The formula for crystals of hydrated copper(II) sulfate is CuS*O_{4} * 5H_{2}*O Hydrated copper(II) sulfate is made by reacting copper(II) oxide with dilute sulfuric acid,The overall equation is shown.CuO+H. S*O_{4} + 4H_{3}*O -> CuS*O_{4} * 5H_{3}*OThe crystals are made using the following steps:step 1 50c * m ^ 2 of 0.2mol / d * m ^ 2 dilute sulfuric acid is heated in a beaker. Powdered copper(II) oxide is added until the copper(II) oxide is in excess. Aqueous copper(II) sulfate is formed.step 2The excess copper(II) oxide is separated from the aqueous copper(II) sulfatestep 3The aqueous copper(11) sulfate is heated until a saturated solution is formed.step 4The saturated solution is allowed to cool and crystallise.The crystals are removed and dried.step 5Calculate the maximum mass of copper(II) sulfate crystals, CuS*O_{4} * 5H_{2}*O that can form using the following steps.Calculate the maximum mass of copper(II) sulfate crystals, CuS*O_{4} * 5H_{2}*O that can form usingthe following steps.. Calculate the number of moles of H_{2}*S*O_{4} in 50c * m ^ 3 of 0.2mol / d * m ^ 3 H_{2}*S*O_{4}molDeduce the number of moles of CuS*O_{4} * 5H_{2}*O that can form.mol

The question seems to be asking for the maximum mass of copper(II) sulfate crystals that can be formed and the number of moles of sulfuric acid in a given volume. However, the question is not clearly written and contains several typographical errors, making it difficult to understand.

Here's an attempt to answer based on what I understand:

Step 1: Calculate the number of moles of H2SO4 The volume of the sulfuric acid solution is given as 50 cm^3 and the concentration is 0.2 mol/dm^3.

First, convert the volume from cm^3 to dm^3: 50 cm^3 = 0.05 dm^3

Then, use the formula for calculating moles: moles = concentration * volume So, moles of H2SO4 = 0.2 mol/dm^3 * 0.05 dm^3 = 0.01 mol

Step 2: Deduce the number of moles of CuSO4 * 5H2O that can form From the balanced chemical equation, we can see that 1 mole of H2SO4 reacts with CuO to produce 1 mole of CuSO4 * 5H2O.

So, the number of moles of CuSO4 * 5H2O that can form is equal to the number of moles of H2SO4, which is 0.01 mol.

Step 3: Calculate the maximum mass of CuSO4 * 5H2O The molar mass of CuSO4 * 5H2O is approximately 249.7 g/mol.

So, the maximum mass that can form is: mass = moles * molar mass Mass of CuSO4 * 5H2O = 0.01 mol * 249.7 g/mol = 2.497 g

So, the maximum mass of copper(II) sulfate crystals that can form is approximately 2.497 g.

The question seems to be asking for the calculation of the maximum mass of copper(II) sulfate crystals that can form from a given amount of sulfuric acid. However, the question is not clearly written and contains several typographical errors, making it difficult to understand.

Here's a general approach to solve such problems:

1. Calculate the number of moles of sulfuric acid (H2SO4) in the given volume. The number of moles can be calculated using the formula: moles = concentration * volume.

2. According to the balanced chemical equation, one mole of sulfuric acid reacts with one mole of copper(II) oxide to produce one mole of copper(II) sulfate. Therefore, the number of moles of copper(II) sulfate that can form is equal to the number of moles of sulfuric acid.

3. Calculate the mass of copper(II) sulfate that can form. The mass can be calculated using the formula: mass = moles * molar mass. The molar mass of copper(II) sulfate pentahydrate (CuSO4.5H2O) is approximately 249.7 g/mol.

Please provide the correct values and units for the volume and concentration of sulfuric acid, and I can help you with the calculations.