for each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. write the chemical formulae of any reactants that will be reduced in the third column. reaction reactants oxidized reactants reduced $\ce{pb(s) + 2cl_{2}(g) - pbcl_{4}(s)}$ $\ce{o_{2}(g) + cr(s) - cro_{2}(s)}$ $\ce{8mg(s) + s_{8}(s) - 8mgs(s)}$

Question

for each reaction in the table below, write the chemical formulae of any reactants that will be oxidized in the second column of the table. write the chemical formulae of any reactants that will be reduced in the third column. reaction reactants oxidized reactants reduced $\ce{pb(s) + 2cl_{2}(g) -> pbcl_{4}(s)}$ $\ce{o_{2}(g) + cr(s) -> cro_{2}(s)}$ $\ce{8mg(s) + s_{8}(s) -> 8mgs(s)}$

Accepted Answer

# Explanation:
## Step1: Determine oxidation states
- For $Pb(s)+2Cl_{2}(g)\to PbCl_{4}(s)$:
    - Oxidation state of $Pb$ in $Pb(s)$ is $0$, in $PbCl_{4}$ is $+4$ (since $Cl$ is $- 1$ and $x + 4\times(-1)=0$ gives $x = + 4$).
    - Oxidation state of $Cl$ in $Cl_{2}(g)$ is $0$, in $PbCl_{4}$ is $-1$.
    - $Pb$ is oxidized (loses electrons, oxidation state increases), $Cl_{2}$ is reduced (gains electrons, oxidation state decreases).
## Step2: For $O_{2}(g)+Cr(s)\to CrO_{2}(s)$:
    - Oxidation state of $Cr$ in $Cr(s)$ is $0$, in $CrO_{2}$ is $+4$ (since $x+2\times(-2) = 0$ gives $x=+4$).
    - Oxidation state of $O$ in $O_{2}(g)$ is $0$, in $CrO_{2}$ is $-2$.
    - $Cr$ is oxidized, $O_{2}$ is reduced.
## Step3: For $8Mg(s)+S_{8}(s)\to8MgS(s)$:
    - Oxidation state of $Mg$ in $Mg(s)$ is $0$, in $MgS$ is $+2$ (since $x+(-2)=0$ gives $x = + 2$).
    - Oxidation state of $S$ in $S_{8}(s)$ is $0$, in $MgS$ is $-2$.
    - $Mg$ is oxidized, $S_{8}$ is reduced.

# Answer:
| reaction | reactants oxidized | reactants reduced |
|--|--|--|
| $Pb(s)+2Cl_{2}(g)\to PbCl_{4}(s)$ | $Pb$ | $Cl_{2}$ |
| $O_{2}(g)+Cr(s)\to CrO_{2}(s)$ | $Cr$ | $O_{2}$ |
| $8Mg(s)+S_{8}(s)\to8MgS(s)$ | $Mg$ | $S_{8}$ |

reaction	reactants oxidized	reactants reduced
\(O_{2}(g)+Cr(s)\to CrO_{2}(s)\)	\(Cr\)	\(O_{2}\)
\(8Mg(s)+S_{8}(s)\to8MgS(s)\)	\(Mg\)	\(S_{8}\)

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QUESTION IMAGE

Question

Explanation:

Step1: Determine oxidation states

Step2: For \(O_{2}(g)+Cr(s)\to CrO_{2}(s)\):

Step3: For \(8Mg(s)+S_{8}(s)\to8MgS(s)\):

Answer: