Final answer:
To answer how many milliliters of 5.1 M H₂SO₄ are required to react with 0.75 g of CuO, the molar mass of CuO is used to calculate the moles, which then allows us to determine the volume needed based on the molarity. The result is 1.85 mL, which does not match the provided answer choices.
Step-by-step explanation:
To calculate how many milliliters of 5.1 M H₂SO₄ are required to react with 0.75 g of CuO, we first need to find the molar mass of CuO: CuO = 63.55 g/mol (Cu) + 16.00 g/mol (O) = 79.55 g/mol. Next, the number of moles of CuO is calculated: 0.75 g CuO × (1 mol/79.55 g) = 0.00943 mol CuO.
According to the balanced chemical equation, 1 mole of CuO reacts with 1 mole of H₂SO₄. Therefore, 0.00943 mol of CuO would need 0.00943 mol of H₂SO₄ to react completely. Since the concentration of H₂SO₄ is 5.1 M, we can find the volume required using: Volume = moles of solute / molarity = 0.00943 mol / 5.1 M = 0.00185 L or 1.85 mL.
So the volume of 5.1 M H₂SO₄ needed is 1.85 mL, which is not listed in your options as a possible answer. Therefore, please check the question details and options again or confirm if there are any constraints or assumptions we haven't considered.