Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 3.6 g of iron are to be dissolved in 1.2 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?

To find the minimum volume of the HCl solution required to react with all of the iron, we need to first calculate the amount of iron and then use stoichiometry to determine the number of moles of HCl needed for the reaction.

1. Calculate the number of moles of iron:
The molar mass of iron (Fe) is 55.85 g/mol.
Using the given mass of iron (3.6 g), we can calculate the number of moles:
moles of iron = mass of iron / molar mass of iron
= 3.6 g / 55.85 g/mol

2. Calculate the number of moles of HCl required:
From the balanced chemical equation, we know that one mole of iron reacts with 2 moles of HCl.
So, the number of moles of HCl required is twice the number of moles of iron:
moles of HCl = 2 * moles of iron

3. Calculate the volume of the HCl solution required:
The given concentration of HCl is 1.2 M, which means there are 1.2 moles of HCl in 1 liter (1000 mL) of solution.
From this, we can calculate the volume of the acid solution needed to provide the required number of moles:
volume of HCl solution = (moles of HCl) / (concentration of HCl)
= (moles of HCl) / (1.2 M)

4. Substitute the values and calculate:
volume of HCl solution = (2 * moles of iron) / (1.2 M)
volume of HCl solution = (2 * (3.6 g / 55.85 g/mol)) / (1.2 M)

Now, let's calculate the minimum volume of the acid solution required to react with all of the iron:

volume of HCl solution = (2 * (3.6 g / 55.85 g/mol)) / (1.2 M)

Note: Make sure to convert the final answer to milliliters (mL) if necessary.

To find the minimum volume of the HCl solution required to react with all of the iron, we need to calculate the moles of iron and then determine the volume of the HCl solution needed. Here are the step-by-step calculations:

1. Determine the moles of iron:
- The molar mass of iron (Fe) is 55.85 g/mol.
- Moles of iron = (mass of iron) / (molar mass of iron)
= 3.6 g / 55.85 g/mol

2. Calculate the moles of HCl required:
- The balanced chemical equation for the reaction is:
Fe(s) + 2HCl(aq) -> FeCl2(aq) + H2(g)
- From the balanced equation, we can see that 1 mol of iron reacts with 2 moles of HCl.
- Moles of HCl required = 2 * (moles of iron)

3. Calculate the volume of the HCl solution:
- The concentration of the HCl solution is 1.2 M, which means 1.2 moles of HCl are present in 1 liter (1000 mL) of the solution.
- Volume of HCl solution required = (moles of HCl required) / (concentration of HCl solution)
= (moles of HCl required) / (1.2 mol/L)

4. Convert the volume from liters to milliliters:
- Volume of HCl solution required (in mL) = Volume of HCl solution required (in L) * 1000 mL/L

Let's now calculate the minimum volume of the HCl solution required to react with all of the iron:

1. Moles of iron = (3.6 g) / (55.85 g/mol)
≈ 0.0644 mol

2. Moles of HCl required = 2 * (0.0644 mol)
≈ 0.1288 mol

3. Volume of HCl solution required (in mL) = (0.1288 mol) / (1.2 mol/L)
≈ 0.1073 L * 1000 mL/L
≈ 107.3 mL

Therefore, the minimum volume of the HCl solution required to react with all of the iron is approximately 107.3 mL.

Fe + 2HCl ==> FeCl2 + H2

mols Fe = grams/molar mass = approx 0,06 but you need a better answer than that.
Convert to mols HCl which will be twice mols Fe and you get that from the coefficients in the balanced equation. Then M HCl = mols HCl/L HCl. You have M and mols, solve for L and convert to mL.