How much copper 2 sulfate do you need to react with 0.5grams of steel wool?
To determine the amount of copper (II) sulfate needed to react with 0.5 grams of steel wool, we first need to understand the stoichiometry of the reaction between the two.
The reaction between copper (II) sulfate and steel wool can be represented by the following balanced chemical equation:
3Fe + 2CuSO4 -> Fe3(SO4)2 + 2Cu
From the equation, we can see that 3 moles of iron (Fe) react with 2 moles of copper (II) sulfate (CuSO4) to produce 1 mole of iron (III) sulfate (Fe3(SO4)2) and 2 moles of copper (Cu).
To calculate the amount of copper (II) sulfate needed, we can follow these steps:
Step 1: Determine the molar mass of steel wool (Fe).
The atomic mass of iron (Fe) is approximately 55.85 grams/mol.
Step 2: Convert the given mass of steel wool to moles.
Using the molar mass of iron (Fe), we can calculate the number of moles of steel wool:
0.5 grams / 55.85 g/mol = 0.00895 moles
Step 3: Use stoichiometry to determine the moles of copper (II) sulfate needed.
From the balanced equation, we know that 3 moles of iron (Fe) react with 2 moles of copper (II) sulfate (CuSO4).
So, we can set up a ratio using the coefficients in the balanced equation:
2 moles of CuSO4 / 3 moles of Fe
Multiplying the moles of steel wool by the stoichiometric ratio:
0.00895 moles * (2/3) = 0.00597 moles of CuSO4
Step 4: Convert moles of copper (II) sulfate to grams.
We can use the molar mass of copper (II) sulfate (CuSO4) to calculate the corresponding mass:
Molar mass of CuSO4 = 63.55 g/mol (copper) + (32.07 g/mol (sulfur) + 4 * 16.00 g/mol (oxygen)) = 159.61 g/mol
Converting moles to grams:
0.00597 moles * 159.61 g/mol = 0.953 grams of CuSO4
Therefore, you would need approximately 0.953 grams of copper (II) sulfate to react with 0.5 grams of steel wool.