To find how many moles of [tex]\( PbI_2 \)[/tex] are formed during the reaction, we need to follow these steps:
1. Determine the stoichiometric relationship from the balanced chemical equation:
The balanced chemical equation is:
[tex]\[
2 \, KI (aq) + Pb(NO_3)_2 (aq) \rightarrow 2 \, KNO_3 (aq) + PbI_2 (s)
\][/tex]
According to the equation, 2 moles of [tex]\( KI \)[/tex] react with 1 mole of [tex]\( Pb(NO_3)_2 \)[/tex] to produce 1 mole of [tex]\( PbI_2 \)[/tex].
2. Given moles of [tex]\( KI \)[/tex]:
It was determined previously that there are 0.025 moles of [tex]\( KI \)[/tex] reacting.
3. Calculate moles of [tex]\( PbI_2 \)[/tex] produced:
Use the stoichiometric relationship from the balanced equation. For every 2 moles of [tex]\( KI \)[/tex], 1 mole of [tex]\( PbI_2 \)[/tex] is produced. Therefore:
[tex]\[
\text{moles of } PbI_2 = \frac{\text{moles of } KI}{2}
\][/tex]
Given 0.025 moles of [tex]\( KI \)[/tex]:
[tex]\[
\text{moles of } PbI_2 = \frac{0.025 \, \text{moles}}{2} = 0.0125 \, \text{moles}
\][/tex]
Thus, the moles of [tex]\( PbI_2 \)[/tex] formed during the reaction are [tex]\( 0.0125 \)[/tex] moles.
