Final answer:
Approximately 17.0 grams of silver oxide (Ag2O) is required to produce 25.0 grams of silver sulfadiazine, based on stoichiometry and molar mass calculations.
Step-by-step explanation:
To calculate the mass of silver oxide, Ag2O, required to produce 25.0 g of silver sulfadiazine, AgC10H9N4SO2, from its reaction with sulfadiazine, we need to use stoichiometry. First, we should calculate the molar mass of both compounds. The molar mass of silver sulfadiazine is approximately 357.14 g/mol, and the molar mass of silver oxide is approximately 231.74 g/mol.
The balanced chemical equation given is:
2C10H10N4SO2 + Ag2O → 2AgC10H9N4SO2 + H2O
Next, we'll convert the mass of silver sulfadiazine to moles:
(25.0 g AgC10H9N4SO2) / (357.14 g/mol) = Approximately 0.070 moles
Since the reaction shows a 1:1 mole ratio between AgC10H9N4SO2 and Ag2O, this means 0.070 moles of Ag2O is also required. To find the mass of Ag2O:
(0.070 moles) x (231.74 g/mol) = Approximately 16.2 g
Therefore, the closest answer to this calculation is 17.0 g, which corresponds to option (a).