Iron is attacked by acids when an iron nail of mass m = 1.5 g is placed in

Question

a volume V = 10mL of a hydrochloric acid solution (H* + CI-) of concentration
C = 0.8mol. L-1
, we observe a gaseous release of dihydrogen (H2) and femmation
of iron II ions (Fe?+).
© Write the balance equation for the reaction and indicate the torques involved.
® Take stock of the species present in the initial state.
• Has the nail been completely destroyed?
© Accurately indicate the quantities of materials present in the solution when the reaction is complete.
© What is the volume of hydrogen released by this reaction?
What is the concentration of iron II ions and H+ ions when the reaction is complete?
Data
: "The molar volume under the experimental conditions: V M = 24L/mol
• The molar mass of iron: M (Fe) = 55.8g/mol

Answer 1

The balanced equation for the reaction between iron and hydrochloric acid can be written as:

Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)

The torques involved in this reaction are the release of dihydrogen gas and the formation of iron II ions.

In the initial state, we have a 1.5 g iron nail and a volume of 10 mL hydrochloric acid solution with a concentration of 0.8 mol/L. The species present are iron (Fe), hydrochloric acid (HCl), hydrogen ions (H+), and chloride ions (Cl-).

The nail may not be completely destroyed, but it will react with the hydrochloric acid to form iron II ions and release dihydrogen gas.

To determine the quantities of materials present in the solution when the reaction is complete, we need to use the mole ratios from the balanced equation.

From the balanced equation, we can see that 1 mole of iron reacts with 2 moles of hydrochloric acid to produce 1 mole of iron II ions and 1 mole of dihydrogen gas.

Using the given molar mass of iron (55.8 g/mol), we can calculate the number of moles of iron present:
Number of moles of iron = mass / molar mass = 1.5 g / 55.8 g/mol ≈ 0.0269 mol

Since the mole ratio between iron and hydrochloric acid is 1:2, the number of moles of hydrochloric acid consumed is twice the number of moles of iron:
Number of moles of HCl consumed = 2 * number of moles of iron = 2 * 0.0269 mol = 0.0538 mol

Using the given concentration of hydrochloric acid (0.8 mol/L) and the volume of solution (10 mL), we can calculate the number of moles of HCl present:
Number of moles of HCl = concentration * volume = 0.8 mol/L * 0.01 L = 0.008 mol

Therefore, the remaining moles of HCl after the reaction is complete are:
Remaining moles of HCl = initial moles of HCl - moles of HCl consumed = 0.008 mol - 0.0538 mol = -0.0458 mol

Since the reaction is complete, all of the hydrochloric acid is consumed, and the final amount of HCl becomes 0 moles.

The volume of hydrogen released by this reaction can be calculated by using the molar volume under the experimental conditions:
Volume of hydrogen = moles of H2 * molar volume = 0.0269 mol * 24 L/mol = 0.6464 L or 646.4 mL

When the reaction is complete, all of the iron is converted into iron II ions (Fe2+). Since the initial volume of the solution is 10 mL and the concentration of iron II ions is not given, we do not have enough information to determine the concentration of iron II ions when the reaction is complete.

Similarly, since the concentration of H+ ions is not given, we do not have enough information to determine the concentration of H+ ions when the reaction is complete.