Suppose that you have an unlimited supply of copper (I) chloride to react with iron. How many moles of copper would beproduced by reacting 94.0 g of iron with the copper (II) chloride solution?
2. How many moles of iron would have been used up if 35.0 g of copper were to be produced?
3. How many atoms of copper would be involved in problem 2?
4. How many atoms of iron would be involved in problem 2?
5. How many grams of copper would be produced if 333 g of iron were reacted?
1. To determine the number of moles of copper produced, we need to use the molar mass of iron. The molar mass of iron is 55.85 g/mol.
First, we need to convert the mass of iron (94.0 g) to moles:
Number of moles of iron = mass of iron / molar mass of iron
Number of moles of iron = 94.0 g / 55.85 g/mol
Number of moles of iron = 1.683 mol
The stoichiometric ratio between iron and copper in the reaction is 2:1. This means that for every 2 moles of iron reacted, 1 mole of copper is produced.
Number of moles of copper produced = (1.683 mol x 1 mol of copper) / 2 mol of iron
Number of moles of copper produced = 0.8415 mol
Therefore, 0.8415 moles of copper would be produced by reacting 94.0 g of iron.
2. The stoichiometric ratio between copper and iron is still 2:1. This means that for every 2 moles of iron reacted, 1 mole of copper is produced.
First, we need to convert the mass of copper (35.0 g) to moles:
Number of moles of copper = mass of copper / molar mass of copper
Number of moles of copper = 35.0 g / 63.55 g/mol
Number of moles of copper = 0.55 mol
Number of moles of iron used up = (0.55 mol x 2 mol of iron) / 1 mol of copper
Number of moles of iron used up = 1.10 mol
Therefore, 1.10 moles of iron would have been used up if 35.0 g of copper were to be produced.
3. In problem 2, we determined that 1.10 moles of iron would have been used up. Since the stoichiometric ratio between copper and iron is 2:1, there would be twice the number of moles of copper.
Number of moles of copper involved = 1.10 mol x 2
Number of moles of copper involved = 2.20 mol
To determine the number of atoms of copper, we need to multiply the number of moles by Avogadro's number:
Number of atoms of copper involved = 2.20 mol x 6.022 x 10^23 atoms/mol
Number of atoms of copper involved = 1.3244 x 10^24 atoms
Therefore, there would be 1.3244 x 10^24 atoms of copper involved in problem 2.
4. In problem 2, we determined that 1.10 moles of iron would have been used up. To determine the number of atoms of iron involved, we need to multiply the number of moles by Avogadro's number:
Number of atoms of iron involved = 1.10 mol x 6.022 x 10^23 atoms/mol
Number of atoms of iron involved = 6.6322 x 10^23 atoms
Therefore, there would be 6.6322 x 10^23 atoms of iron involved in problem 2.
5. The stoichiometric ratio between iron and copper in the reaction is 2:1. This means that for every 2 moles of iron reacted, 1 mole of copper is produced.
First, we need to convert the mass of iron (333 g) to moles:
Number of moles of iron = mass of iron / molar mass of iron
Number of moles of iron = 333 g / 55.85 g/mol
Number of moles of iron = 5.965 mol
Number of moles of copper produced = (5.965 mol x 1 mol of copper) / 2 mol of iron
Number of moles of copper produced = 2.9825 mol
To determine the mass of copper produced, we need to use the molar mass of copper:
Mass of copper produced = number of moles of copper produced x molar mass of copper
Mass of copper produced = 2.9825 mol x 63.55 g/mol
Mass of copper produced = 189.49 g
Therefore, 189.49 grams of copper would be produced if 333 g of iron were reacted.