Question

MnO2 (s) + 4HCl (aq)  MnCl2 (s) + Cl2 (g) + 2H2O (l) a) Explain the difference between a limiting reactant and an excess reactant. b) Calculate the theoretical yield (in grams) of chlorine (Cl2) gas that would form according to the above chemical reaction. c) If the percentage yield of chlorine gas in the above reaction is 89.5 %, calculate the experimental yield of chlorine gas in grams.

Answer 1

Answer:

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Answer 2

The answers are as follows:

(a) Limiting reactant (or limiting reagent) is that reactant which will be completely consumed in the reaction.

- Excess reactant is the reactant some of whose amount will be left even after the completion of reaction.

-  The reaction stops when limiting reagent is totally used up and there is always some amount of excess reactant left behind..

(b) According to the given reaction:

87 gm of MnO2 produces 71 gm of Chlorine (Cl2) gas.

(c) Percentage yield = (Experimental yield / theoretical yield) × 100

⇒ Experimental yield = (Percentage yield × theoretical yield) / 100

⇒ Experimental yield = (89.5 × 71) / 100

⇒ Experimental yield = 63.545 gm.

- So, 63.454 gm is the experimental yield of chlorine gas in the given reaction.