When NaHCO3 completely decomposes, it can follow this balanced chemical equation:

2NaHCO3 → Na2CO3 + H2CO3

Determine the theoretical yields of each product using stoichiometry if the mass of the NaHCO3 sample is 3.24 grams. (Show work for both)
In an actual decomposition of NaHCO3, the mass of one of the products was measured to be 2.01 grams. Identify which product this could be and justify your reasoning.
Calculate the percent yield of the product identified in part B. (Show your work)

Question

When NaHCO3 completely decomposes, it can follow this balanced chemical equation:

2NaHCO3 → Na2CO3 + H2CO3

Determine the theoretical yields of each product using stoichiometry if the mass of the NaHCO3 sample is 3.24 grams. (Show work for both)
In an actual decomposition of NaHCO3, the mass of one of the products was measured to be 2.01 grams. Identify which product this could be and justify your reasoning.
Calculate the percent yield of the product identified in part B. (Show your work)

Vocaloid · Answer

The equation is already balanced so we can move straight to the stoichiometry

Starting with 3.24g NaHCO3, convert this to moles by dividing by the molar mass

Then use the balanced equation to convert moles NaHCO3 to Na2CO3

Then multiply moles Na2CO3 by the molar mass of Na2CO3 to get grams Na2CO3

Repeat with the other product

For part B, see which of your yields is closer to 2.01g. That one is more likely to be your product

Finally calculate 2.01/theoretical yield * 100% to get the percent yield.

kekeman · Answer

@vocaloid wrote:

I'm confused can I see step by step the work? The equation is already balanced so we can move straight to the stoichiometry Starting with 3.24g NaHCO3, convert this to moles by dividing by the molar mass Then use the balanced equation to convert moles NaHCO3 to Na2CO3 Then multiply moles Na2CO3 by the molar mass of Na2CO3 to get grams Na2CO3 Repeat with the other product For part B, see which of your yields is closer to 2.01g. That one is more likely to be your product Finally calculate 2.01/theoretical yield * 100% to get the percent yield.

kekeman · Answer

@vocaloid wrote:

The equation is already balanced so we can move straight to the stoichiometry Starting with 3.24g NaHCO3, convert this to moles by dividing by the molar mass Then use the balanced equation to convert moles NaHCO3 to Na2CO3 Then multiply moles Na2CO3 by the molar mass of Na2CO3 to get grams Na2CO3 Repeat with the other product For part B, see which of your yields is closer to 2.01g. That one is more likely to be your product Finally calculate 2.01/theoretical yield * 100% to get the percent yield.

Pls