NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g) 1. Calculate the moles of NaHCO3 in 3.00 g of NaHCO3. 2. Using your answer to question one, if 1 mole of Na2CO3 is produced for every 2 moles of NaHCO3, how many moles of Na2CO3 would theoretically be produced in the reaction? 3. How many grams of Na2CO3 would theoretically be produced in the reaction?
2 NaHCO3 (s) → Na2CO3 (s) + CO2 (g) + H2O (g)
1. Calculate the moles of NaHCO3 in 3.00 g of NaHCO3.
2. Using your answer to question one, if 1 mole of Na2CO3 is produced for every 2 moles of NaHCO3, how
many moles of Na2CO3 would theoretically be produced in the reaction?
3. How many grams of Na2CO3 would theoretically be produced in the reaction?
4. If the actual mass of Na2CO3 produced is 1.25 g, what is the percent yield of Na2CO3?
5. Calculate the theoretical mass of H2O produced from the decomposition of 3.00 g NaHCO3 using similar
calculations as above.
1) Given,
mass of NaHCO3 = 3.00 g
moles of NaHCO3 in 3.00 g of NaHCO3 = ?
Note:
Molar mass of NaHCO3 = (23 + 1 + 12 + 3×16) = 84.0 g/mol
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