Question

for each reaction, write the chemical formulae of the oxidized reactants in the space provided. write the che provided.

$$\
LATEXBLOCK0
} \\\\ { 2 \\mathrm { fe } ( s ) + 3 \\mathrm { pb } \\left( \\mathrm { no } _ { 3 } \ ight) _ { 2 } ( a q ) \ ightarrow 3 \\mathrm { pb } ( s ) + 2 \\mathrm { fe } \\left( \\mathrm { no } _ { 3 } \ ight) _ { 3 } ( a q ) } & { \
LATEXBLOCK1
} \\\\ { 3 \\mathrm { agno } _ { 3 } ( a q ) + \\mathrm { al } ( s ) \ ightarrow 3 \\mathrm { ag } ( s ) + \\mathrm { al } \\left( \\mathrm { no } _ { 3 } \ ight) _ { 3 } ( a q ) } & { \
LATEXBLOCK2
} \\\\ { } & { \
LATEXBLOCK3
} \\end{array}$$

Explanation:

Step1: Determine oxidation states

Oxidation state of \(Zn\) in \(Zn(s)\) is \(0\), in \(Zn(NO_3)_2\) is \(+2\). Oxidation state of \(Ag\) in \(AgNO_3\) is \(+1\), in \(Ag(s)\) is \(0\).

Step2: Identify oxidized and reduced reactants

Since \(Zn\) loses electrons (oxidation state increases), \(Zn\) is oxidized. \(Ag\) gains electrons (oxidation state decreases), \(AgNO_3\) is reduced.

Step3: For the second reaction

Oxidation state of \(Fe\) in \(Fe(s)\) is \(0\), in \(Fe(NO_3)_3\) is \(+3\). Oxidation state of \(Pb\) in \(Pb(NO_3)_2\) is \(+2\), in \(Pb(s)\) is \(0\). \(Fe\) is oxidized, \(Pb(NO_3)_2\) is reduced.

Step4: For the third reaction

Oxidation state of \(Al\) in \(Al(s)\) is \(0\), in \(Al(NO_3)_3\) is \(+3\). Oxidation state of \(Ag\) in \(AgNO_3\) is \(+1\), in \(Ag(s)\) is \(0\). \(Al\) is oxidized, \(AgNO_3\) is reduced.

Answer:

1. reactants oxidized: \(Zn\); reactants reduced: \(AgNO_3\)
2. reactants oxidized: \(Fe\); reactants reduced: \(Pb(NO_3)_2\)
3. reactants oxidized: \(Al\); reactants reduced: \(AgNO_3\)