Iron reacts with HCl solution to give H2 gas and Fe2+ ions. Suppose that 5.3 g of iron are to be dissolved in 1.7 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 understand the stoichiometry of the reaction.
From the given information, we know that iron (Fe) reacts with HCl to produce hydrogen gas (H2) and Fe2+ ions.
The balanced chemical equation for this reaction is:
Fe + 2HCl -> FeCl2 + H2
According to the equation, 1 mole of iron reacts with 2 moles of HCl to produce 1 mole of hydrogen gas. This means that the ratio of iron to HCl is 1:2.
First, we need to calculate the number of moles of iron in 5.3 g. To do this, we use the molar mass of iron (Fe), which is 55.845 g/mol.
Number of moles of iron = mass of iron / molar mass of iron
Number of moles of iron = 5.3 g / 55.845 g/mol
Number of moles of iron ≈ 0.095 moles
Since the ratio of iron to HCl is 1:2, the number of moles of HCl required will be twice the number of moles of iron.
Number of moles of HCl = 2 * Number of moles of iron
Number of moles of HCl ≈ 2 * 0.095 moles
Number of moles of HCl ≈ 0.19 moles
Now, we can use the given concentration of HCl to determine the volume of the acid solution required.
Concentration of HCl = 1.7 M
Molarity (M) is defined as moles of solute divided by liters of solution. Rearranging the formula, we get:
Volume of HCl = Number of moles of HCl / Concentration of HCl
Volume of HCl = 0.19 moles / 1.7 M
Volume of HCl ≈ 0.112 L
Finally, we convert the volume from liters to milliliters:
Volume of HCl = 0.112 L * 1000 mL/L
Volume of HCl ≈ 112 mL
Therefore, the minimum volume of the HCl solution required to react with all of the iron is approximately 112 mL.
To find the minimum volume of the HCl solution required to react with all of the iron, we will need to calculate the number of moles of iron and then use stoichiometry to determine the volume of the HCl solution.
1. Calculate the number of moles of iron:
Molar mass of iron (Fe) = 55.85 g/mol
Number of moles of iron = mass / molar mass = 5.3 g / 55.85 g/mol
2. Use stoichiometry to determine the volume of HCl:
The balanced chemical equation for the reaction is:
Fe(s) + 2HCl(aq) -> FeCl2(aq) + H2(g)
From the equation, it is clear that 1 mole of iron reacts with 2 moles of HCl.
Number of moles of HCl required = 2 * number of moles of iron
3. Calculate the volume of HCl solution:
Molarity (M) = number of moles / volume (in L)
Rearrange the equation to solve for the volume:
Volume (in L) = number of moles / Molarity
Given: Molarity = 1.7 M (since HCl is 1.7 M)
Number of moles of HCl = 2 * number of moles of iron
Using the values obtained in step 1 and step 3, we can now calculate the volume of the HCl solution in liters.
4. Convert the volume to milliliters:
1 L = 1000 mL
Now, let's perform the calculations:
Step 1:
Number of moles of iron = 5.3 g / 55.85 g/mol
Step 3:
Number of moles of HCl = 2 * (5.3 g / 55.85 g/mol)
Volume of HCl solution (in L) = (2 * 5.3 g / 55.85 g/mol) / 1.7 M
Step 4:
Volume of HCl solution (in mL) = Volume (in L) * 1000 mL/L
Calculate the values to find the minimum volume of the HCl solution required to react with all of the iron.
Here is a worked example of a stoichiometry problem such as this. After you determine the mole HCl, then M = mole/L. You ave moles and M, solve for L and convert to mL.
http://www.jiskha.com/science/chemistry/stoichiometry.html