Final answer:
To identify the limiting reagent in the reaction between CuO and H₂SO₄, first calculate the moles of each reactant and compare the amounts. The reactant with the lower number of moles is the limiting reagent. Then, use the stoichiometric ratios to calculate the moles of the product formed.
Step-by-step explanation:
In the reaction CuO + H₂SO₄ → CuSO₄ + H₂O, the limiting reagent can be identified by comparing the stoichiometric ratios of the reactants. The moles of CuO and H₂SO₄ are in a 1:1 ratio, meaning that if there is an equal amount of moles for both reactants, neither will be in excess. However, if one reactant is present in a lower amount, it will be completely consumed, making it the limiting reagent. In this case, the moles of CuO and H₂SO₄ can be determined and compared to identify the limiting reagent.
First, convert the grams of CuO and H₂SO₄ to moles by dividing by their respective molar masses: CuO (63.55 g/mol) and H₂SO₄ (98.09 g/mol). Then, compare the number of moles to see which reactant is present in a lower amount. The reactant with the lower number of moles is the limiting reagent.
Finally, calculate the moles of the product formed using the stoichiometric ratios provided by the balanced equation.