Final answer:
Without a specific chemical reaction equation, it is impossible to determine the limiting reactant when 6.50 g O2 are reacted with 8.75 g N2 and 12.5 g H2O as the stoichiometric relationships between the reactants are unknown.
Step-by-step explanation:
To identify the limiting reactant when 6.50 g of O2 are reacted with 8.75 g of N2 and 12.5 g of H2O, we first need to know the chemical equation for the reaction. However, without a specific reaction provided, we cannot determine the limiting reactant because the stoichiometry is not clear. For the purpose of this exercise, let's assume a hypothetical reaction where both O2 and N2 are reactants (likely in the presence of a catalyst since these elements do not typically react directly) and H2O is a product. To determine the limiting reactant, we compare the mole ratio of reactants to that required by the equation.
For example, if the reaction were:
2H2 + O2 → 2H2O
The molar mass of H2 is about 2.02 g/mol and of O2 is about 32.00 g/mol. In comparing moles, we need 2 moles of H2 for every mole of O2. If you had 8.75 g of N2 (with a molar mass of about 28.02 g/mol) react with O2, you would have to ensure the N2 is involved in a balanced chemical equation to identify the actual limiting reactant. As such, without a balanced equation involving N2, we cannot correctly answer which is the limiting reactant among O2, N2, and H2O.
You are encouraged to look for the balanced chemical equations involving these reactants to perform the correct stoichiometric calculations.