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Questions and Answers
Which species acts as the reducing agent in the reaction: Cr2O7^2- + 14H^+ + 6Fe^2+ → 2Cr^3+ + 6Fe^3+ + 7H2O?
Which species acts as the reducing agent in the reaction: Cr2O7^2- + 14H^+ + 6Fe^2+ → 2Cr^3+ + 6Fe^3+ + 7H2O?
In the reaction MnO4^- + 8H^+ + 5e^- → Mn^2+ + 4H2O, what is the change in oxidation state of Mn?
In the reaction MnO4^- + 8H^+ + 5e^- → Mn^2+ + 4H2O, what is the change in oxidation state of Mn?
Which reaction is classified as a redox reaction?
Which reaction is classified as a redox reaction?
Which element gets oxidized in the reaction Zn + CuSO4 → ZnSO4 + Cu?
Which element gets oxidized in the reaction Zn + CuSO4 → ZnSO4 + Cu?
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What is the oxidation number of S in H2SO4?
What is the oxidation number of S in H2SO4?
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Which of the following reactions does not involve redox processes?
Which of the following reactions does not involve redox processes?
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Identify the oxidizing agent in the reaction: 2KMnO4 + 16HCl → 2KCl + 2MnCl2 + 5Cl2 + 8H2O.
Identify the oxidizing agent in the reaction: 2KMnO4 + 16HCl → 2KCl + 2MnCl2 + 5Cl2 + 8H2O.
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Which reaction represents a disproportionation process?
Which reaction represents a disproportionation process?
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What is the change in oxidation number of Fe in the reaction: 2FeCl3 + H2S → 2FeCl2 + 2HCl + S?
What is the change in oxidation number of Fe in the reaction: 2FeCl3 + H2S → 2FeCl2 + 2HCl + S?
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Flashcards
Oxidizing agent
Oxidizing agent
A substance that loses electrons and its oxidation number increases.
Reducing agent
Reducing agent
A substance that gains electrons and its oxidation number decreases.
Redox reaction
Redox reaction
A reaction involving the transfer of electrons, resulting in changes in oxidation numbers.
Reduction
Reduction
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Oxidation
Oxidation
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Oxidation number
Oxidation number
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Disproportionation reaction
Disproportionation reaction
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Oxidized species
Oxidized species
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Reduced species
Reduced species
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Oxidation-reduction reaction
Oxidation-reduction reaction
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Study Notes
Redox Reactions
- Reducing Agent in a Reaction: Fe2+ in the reaction Cr2O72- + 14H+ + 6Fe2+ → 2Cr3+ + 6Fe3+ + 7H2O
- Oxidation State Change in Mn: In MnO4- + 8H+ + 5e- → Mn2+ + 4H2O, the oxidation state of Mn changes from +7 to +2.
- Redox Reaction Identification: A redox reaction involves a change in oxidation states of elements (e.g., 2Na + Cl2 → 2NaCl).
- Oxidation Number of S in H2SO4: +6
- Non-Redox Reaction: CaCO3 → CaO + CO2 is not a redox reaction.
- Oxidizing Agent: KMnO4 in the reaction 2KMnO4 + 16HCI → 2KCl + 2MnCl2 + 5CI2 + 8H2O
- Oxidation Number of Cl in HClO4: +7
- Disproportionation Reaction: Cl2 + 2NaOH → NaCl + NaCIO + H2O is a disproportionation reaction.
- Oxidation Number Change in Fe: In 2FeCl3 + H2S → 2FeCl2 + 2HCI + S, the oxidation number of Fe changes from +3 to +2.
- Reducing Agent: H2S is a reducing agent.
- Oxidation Number of S in Na2S2O3: +2
- Reduced Element in CuO + H2 → Cu + H2O: Copper (Cu)
- Oxidation Number of Cr in K2Cr2O7: +6
- Characteristics of Redox Reactions: Redox reactions involve simultaneous oxidation and reduction, a change in oxidation number, and electron transfer; however, redox reactions are not always exothermic.
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Description
Test your knowledge on redox reactions, including identifying oxidizing and reducing agents, changes in oxidation states, and distinguishing between redox and non-redox reactions. This quiz covers fundamental concepts essential for understanding chemical reactions in a variety of contexts.
