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a 3.24-gram sample of nahco3 was completely decomposed in an experiment. 2nahco3 → na2co3 + h2co3 in this experiment, carbon dioxide and water vapors combine to form h2co3. after decomposition, the na2co3 had a mass of 2.19 grams. determine the mass of the h2co3 produced. calculate the percentage yield of h2co3 for the reaction. show your work or describe the calculation process in detail.

32.06% yield
explanation:
first, calculate theoretical yield of carbonic acid
balanced equation: 2nahco3 → na2co3 + h2co3
step 1: convert 3.24 grams nahco3 to moles nahco3 by dividing by molar mass
          - 3.24 g nahco3 / (22.99 + 1.008 + 12.01 + 3(15.999)) g/mol nahco3 = 0.039         moles
step 2: use mol: mol ratio to convert moles nahco3 to moles h2co3
          - 0.039 mol nahco3 x 1 mol h2co3 / 2 mol nahco3 = 0.0195 moles h2co3
step 3: convert to grams h2co3 by multiplying by molar mass
          - 0.0195 moles h2co3 x ( 2(1.008) + 12.01 + 3(15.999)) = 1.209 grams h2co3
second: calculate the actual yield of carbonic acid, using the (3.24 - 2.19) 1.05 grams nahco3 that actually decomposed.
step 1: convert 1.05 grams nahco3 to moles nahco3 by dividing by molar mass
          - 1.05 g nahco3 / (22.99 + 1.008 + 12.01 + 3(15.999)) g/mol nahco3 = 0.0125 moles
step 2: use mol: mol ratio to convert moles nahco3 to moles h2co3
          - 0.0125 mol nahco3 x 1 mol h2co3 / 2 mol nahco3 = 0.0063 moles h2co3
step 3: convert to grams h2co3 by multiplying by molar mass
          - 0.0063 moles h2co3 x ( 2(1.008) + 12.01 + 3(15.999)) = 0.388 grams h2co3
third: calculate percent yield by dividing actual yield by theoretical yield, and multiplying by 100
0.388 g h2co3 / 1.209 g h2co3 (x 100%) = 32.06% yield.

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