Copper sulfate is a blue solid that is used as an algicide. Solutions of copper sulfate that come in contact with zinc metal such as the surface of galvanized (zinc-plated) steel- undergo the following reaction that forms copper metal on the zinc surface:

CuSO4(aq)+Zn(s) ---> Cu(s)+ZnSO4(aq)

How many grams of zinc could 454g of copper sulfate react with?

The balanced equation shows mole for mole of zinc reacting with coppersulfate, and one gets a mole of copper from the reaction. So convert 454g of copper sulfate to moles. The main difficulty for me is the description of the problem: Copper sulfate is a blue solid....Hmmm. This has to be copper(II) sulfate pentahydrate, not CuSO4 (a white powder).

So I wonder what the 454 grams is actually refering to. Perhaps it will be a mystery.

To determine the number of grams of zinc that can react with 454g of copper sulfate, we need to use the molar ratios from the balanced chemical equation.

The molar mass of copper sulfate (CuSO4) is calculated as follows:
1 atom of copper (Cu) = 1 * 63.546 = 63.546 g/mol
1 atom of sulfur (S) = 1 * 32.06 = 32.06 g/mol
4 atoms of oxygen (O) = 4 * 16.00 = 64.00 g/mol
Total molar mass of copper sulfate (CuSO4) = 63.546 + 32.06 + 64.00 = 159.606 g/mol

Now, we can calculate the moles of copper sulfate (CuSO4) using its molar mass:
454g * (1 mol / 159.606 g) = 2.845 mol

From the balanced chemical equation, we can see that the molar ratio of copper sulfate (CuSO4) to zinc (Zn) is 1:1. This means that for every 1 mol of copper sulfate (CuSO4) reacted, 1 mol of zinc (Zn) is consumed.

Therefore, the number of moles of zinc (Zn) that can react with 454g of copper sulfate is also 2.845 mol.

Finally, we can calculate the grams of zinc (Zn) that can react with 454g of copper sulfate using the molar mass of zinc:
2.845 mol * (65.38 g / mol) = 186.1 g

Therefore, 454g of copper sulfate can react with approximately 186.1 g of zinc.

To determine how many grams of zinc could react with 454g of copper sulfate, we need to use stoichiometry and the balanced chemical equation provided.

First, let's find the molar mass of copper sulfate (CuSO4). The molar masses are:

- Cu: 63.55 g/mol
- S: 32.07 g/mol
- O: 16.00 g/mol (there are four oxygen atoms in CuSO4)
- Total molar mass: 63.55 + 32.07 + (16.00 x 4) = 159.61 g/mol

Next, we need to determine the number of moles of copper sulfate present in 454g. To do this, we'll use the formula:

moles = mass / molar mass

moles = 454g / 159.61 g/mol ≈ 2.846 moles

Now, let's use the balanced chemical equation to find the mole ratio between copper sulfate (CuSO4) and zinc (Zn). According to the equation, the ratio is 1:1:

CuSO4(aq) + Zn(s) → Cu(s) + ZnSO4(aq)

This means that for every one mole of copper sulfate, we need one mole of zinc.

Since the ratio is 1:1, the number of moles of zinc required will be equal to the number of moles of copper sulfate, which is approximately 2.846 moles.

Finally, we can find the mass of zinc using its molar mass. The molar mass of zinc (Zn) is 65.38 g/mol.

mass of zinc = moles of zinc × molar mass of zinc
mass of zinc = 2.846 moles × 65.38 g/mol ≈ 186.15 g

Therefore, approximately 186.15 grams of zinc could react with 454 grams of copper sulfate.