what mass of copper may be produced when excess CuSO4 is reacted with 100g of aluminum metal?
assistance needed
Balance the reaction first.
Then, figure the moles of Al in 100 g of Al.
Now, use the mole relationships to figure themoles of Cu.
We will be happy to critique your thinking.
To determine the mass of copper that can be produced from the reaction between excess CuSO4 (copper sulfate) and 100g of aluminum metal, we need to balance the chemical equation and use stoichiometry.
The balanced chemical equation for the reaction is:
2Al + 3CuSO4 → Al2(SO4)3 + 3Cu
From the equation, we see that 2 moles of aluminum (Al) react with 3 moles of copper sulfate (CuSO4) to produce 3 moles of copper (Cu).
First, we need to convert the 100g of aluminum to moles. The molar mass of aluminum is 26.98 g/mol.
Moles of aluminum = Mass of aluminum / Molar mass of aluminum
Moles of aluminum = 100g / 26.98 g/mol ≈ 3.705 mol
Since the reaction ratio between aluminum and copper is 2:3, we can determine the moles of copper produced.
Moles of copper = Moles of aluminum × (3 moles of copper / 2 moles of aluminum)
Moles of copper = 3.705 mol × (3/2)
Moles of copper = 5.558 mol
Finally, we can calculate the mass of copper produced by multiplying the moles of copper by its molar mass. The molar mass of copper is 63.55 g/mol.
Mass of copper = Moles of copper × Molar mass of copper
Mass of copper = 5.558 mol × 63.55 g/mol ≈ 353.25 g
Therefore, approximately 353.25 grams of copper can be produced when 100g of aluminum reacts with excess CuSO4.