Final answer:
The mass of silver sulfadiazine produced, the stoichiometry of Ag2O with C10H10N4SO2 must be understood. Limiting reactant calculations determine the product mass, but without the full equation, the exact mass cannot be concluded. The answer would match one of the provided options with a balanced equation.
Step-by-step explanation:
To calculate the mass of silver sulfadiazine that can be produced from the reaction of Ag2O (silver oxide) with C10H10N4SO2 (sulfadiazine), we need to use the stoichiometry of the balanced chemical equation. However, given that the equation is not provided in the question, the calculation is based on assuming that it proceeds with a 1:1 ratio between Ag2O and C10H10N4SO2 to form one molecule of AgC10H9N4SO2.
To solve the question, we need the molar masses of the compounds involved in the reaction:
- Ag2O (231.735 g/mol)
- C10H10N4SO2 (250.3 g/mol)
- AgC10H9N4SO2 (256 g/mol)
The limiting reactant determines the amount of product that can be formed, so first we calculate the moles of each reactant:
- Moles of Ag2O = 25.0 g / 231.735 g/mol
- Moles of C10H10N4SO2 = 50.0 g / 250.3 g/mol
We then compare the mole ratio to find the limiting reactant. Assuming equal stoichiometry, Ag2O is the limiting reactant. We use its moles to calculate the mass of AgC10H9N4SO2 produced:
Mass of AgC10H9N4SO2 = Moles of Ag2O * 256 g/mol
The answer can be matched to one of the choices provided in the question, assuming we're given the balanced chemical equation. Without it, we cannot definitively conclude the exact mass of product formed.