produces iron (III) oxide:
                                      FeCO3 + O2  Fe2O3 + CO2
       a. What is the balanced equation?
           4 FeCO3 + O2  2 Fe2O3 + 4 CO2
       b. A 15.0 g FeCO3 sample is 42.0% pure. What mass of Fe2O3 can the sample produce?
           (6.30 g pure FeCO3 will react)
           4.34 g Fe2O3
       c. A second sample of FeCO3, with a mass of 55.0 g is roasted so as to produce 37.0g of Fe2O3.
           What is the percentage purity of FeCO3?
           (49.9g pure FeCO3)
           49.9g / 55.0 g * 100% = 97.6 %
       d. A 35.0 g sample of pure FeCO3 produces 22.5 g of Fe2O3. What is the percentage yield of the
           reaction?
           (24.1g pure Fe2O3 produced)
           22.5g / 24.1 g *100% = 93.3%
       e. What mass of siderite ore with a purity of 62.8% is needed to make 1.00 kg of Fe2O3?
           2310 g

 2. A 100. g sample of impure FeS2 is roasted to produce Fe2O3 + SO2:
                                      4 FeS2 + 11 O2  2 Fe2O3 + 8 SO2
    If 4.50 L of SO2 is collected at STP, what percentage of FeS2 is in the sample?
    (find the mass of FeS2 required to make 4.50L of SO2 = 12.1 g FeS2)
    12.1%

 3. ***This question is quite challenging***
    The reaction:
                                SiO2 (g) + HF (g)  SiF4 (g) + 2 H2O (g)
    produces 2.50g of H2O when 12.20g of SiO2 is treated with a small excess of HF?
        a. What is the balanced equation?
            SiO2 + 4 HF  SiF4 + 2 H2O
        b. What mass of SiF4 is formed?
            7.23g
        c. What mass of SiO2 is left unreacted?
            8.03g
        d. What is the percentage yield of SiF4?
            34.2%

 4. When 5.000 kg of malachite ore containing 4.30% of malachite, Cu2(OH)2CO3, is heated, the product
    is copper (II) oxide:
                                  Cu2(OH)2CO3  CO2 + CuO + H2O
        a. What is the balanced equation?
            Cu(OH)2CO3  CO2 + 2 CuO + H2O
        b. If the reaction has an 84.0% yield, how many grams of CuO are produced?
            1.30 x 102 g
        c. If the decomposition reaction has an 87.0% yield, what mass of ore containing 3.70%
            malachite is required to produce 100.0g of CuO?
            4.32 x 103 g

 5. A mine produces a silver ore named argentite, Ag2S. The ore is smelted according to the overall
    reaction
                                  Ag2S + C + O2  Ag + CO2 + SO2
a. What is the balanced equation?
   Ag2S + C + 2 O2  2 Ag + CO2 + SO2
b. A 250.0 kg load of argentite ore contains 0.135% pure Ag2S. What mass of silver metal can
   be produced from the load of core?
   294 g
c. A 76.4 g test sample of ore from a new ore vein produces 0.261g of pure silver. What is the
   percentage of pure argentite in the ore?
   0.392%
d. A sample of pure Ag2S has a mass of 152.6 g. When smelted, the sample produces 117.4 g of
   pure Ag. What is the percentage yield of the smelting process?
   88.38%
e. What mass of ore containing 0.795 % Ag2S is required to produce a 50.0 kg ingot of silver
   metal?
   7.22 x 106 g
f. If 89.2% of the Ag2S present is extracted from 3.50x104 kg of ore containing 1.86% Ag2S,
   what mass of silver metal can be produced?
   5.05 x 105 g

				
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