Final answer:
The question requires applying stoichiometry to a precipitation reaction between potassium chromate and silver nitrate to calculate the mass of silver chromate precipitate formed. This involves identifying the limiting reactant, calculating the moles of precipitate, and then converting this to mass using the molar mass.
Step-by-step explanation:
The question addresses the process of a precipitation reaction in a stoichiometry problem involving the chemical reaction between potassium chromate (K₂CrO₄) and silver nitrate (AgNO₃), where silver chromate (Ag₂CrO₄) is the precipitate formed. To solve the problem, the first step is to identify the limiting reactant by calculating the number of moles of each reactant based on their concentrations and volumes provided. Since the reaction shows that two moles of AgNO₃ are required for every one mole of K₂CrO₄, the limiting reactant can be found by comparing the stoichiometric ratios of the reactants.
Once the limiting reactant is known, the moles of Ag₂CrO₄ that can form are determined. This number is then multiplied by the molar mass of Ag₂CrO₄ to find the mass of precipitate. It’s important to note that any reactant in excess will not affect the amount of precipitate formed beyond the stoichiometric relationship defined by the balanced equation.
For a better understanding of what happens in solution, a more informative approach is to write a complete ionic equation, revealing the actual species in solution, including those that form the solid precipitate. Through this analysis, the mass of the precipitate can be accurately calculated, which also highlights concepts like stoichiometry, limiting reactant analysis, precipitation reactions, and molar calculations.