Final answer:
The question seems to be mistakingly asking for the stoichiometry of aluminum nitrate formation in a reaction that doesn't involve aluminum. It's important to balance chemical equations properly using stoichiometry. The example with copper and silver nitrate shows a 1:2 ratio, producing one mole of copper (II) nitrate per mole of copper reacting.
Step-by-step explanation:
The question seems to be asking for the stoichiometry of a chemical reaction involving copper (Cu) and aluminum nitrate (Al(NO3)3), but the provided chemical reactions and scenarios do not directly involve aluminum reacting to form aluminum nitrate. Instead, they involve reactions between copper, nitric acid (HNO3), and copper(II) nitrate (Cu(NO3)2). Given that there may be a misunderstanding in the question since aluminum is not mentioned to react with any compound to form aluminum nitrate, we can focus on the stoichiometry of the reactions provided which principally concern copper and copper(II) nitrate.
To correctly identify the stoichiometry of a reaction, one would normally balance the reaction equation by ensuring the number of atoms of each element is the same on both sides of the reaction. If we consider the reaction between copper and silver nitrate as an example:
Cu (s) + 2AgNO3(aq) → Cu(NO3)2 (aq) + 2Ag (s)
The balanced equation shows that one mole of copper reacts with two moles of silver nitrate to produce one mole of copper (II) nitrate and two moles of silver. To find the amount of products formed from given reactants, one must use stoichiometry based on the balanced equation, which specifies the ratios of reactants to products.