To find the mass of ferric ions (Fe³⁺) required to react with 1.5 moles of stannous ions (Sn²⁺), follow the steps below:
1. Determine the stoichiometric ratio:
The balanced chemical equation given is:
[tex]\[
Sn^{++} + 2Fe^{+++} \longrightarrow Sn^{+++} + 2Fe^{++}
\][/tex]
According to the equation, 1 mole of [tex]\( Sn^{++} \)[/tex] reacts with 2 moles of [tex]\( Fe^{+++} \)[/tex].
2. Calculate the moles of [tex]\( Fe^{+++} \)[/tex] required:
Since 1 mole of [tex]\( Sn^{++} \)[/tex] requires 2 moles of [tex]\( Fe^{+++} \)[/tex], then 1.5 moles of [tex]\( Sn^{++} \)[/tex] will require:
[tex]\[
1.5 \text{ moles of } Sn^{++} \times 2 = 3 \text{ moles of } Fe^{+++}
\][/tex]
3. Find the atomic mass of iron (Fe):
The atomic mass of Fe is given as 56 atomic mass units (amu).
4. Calculate the mass of [tex]\( Fe^{+++} \)[/tex] required:
The mass of a substance in grams can be found by multiplying the number of moles by its atomic mass. Therefore, the mass of 3 moles of [tex]\( Fe^{+++} \)[/tex] is given by:
[tex]\[
\text{Mass of } Fe^{+++} = 3 \text{ moles} \times 56 \text{ amu}
\][/tex]
5. Perform the multiplication to get the final mass:
[tex]\[
\text{Mass of } Fe^{+++} = 3 \times 56 = 168 \text{ grams}
\][/tex]
So, the mass of ferric ions (Fe³⁺) required to react with 1.5 moles of stannous ions (Sn²⁺) is 168 grams.
