If 23.5 grams of iron chloride are produced how many grams of iron did you start with?
Write the equation and balance it.
Convert 23.5 grams iron chloride (did you mean iron(II) chloride or iron(III) chloride?)
Using the coefficients in the balanced equation, convert moles iron chloride to moles iron.
Now convert moles iron to grams. g = moles x molar mass.
moles iron chloride = 23.5 g/molar mass.
To determine how many grams of iron you started with, we need to know the stoichiometry of the reaction that produced the iron chloride. The balanced chemical equation will tell us the molar ratios between reactants and products.
Assuming the formation of iron chloride is a single-step reaction, let's consider the balanced equation:
2Fe + 3Cl2 -> 2FeCl3
From this equation, we can see that 2 moles of iron react with 3 moles of chlorine gas to produce 2 moles of iron chloride.
To find the number of moles of iron chloride produced, we can use the formula:
moles = mass / molar mass
The molar mass of FeCl3 (iron chloride) is the sum of the atomic masses of its constituent elements, which can be found on the periodic table. It consists of one iron atom (Fe) and three chlorine atoms (Cl), so:
molar mass of FeCl3 = (atomic mass of Fe) + 3 x (atomic mass of Cl)
Once we know the moles of iron chloride produced, we can use the stoichiometric ratios from the balanced equation to determine the number of moles of iron that reacted to produce that amount of iron chloride.
Finally, we can convert the number of moles of iron reactant to grams using the molar mass of iron (atomic mass of Fe). This will give us the mass of iron present before the reaction.
Please provide the atomic masses of iron (Fe) and chlorine (Cl) to proceed with the calculation.