Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 6.5 g of iron are to be dissolved in 1.4 M HCl. What is the minimum volume (in mL) of the acid solution required to react with all of the iron?
Here is a worked example of a stoichiometry problem. After find the number of moles HCl, use M = moles/L to solve for L and convert to mL.
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To determine the minimum volume of HCl solution required to react with all of the iron, we first need to calculate the moles of iron present in 6.5 g of iron.
The molar mass of iron (Fe) is 55.845 g/mol. Thus, the number of moles of iron can be calculated as follows:
moles of iron = mass of iron / molar mass of iron
moles of iron = 6.5 g / 55.845 g/mol
moles of iron ≈ 0.1162 mol
Now, let's consider the balanced chemical equation for the reaction between iron and hydrochloric acid:
Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)
From the balanced equation, we can see that 1 mole of iron reacts with 2 moles of HCl.
Therefore, the number of moles of HCl required will be twice the number of moles of iron:
moles of HCl required = 2 * moles of iron
moles of HCl required = 2 * 0.1162 mol
moles of HCl required ≈ 0.2324 mol
Now, we can use the molarity and the moles of HCl to calculate the volume of HCl solution required.
The molarity of the HCl solution is given as 1.4 M, which means 1.4 moles of HCl are present in 1 liter (1000 mL) of solution.
Using the formula:
volume (in liters) = moles / molarity
volume (in liters) = 0.2324 mol / 1.4 M
volume (in liters) ≈ 0.1663 L
Finally, we convert the volume from liters to milliliters:
volume (in mL) = 0.1663 L * 1000 mL/L
volume (in mL) ≈ 166.3 mL
Therefore, the minimum volume of the HCl solution required to react with all of the iron is approximately 166.3 mL.
To determine the minimum volume of the HCl solution required to react with all of the iron, we first need to calculate the number of moles of iron present in 6.5 g of iron.
1. Calculate the molar mass of iron (Fe):
The molar mass of iron (Fe) is approximately 55.85 g/mol.
2. Calculate the number of moles of iron (Fe) in 6.5 g of iron:
Number of moles = Mass / Molar mass
Number of moles = 6.5 g / 55.85 g/mol
Now, we need to determine the stoichiometry of the reaction between iron and HCl. From the given information, we know that the reaction produces H2 gas and Fe2+ ions. The balanced chemical equation for the reaction is:
2 Fe(s) + 6 HCl(aq) → 2 FeCl3(aq) + 3 H2(g)
This balanced equation tells us that for every 2 moles of iron (Fe), we need 6 moles of HCl to completely react. Therefore, we can determine the moles of HCl required.
3. Calculate the moles of HCl required to react with all of the iron:
Moles of HCl = (Moles of Fe / 2) * 6
4. Calculate the volume of the acid solution required:
Volume (in L) = Moles of HCl / Molarity
Volume (in mL) = (Volume in L) * 1000
Plug in the values to get the final answer:
Moles of Fe = 6.5 g / 55.85 g/mol
Moles of HCl = (Moles of Fe / 2) * 6
Volume (in L) = Moles of HCl / Molarity
Volume (in mL) = (Volume in L) * 1000
Thus, by performing these calculations, you can find the minimum volume (in mL) of the HCl solution required to react with all of the iron.