Final answer:
The question contains an inaccurate representation of chemical reactivity as NaHCO₃ and CaCl₂ do not directly react in a simple exchange to form CaCO₃. For a proper stoichiometric calculation, the actual reaction conditions and the balanced equations for the actual reaction pathway need to be provided.
Step-by-step explanation:
To determine how many grams of solid CaCO₃ should precipitate out when 1.00 g of NaHCO₃ reacts with an excess amount of CaCl₂, we first need to write the balanced chemical equation. The reaction between sodium bicarbonate (NaHCO₃) and calcium chloride (CaCl₂) that leads to the formation of solid calcium carbonate (CaCO₃) is as follows:
NaHCO₃ + CaCl₂ → CaCO₃(s) + 2 NaCl + CO₂ + H₂O
However, it is important to note that this reaction is not straightforward because NaHCO₃ and CaCl₂ do not directly react in a simple exchange reaction to produce CaCO₃. Instead, the formation of CaCO₃ would typically occur in an aqueous environment where NaHCO₃ can react with a calcium-containing solution, possibly through a different reaction pathway involving intermediate steps. Therefore, we cannot give a definitive answer based on the information provided. Additional details about the reaction conditions and the actual balanced equations for the intermediate steps would be required to perform a stoichiometric calculation to find the mass of CaCO₃ that would precipitate.