Final answer:
To calculate the maximum mass of hydrated copper(II) sulfate crystals, we can use stoichiometry. The maximum mass is approximately 4.79 g.
Step-by-step explanation:
To calculate the maximum mass of hydrated copper(II) sulfate crystals, we need to use stoichiometry.
The balanced chemical equation for the reaction between sulfuric acid (H₂SO₄) and hydrated copper(II) sulfate (CuSO₄·xH₂O) is:
H₂SO₄ + CuSO₄·xH₂O → CuSO₄ + xH₂O
From the equation, we can see that the molar ratio between H₂SO₄ and CuSO₄ is 1:1. Therefore, the number of moles of CuSO₄ that can be made is equal to the number of moles of H₂SO₄ used.
Using the given concentration and volume of H₂SO₄, we can calculate the number of moles of H₂SO₄:
Moles of H₂SO₄ = concentration × volume = 2.00 mol/dm³ × 0.0150 dm³ = 0.0300 mol
Since the molar ratio between H₂SO₄ and CuSO₄ is 1:1, the number of moles of CuSO₄ that can be made is also 0.0300 mol. To calculate the maximum mass of hydrated copper(II) sulfate crystals, we need to know the molar mass of CuSO₄·xH₂O.
To find the molar mass of CuSO₄·xH₂O, we must consider the molar mass of each individual element and account for the number of atoms in the compound. The molar mass of CuSO₄ is 159.61 g/mol.
Now we can calculate the maximum mass of CuSO₄·xH₂O crystals:
Maximum mass = number of moles × molar mass = 0.0300 mol × 159.61 g/mol = 4.79 g
Therefore, the maximum mass of hydrated copper(II) sulfate crystals that could be made is approximately 4.79 g.