how much HCl is needed to dissolve a 2.5grams iron bar on a padlock
To determine how much hydrochloric acid (HCl) is needed to dissolve a 2.5 gram iron bar on a padlock, we need to consider the stoichiometry of the reaction between iron and hydrochloric acid. The balanced chemical equation for this reaction is:
Fe + 2HCl -> FeCl2 + H2
From this equation, we can see that 1 mole of iron (Fe) reacts with 2 moles of hydrochloric acid (HCl) to produce 1 mole of iron(II) chloride (FeCl2) and 1 mole of hydrogen gas (H2).
To calculate the amount of HCl needed, we'll follow these steps:
1. Calculate the molar mass of iron (Fe) using the periodic table. The atomic mass of iron is approximately 55.85 g/mol.
2. Convert the mass of the iron bar (2.5 grams) to moles by dividing it by the molar mass of Fe.
Moles of Fe = 2.5 g / 55.85 g/mol
3. Since the reaction stoichiometry is 1:2 between Fe and HCl, to fully react with the moles of Fe calculated in step 2, we need twice the number of moles of HCl.
Moles of HCl = 2 * Moles of Fe
4. Finally, convert the moles of HCl to grams by multiplying it by the molar mass of HCl (approximately 36.46 g/mol).
Grams of HCl = Moles of HCl * 36.46 g/mol
By following these calculations, you can determine the amount of HCl needed to dissolve a 2.5 gram iron bar on a padlock.