Final answer:
To determine the mass of nickel(II) perchlorate that contains the same number of moles as 244 g of iron(III) sulfate, divide the mass of iron(III) sulfate by its molar mass to find the number of moles. Then, use the molar ratio between iron(III) sulfate and nickel(II) perchlorate to calculate the mass of nickel(II) perchlorate.
Step-by-step explanation:
To determine the mass of nickel(II) perchlorate that contains the same number of moles as 244 g of iron(III) sulfate, we need to use the concept of molar mass. The molar mass of a compound is the mass of one mole of that compound. First, we need to calculate the number of moles of iron(III) sulfate using its molar mass of 162.2 g/mol. The number of moles can be calculated by dividing the mass of the compound by its molar mass:
Moles = Mass / Molar mass
Moles of iron(III) sulfate = 244 g / 162.2 g/mol ≈ 1.50 moles
Now, we can use the molar ratio between iron(III) sulfate and nickel(II) perchlorate to find the mass of nickel(II) perchlorate. The molar ratio is determined from the balanced chemical equation:
Fe2(SO4)3 + 6 Ni(ClO4)2 → 3 Ni2(SO4)3 + 2 Fe(ClO4)3
We can see that for every 1 mole of iron(III) sulfate, 3 moles of nickel(II) perchlorate are required. Therefore, the mass of nickel(II) perchlorate can be calculated as:
Mass of nickel(II) perchlorate = Moles of nickel(II) perchlorate × Molar mass of nickel(II) perchlorate