How many Moles of Aluminum are needed to completely react with the 1.50 moles of copper 2 sulfate you collected. ( equation: 2Al + 3CuSO4 —> Al2(SO4)3 + 3Cu
2Al + 3CuSO4 —> Al2(SO4)3 + 3Cu
Did you collect 1.50 mols CuSO4 and use that in this reaction? Are you asking how many mols Al are needed to react with 1.50 mols CuSO4? I assume that's the question. Look at the coefficients. They tell you that 2 mols Al will react with 3 mols CuSO4; therefore,
1.50 mols CuSO4 x ( 2 mols Al/3 mols CuSO4) = 1.50 x 2/3 = ?
To determine the number of moles of aluminum needed to completely react with 1.50 moles of copper (II) sulfate (CuSO4), we need to use the stoichiometry of the balanced chemical equation.
From the equation: 2Al + 3CuSO4 → Al2(SO4)3 + 3Cu
We can see that 2 moles of aluminum react with 3 moles of copper (II) sulfate. This means that the ratio of moles of aluminum to moles of copper (II) sulfate is 2:3.
To find the number of moles of aluminum needed, we can use the following proportion:
2 moles Al / 3 moles CuSO4 = x moles Al / 1.50 moles CuSO4
Cross-multiplying:
(2 moles Al)(1.50 moles CuSO4) = (3 moles CuSO4)(x moles Al)
3 moles Al = (2 moles Al)(1.50 moles CuSO4) / (3 moles CuSO4)
3 moles Al = 1.50 moles Al
Therefore, to completely react with 1.50 moles of copper (II) sulfate, you would need 1.50 moles of aluminum.
To determine the number of moles of aluminum needed to react with 1.50 moles of copper(II) sulfate (CuSO4), we first need to establish the stoichiometric relationship between the two substances using the balanced chemical equation provided:
2Al + 3CuSO4 → Al2(SO4)3 + 3Cu
According to the equation, 2 moles of aluminum (Al) react with 3 moles of copper(II) sulfate (CuSO4). This means that the mole ratio between Al and CuSO4 is 2:3.
To find the number of moles of aluminum required, we can set up a proportion using this mole ratio:
(2 moles Al / 3 moles CuSO4) = (x moles Al / 1.50 moles CuSO4)
Cross-multiplying the proportion:
(2 moles Al)(1.50 moles CuSO4) = (3 moles CuSO4)(x moles Al)
3 moles Al = (2 moles Al)(1.50 moles CuSO4) / (3 moles CuSO4)
Now, we can plug in the values and solve for x:
x = (2)(1.50) / 3
x = 1.00
Therefore, 1.00 mole of aluminum is required to completely react with the 1.50 moles of copper(II) sulfate.