General Chemistry

Organic Chemistry

To determine which of the given chemical reactions are oxidation-reduction (redox) reactions, we need to analyze the change in oxidation states of the elements involved in each reaction. A redox reaction involves the transfer of electrons between species, resulting in a change in oxidation states. ### Step 1: Understanding Oxidation States Oxidation states (or numbers) indicate the degree of oxidation of an atom in a compound. An increase in oxidation state through a reaction indicates oxidation (loss of electrons), while a decrease indicates reduction (gain of electrons). ### Step 2: Analyzing Each Reaction #### Reaction 1: $$\ce{2H2 + O2 -> 2H2O}$$ - **Hydrogen ($\ce{H}$)** in $\ce{H2}$ is $0$ (elemental form) and in $\ce{H2O}$ is $+1$. - **Oxygen ($\ce{O}$)** in $\ce{O2}$ is $0$ (elemental form) and in $\ce{H2O}$ is $-2$. **Changes:** - $\ce{H}$: $0 \to +1$ (oxidation) - $\ce{O}$: $0 \to -2$ (reduction) This is a redox reaction. #### Reaction 2: $$\ce{2Fe + 3Cl2 -> 2FeCl3}$$ - **Iron ($\ce{Fe}$)** in $\ce{Fe}$ is $0$ (elemental form) and in $\ce{FeCl3}$ is $+3$. - **Chlorine ($\ce{Cl}$)** in $\ce{Cl2}$ is $0$ (elemental form) and in $\ce{FeCl3}$ is $-1$. **Changes:** - $\ce{Fe}$: $0 \to +3$ (oxidation) - $\ce{Cl}$: $0 \to -1$ (reduction) This is a redox reaction. #### Reaction 3: $$\ce{2Na + Cl2 -> 2NaCl}$$ - **Sodium ($\ce{Na}$)** in $\ce{Na}$ is $0$ (elemental form) and in $\ce{NaCl}$ is $+1$. - **Chlorine ($\ce{Cl}$)** in $\ce{Cl2}$ is $0$ (elemental form) and in $\ce{NaCl}$ is $-1$. **Changes:** - $\ce{Na}$: $0 \to +1$ (oxidation) - $\ce{Cl}$: $0 \to -1$ (reduction) This is a redox reaction. #### Reaction 4: $$\ce{2H2O2 -> 2H2O + O2}$$ - **Oxygen ($\ce{O}$)** in $\ce{H2O2}$ is $-1$, in $\ce{H2O}$ is $-2$, and in $\ce{O2}$ is $0$. **Changes:** - $\ce{O}$ in $\ce{H2O2} \to \ce{H2O}$: $-1 \to -2$ (reduction) - $\ce{O}$ in $\ce{H2O2} \to \ce{O2}$: $-1 \to 0$ (oxidation) This is a redox reaction. #### Reaction 5: $$\ce{2H2S + 3O2 -> 2H2O + 2SO2}$$ - **Hydrogen ($\ce{H}$)** in $\ce{H2S}$ is $+1$ and in $\ce{H2O}$ is $+1$. - **Sulfur ($\ce{S}$)** in $\ce{H2S}$ is $-2$ and in $\ce{SO2}$ is $+4$. - **Oxygen ($\ce{O}$)** in $\ce{O2}$ is $0$ and in $\ce{H2O}$ and $\ce{SO2}$ is $-2$. **Changes:** - $\ce{S}$: $-2 \to +4$ (oxidation) - $\ce{O}$: $0 \to -2$ (reduction) This is a redox reaction. ### Conclusion All the reactions provided are redox reactions as they involve changes in oxidation states of the elements, indicating the transfer of electrons among them. Each reaction shows at least one element being oxidized and another being reduced.

Chemistry

Which of the following chemical reactions can be classified as an oxidation reduction reaction, based on the change in oxidation states of the elements involved:   $$\ce{2H2 + O2 -> 2H2O}$$ $$\ce{2Fe + 3Cl2 -> 2FeCl3}$$ $$\ce{2Na + Cl2 -> 2NaCl}$$  $$\ce{2H2O2 -> 2H2O + O2}$$  $$\ce{2H2S + 3O2 -> 2H2O + 2SO2}$$  $$\ce{2H2 + O2 -> 2H2O}$$

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Which of the following chemical reactions can be classified as an oxidation reduction reaction, base...
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Which of the following chemical reactions can be classified as an oxidation reduction reaction, base...Show More

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Which of the following chemical reactions can be classified as an oxidation reduction reaction, base...
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