Final answer:
The synthesis of sodium bicarbonate involves adding carbon dioxide to sodium carbonate, and three soluble carbonate salts include sodium carbonate, potassium carbonate, and ammonium carbonate. To find the amount of carbon dioxide produced from carbonic acid and to calculate theoretical and actual yields of a chemical reaction, molar masses and stoichiometry are used.
Step-by-step explanation:
Predicting Chemical Equations and Calculating Theoretical and Actual Yields
To synthesize sodium bicarbonate (NaHCO3), carbon dioxide (CO2) is bubbled through a solution of ammonia and sodium chloride, leading to the formation of ammonium carbonate, which then reacts with NaCl to form sodium bicarbonate and ammonium chloride. The chemical equation for synthesis of sodium bicarbonate from sodium carbonate (Na2CO3) is as follows:
Na2CO3 + CO2 + H2O → 2 NaHCO3
To predict the equation for the synthesis of sodium carbonate, one could use the decomposition of sodium bicarbonate:
2 NaHCO3 → Na2CO3 + CO2 + H2O
Three soluble carbonate salts include sodium carbonate (Na2CO3), potassium carbonate (K2CO3), and ammonium carbonate ((NH4)2CO3). From 6.20 g of carbonic acid (H2CO3), we can calculate the amount of carbon dioxide produced by using the molar mass of H2CO3 and the stoichiometry of its decomposition reaction:
H2CO3 → H2O + CO2
Finally, to balance the given reaction and calculate the theoretical yield of B2H6 from 10.5 g of NaBH4, it's essential to write correct formulas and apply stoichiometry. The balanced reaction and yield calculations require molar masses and the stoichiometric relationship between reactants and products. If the actual yield is 3.24 g of B2H6, the percent yield can be calculated from the theoretical yield.