Consider the following balanced chemical equation: 2Fe(s)+3Pb(NO_(3))_(2)(aq)arrow 3Pb(s)+2Fe(NO_(3)) If 53.6 moles of Fe are reacted, how many moles of Pb were formed?

To determine the number of moles of lead (Pb) formed when 53.6 moles of iron (Fe) are reacted, we need to use the stoichiometric relationship from the balanced chemical equation:<br /><br />\[ 2Fe(s) + 3Pb(NO_3)_2(aq) \rightarrow 3Pb(s) + 2Fe(NO_3)_3(aq) \]<br /><br />From the equation, we see that 2 moles of Fe produce 3 moles of Pb. This gives us the mole ratio:<br /><br />\[ \frac{3 \text{ moles of Pb}}{2 \text{ moles of Fe}} \]<br /><br />Now, we can use this ratio to find the number of moles of Pb formed from 53.6 moles of Fe:<br /><br />\[ \text{Moles of Pb} = 53.6 \text{ moles of Fe} \times \frac{3 \text{ moles of Pb}}{2 \text{ moles of Fe}} \]<br /><br />\[ \text{Moles of Pb} = 53.6 \times \frac{3}{2} \]<br /><br />\[ \text{Moles of Pb} = 53.6 \times 1.5 \]<br /><br />\[ \text{Moles of Pb} = 80.4 \]<br /><br />Therefore, 80.4 moles of Pb were formed when 53.6 moles of Fe were reacted.