Final answer:
The amount of aluminum nitrate produced from 15.5 grams of barium nitrate can be calculated using stoichiometry, which involves converting grams of barium nitrate to moles, using the molar ratio from the balanced equation, and converting moles of aluminum nitrate back to grams.
Step-by-step explanation:
To determine the amount of aluminum nitrate that can be produced from the reaction of 15.5 grams of barium nitrate and excess aluminum sulfate, we must use stoichiometry.
Steps:
- Write the balanced chemical equation.
- Calculate the number of moles of barium nitrate.
- Use the mole ratio from the balanced equation to find the moles of aluminum nitrate that can be formed.
- Convert moles of aluminum nitrate to grams to find the answer.
Without the balanced equation and molar masses, we cannot provide a precise answer. However, typically we would divide the initial mass of barium nitrate by its molar mass to find the moles of barium nitrate available for the reaction. Then, we would multiply these moles by the stoichiometric mole ratio between barium nitrate and aluminum nitrate, obtained from the balanced chemical equation. Finally, we would multiply the moles of aluminum nitrate by its molar mass to find the mass in grams of aluminum nitrate produced.