During a laboratory experiment, a 3.81-gram sample of nahco3 was thermally decomposed. in this experiment, carbon dioxide and water vapors escape and are combined to form carbonic acid. after decomposition, the sample weighed 2.86 grams. calculate the percentage yield of carbonic acid for the reaction. describe the calculation process in detail. nahco3 → na2co3 + h2co3

Answer : The percent yield of  is, 24.44 %

Explanation :

First we have to calculate the moles of 3.81 g and 2.86 g of .

Moles of  reacted = 0.045 - 0.034 = 0.011 g

Now we have to calculate the moles of

The balanced chemical reaction will be,

From the balanced reaction, we conclude that

As, 2 moles of react to give 1 mole of

So, 0.011 moles of react to give mole of

Now we have to calculate the mass of

The actual yield of  = 0.341 g

If whole of  have reacted then  produced.

From the balanced reaction, we conclude that

As, 2 moles of react to give 1 mole of

So, 1 mole of react to give 0.5 mole of

And, 0.045 mole of react to give mole of

The mass of  produced.

The theoretical yield of  = 1.395 g

Now we have to calculate the percent yield of

Therefore, the percent yield of  is, 24.44 %

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