decide whether each chemical reaction in the table below is an oxidation - reduction (
edox\) reaction. if the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent.

\begin{array} { l | l | l } & ext { redox reaction? } & \ mathrm { cuso } _ { 4 } ( a q ) + mathrm { zn } ( s )
ightarrow mathrm { znso } _ { 4 } ( a q ) + mathrm { cu } ( s ) & \begin{array} { l } { \bigcirc ext { yes } } \ { ext { reducing } } end{array} & \bigcirc ext { no } \ & ext { agent: } & \ & ext { oxidizing } & \ & ext { agent: } & \ & ext { redox reaction? } & \ mathrm { hcl } ( a q ) + mathrm { nh } _ { 3 } ( a q )
ightarrow mathrm { nh } _ { 4 } mathrm { cl } ( a q ) & \begin{array} { l } { \bigcirc ext { yes } } \ { ext { reducing } } end{array} & \bigcirc ext { no } \ & ext { agent: } & \ & ext { oxidizing } & \ & ext { agent: } & \ & ext { redox reaction? } & \ mathrm { co } ( g ) + mathrm { h } _ { 2 } mathrm { o } ( g )
ightarrow mathrm { co } _ { 2 } ( g ) + mathrm { h } _ { 2 } ( g ) & \begin{array} { l } { \bigcirc ext { yes } } \ { ext { reducing } } end{array} & \bigcirc ext { no } \ & ext { agent: } & \ & ext { oxidizing } & \ & ext { agent: } & end{array}

Question

decide whether each chemical reaction in the table below is an oxidation - reduction (
edox\) reaction. if the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent.

\begin{array} { l | l | l } & 	ext { redox reaction? } & \ mathrm { cuso } _ { 4 } ( a q ) + mathrm { zn } ( s )
ightarrow mathrm { znso } _ { 4 } ( a q ) + mathrm { cu } ( s ) & \begin{array} { l } { \bigcirc 	ext { yes } } \ { 	ext { reducing } } end{array} & \bigcirc 	ext { no } \ & 	ext { agent: } & \ & 	ext { oxidizing } & \ & 	ext { agent: } & \ & 	ext { redox reaction? } & \ mathrm { hcl } ( a q ) + mathrm { nh } _ { 3 } ( a q )
ightarrow mathrm { nh } _ { 4 } mathrm { cl } ( a q ) & \begin{array} { l } { \bigcirc 	ext { yes } } \ { 	ext { reducing } } end{array} & \bigcirc 	ext { no } \ & 	ext { agent: } & \ & 	ext { oxidizing } & \ & 	ext { agent: } & \ & 	ext { redox reaction? } & \ mathrm { co } ( g ) + mathrm { h } _ { 2 } mathrm { o } ( g )
ightarrow mathrm { co } _ { 2 } ( g ) + mathrm { h } _ { 2 } ( g ) & \begin{array} { l } { \bigcirc 	ext { yes } } \ { 	ext { reducing } } end{array} & \bigcirc 	ext { no } \ & 	ext { agent: } & \ & 	ext { oxidizing } & \ & 	ext { agent: } & end{array}

Accepted Answer

# Explanation:
## Step1: Analyze the first reaction $CuSO_{4}(aq)+Zn(s)\to ZnSO_{4}(aq)+Cu(s)$
- For $Zn$: $Zn$ goes from $0$ (in $Zn(s)$) to $+ 2$ (in $ZnSO_{4}$). It is oxidized. So $Zn$ is the reducing agent.
- For $Cu$: $Cu$ goes from $+2$ (in $CuSO_{4}$) to $0$ (in $Cu(s)$). It is reduced. So $CuSO_{4}$ is the oxidizing agent. This is a redox reaction.
## Step2: Analyze the second reaction $HCl(aq)+NH_{3}(aq)\to NH_{4}Cl(aq)$
- Check oxidation states:
    - In $HCl$, $H = + 1$, $Cl=-1$; in $NH_{3}$, $N=-3$, $H = + 1$; in $NH_{4}Cl$, $N=-3$, $H = + 1$, $Cl=-1$. No change in oxidation states. So it is not a redox reaction.
## Step3: Analyze the third reaction $CO(g)+H_{2}O(g)\to CO_{2}(g)+H_{2}(g)$
- For $C$: $C$ goes from $+2$ (in $CO$) to $+4$ (in $CO_{2}$). It is oxidized. So $CO$ is the reducing agent.
- For $H$: $H$ goes from $+1$ (in $H_{2}O$) to $0$ (in $H_{2}$). It is reduced. So $H_{2}O$ is the oxidizing agent. This is a redox reaction.

# Answer:
- For $CuSO_{4}(aq)+Zn(s)\to ZnSO_{4}(aq)+Cu(s)$: redox reaction? yes; reducing agent: $Zn$; oxidizing agent: $CuSO_{4}$
- For $HCl(aq)+NH_{3}(aq)\to NH_{4}Cl(aq)$: redox reaction? no
- For $CO(g)+H_{2}O(g)\to CO_{2}(g)+H_{2}(g)$: redox reaction? yes; reducing agent: $CO$; oxidizing agent: $H_{2}O$

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Step1: Analyze the first reaction \(CuSO_{4}(aq)+Zn(s)\to ZnSO_{4}(aq)+Cu(s)\)

Step2: Analyze the second reaction \(HCl(aq)+NH_{3}(aq)\to NH_{4}Cl(aq)\)

Step3: Analyze the third reaction \(CO(g)+H_{2}O(g)\to CO_{2}(g)+H_{2}(g)\)

Answer: