How many moles of iron would have been used up if 35.0 g of copper were to be produced?
To determine the number of moles of iron that would have been used up, we need to first find the molar ratio between iron and copper using the balanced chemical equation.
The balanced chemical equation for the reaction between iron and copper is:
Fe + CuSO4 -> FeSO4 + Cu.
From the equation, we can see that 1 mole of iron reacts with 1 mole of copper.
Next, we need to calculate the number of moles of copper that would be produced from 35.0 g of copper. We can use the molar mass of copper (Cu) to convert grams to moles.
The molar mass of copper is 63.55 g/mol.
Number of moles of copper = Mass of copper / Molar mass of copper
= 35.0 g / 63.55 g/mol
≈ 0.55 mol.
Since the molar ratio between iron and copper is 1:1, the number of moles of iron used up will also be 0.55 moles.