Questions: Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. 7 O2(g) + 2 CH3CH3(g) → 4 CO2(g) + 6 H2O(g) redox reaction? yes no reducing agent: oxidizing agent: HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq) redox reaction? yes no reducing agent: oxidizing agent: CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) redox reaction? yes no reducing agent: oxidizing agent:

Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent.

7 O2(g) + 2 CH3CH3(g) → 4 CO2(g) + 6 H2O(g) redox reaction? yes no reducing agent: oxidizing agent:

HNO3(aq) + H2O(l) → H3O+(aq) + NO3-(aq) redox reaction? yes no reducing agent: oxidizing agent:

CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) redox reaction? yes no reducing agent: oxidizing agent:

Transcript text: Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the formula of the reducing agent and the formula of the oxidizing agent. $7 \mathrm{O}_{2}(\mathrm{~g})+2 \mathrm{CH}_{3} \mathrm{CH}_{3}(\mathrm{~g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{~g})+6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$ redox reaction? yes no reducing agent: oxidizing agent: $\mathrm{HNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{NO}_{3}^{-}(a q)$ redox reaction? yes no reducing agent: oxidizing agent: $\mathrm{CuSO}_{4}(a q)+\mathrm{Zn}(s) \rightarrow \mathrm{ZnSO}_{4}(a q)+\mathrm{Cu}(s)$ redox reaction? yes no reducing agent: oxidizing agent:

Solution

Solution Steps

Step 1: Determine if the first reaction is a redox reaction

The first reaction is: \[ 7 \mathrm{O}_{2}(\mathrm{~g}) + 2 \mathrm{CH}_{3} \mathrm{CH}_{3}(\mathrm{~g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{~g}) + 6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \]

To determine if this is a redox reaction, we need to check if there is a change in oxidation states of the elements involved.

Oxygen ($\mathrm{O}_2$) has an oxidation state of 0.
In $\mathrm{CO}_2$, oxygen has an oxidation state of -2, and carbon has an oxidation state of +4.
In $\mathrm{CH}_3\mathrm{CH}_3$, carbon has an oxidation state of -3 (for each hydrogen, +1).

Since the oxidation states of carbon and oxygen change, this is a redox reaction.

Step 2: Identify the reducing and oxidizing agents for the first reaction

The reducing agent is the substance that loses electrons (is oxidized). Here, $\mathrm{CH}_3\mathrm{CH}_3$ (ethane) is oxidized from -3 to +4.
The oxidizing agent is the substance that gains electrons (is reduced). Here, $\mathrm{O}_2$ is reduced from 0 to -2.

Step 3: Determine if the second reaction is a redox reaction

The second reaction is: \[ \mathrm{HNO}_{3}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q) + \mathrm{NO}_{3}^{-}(a q) \]

To determine if this is a redox reaction, we need to check if there is a change in oxidation states of the elements involved.

In $\mathrm{HNO}_3$, nitrogen has an oxidation state of +5.
In $\mathrm{NO}_3^-$, nitrogen still has an oxidation state of +5.

Since there is no change in the oxidation states of the elements, this is not a redox reaction.

Step 4: Determine if the third reaction is a redox reaction

The third reaction is: \[ \mathrm{CuSO}_{4}(a q) + \mathrm{Zn}(s) \rightarrow \mathrm{ZnSO}_{4}(a q) + \mathrm{Cu}(s) \]

To determine if this is a redox reaction, we need to check if there is a change in oxidation states of the elements involved.

In $\mathrm{CuSO}_4$, copper has an oxidation state of +2.
In $\mathrm{Zn}$, zinc has an oxidation state of 0.
In $\mathrm{ZnSO}_4$, zinc has an oxidation state of +2.
In $\mathrm{Cu}$, copper has an oxidation state of 0.

Since the oxidation states of copper and zinc change, this is a redox reaction.

Step 5: Identify the reducing and oxidizing agents for the third reaction

The reducing agent is the substance that loses electrons (is oxidized). Here, $\mathrm{Zn}$ is oxidized from 0 to +2.
The oxidizing agent is the substance that gains electrons (is reduced). Here, $\mathrm{Cu}^{2+}$ is reduced from +2 to 0.

Final Answer

For the reaction $ 7 \mathrm{O}_{2}(\mathrm{~g}) + 2 \mathrm{CH}_{3} \mathrm{CH}_{3}(\mathrm{~g}) \rightarrow 4 \mathrm{CO}_{2}(\mathrm{~g}) + 6 \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) $:
- Redox reaction: Yes
- Reducing agent: $\mathrm{CH}_3\mathrm{CH}_3$
- Oxidizing agent: $\mathrm{O}_2$ \[ \boxed{\text{Redox reaction: Yes, Reducing agent: } \mathrm{CH}_3\mathrm{CH}_3, \text{ Oxidizing agent: } \mathrm{O}_2} \]
For the reaction $ \mathrm{HNO}_{3}(a q) + \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(a q) + \mathrm{NO}_{3}^{-}(a q) $:
- Redox reaction: No \[ \boxed{\text{Redox reaction: No}} \]
For the reaction $ \mathrm{CuSO}_{4}(a q) + \mathrm{Zn}(s) \rightarrow \mathrm{ZnSO}_{4}(a q) + \mathrm{Cu}(s) $:
- Redox reaction: Yes
- Reducing agent: $\mathrm{Zn}$
- Oxidizing agent: $\mathrm{Cu}^{2+}$ \[ \boxed{\text{Redox reaction: Yes, Reducing agent: } \mathrm{Zn}, \text{ Oxidizing agent: } \mathrm{Cu}^{2+}} \]

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