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Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide.4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g)A sample of 36.9 g MnO2 is added to a solution containing 48.9 g HCl.What is the limiting reactant?MnO2HClWhat is the theoretical yield of Cl2?theoretical yield:g Cl2If the yield of the reaction is 74.7%, what is the actual yield of chlorine?actual yield:g Cl2

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Answer:

HCl is limiting reactant

Theoretical yield: 23.8g Clâ‚‚

Actual yield: 17.6g Câ‚‚

Explanation:

Based on the reaction:

4HCl(aq)+MnO2(s)⟶MnCl2(aq)+2H2O(l)+Cl2(g)

4 moles of HCl reacts per mole of MnOâ‚‚ to produce 1 mole of MnClâ‚‚ and Clâ‚‚ and 2 moles of water.

To find the limiting reactant you must know the moles of each reactant and knowing that 4 moles of HCl reacts per mole of MnOâ‚‚ you can sikve this problem, thus:

Moles HCl (Molar mass: 36.46g/mol): 48.9g â‚“ (1mol / 36.46g/mol) =

1.341 moles HCl

Moles MnOâ‚‚ (Molar mass: 86.937g/mol): 36.9g â‚“ (1mol / 86.937g) =

0.424 moles MnOâ‚‚

For a complete reaction of 0.424 moles of MnOâ‚‚ you require:

0.424moles MnOâ‚‚ â‚“ (4 moles HCl / 1 mole MnOâ‚‚) = 1.696 moles of HCl.

As you have just 1.341 moles of HCl. HCl is limiting reactant.

Theoretical yield means, in the reaction, that 4 moles of HCl will produce 1 mole of Clâ‚‚. As moles of HCl are 1.341:

1.341 moles HCl â‚“ (1 mole Clâ‚‚ / 4 moles HCl) = 0.33525 moles Clâ‚‚

In grams (Molar mass Clâ‚‚: 70.9g/mol):

Theoretical yield: 0.33525 moles Clâ‚‚ â‚“ (70.9g / mol) = 23.8g Clâ‚‚

As yield of reaction is 74.7%, the real mass of Clâ‚‚ you obtain (Actual yield) is:

23.8g Clâ‚‚ â‚“ 74% = 17.6g Câ‚‚

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