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25 January, 12:45

Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese (IV) oxide. 4 HCl (aq) + MnO 2 (s) ⟶ MnCl 2 (aq) + 2 H 2 O (l) + Cl 2 (g) A sample of 40.5 g MnO 2 is added to a solution containing 47.7 g HCl. What is the limiting reactant? HCl MnO 2 What is the theoretical yield of Cl 2? theoretical yield: 33.1 g Cl 2 If the yield of the reaction is 85.3 %, what is the actual yield of chlorine? actual yield: 28.23 g Cl 2

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  1. 25 January, 12:50
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    1. HCl is the limiting reactant.

    2. The theoretical yield of Cl2 is 23.197g

    3. The Actual yield 19.787g

    Explanation:

    4HCl + MnO2 - > MnCl2 + 2H2O + Cl2

    First let us calculate the number of mole of HCl and MnO2.

    Molar Mass of HCl = 1 + 35.5 = 36.5g/mol

    Mass of HCl = 47.7g

    Number of mole = Mass / Molar Mass

    Number of mole of HCl = 47.7/36.5 = 1.31mole

    Molar Mass of MnO2 = 35 + (2x16) = 35 + 32 = 67g/mol

    Mass of MnO2 = 40.5g

    Number of mole = Mass / Molar Mass

    Number of mole of MnO2 = 40.5/67 = 0.60mole

    From equation,

    4moles of HCl required 1mole of MnO2. Now let us consider the following:

    4moles HCl require 1mole MnO2. Therefore 0.31mol of HCl will require = 0.31/4 = 0.0775mole of MnO2. This amount is little compared to the amount of MnO2 (i. e 0.60mol) calculated. Therefore, HCl is the limiting reactant.

    2. 4HCl + MnO2 - > MnCl2 + 2H2O + Cl2

    Molar Mass of HCl = 36.5g/mol

    Mass of HCl from the balanced equation = 4 x 36.5 = 146g

    Molar Mass of Cl2 = 2 x 35.5 = 71g/mol

    From the equation,

    146g of HCl produced 71g of Cl2.

    Therefore, 47.7g of HCl will produce = (47.7x 71) / 146 = 23.197g of Cl2.

    The theoretical yield of Cl2 is 23.197g

    3. %yield = 85.3%

    Theoretical yield = 23.197g

    Actual yield = ?

    %yield = Actual yield / Theoretical yield

    Actual yield = %yield x theoretical yield

    Actual yield = 85.3% x 23.197g = (85.3/100) x 23.197 = 19.787g
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