During a laboratory experiment, a 2.36-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 1.57 grams. calculate the percentage yield of carbonic acid for the reaction. describe the calculation process in detail. nahco3 → na2co3 + h2co3

Explanation:

1) Chemical equation (given)

2) Theoretical yield

a) Convert mass of NaHCO₃ to moles:

b) Mole ratio:

c) Proportionality:

       ⇒ x = 0.2809 / 2 mol H₂CO₃ = 0.01405 mol H₂CO₃

3) Actual yield

a) Mass balance: 2.36 g - 1.57 g = 0.79 g

b) Convert 0.79 g of carbonic acid to number of moles:

4) Percentage yield, y (%)

The answer must show 3 significant figures, so y(%) = 90.7%.

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explanation:

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