Redox Reactions Quiz

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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?

  • H^+
  • Cr^3+
  • Cr2O7^2-
  • Fe^2+ (correct)

In the reaction MnO4^- + 8H^+ + 5e^- → Mn^2+ + 4H2O, what is the change in oxidation state of Mn?

  • +7 to +2 (correct)
  • +4 to +2
  • +2 to +4
  • +2 to +7

Which reaction is classified as a redox reaction?

  • 2Na + Cl2 → 2NaCl (correct)
  • NaCl + AgNO3 → AgCl + NaNO3
  • NH4Cl → NH3 + HCl
  • CaCO3 → CaO + CO2

Which element gets oxidized in the reaction Zn + CuSO4 → ZnSO4 + Cu?

<p>Zn (D)</p> Signup and view all the answers

What is the oxidation number of S in H2SO4?

<p>+6 (A)</p> Signup and view all the answers

Which of the following reactions does not involve redox processes?

<p>CaCO3 → CaO + CO2 (C)</p> Signup and view all the answers

Identify the oxidizing agent in the reaction: 2KMnO4 + 16HCl → 2KCl + 2MnCl2 + 5Cl2 + 8H2O.

<p>KMnO4 (B)</p> Signup and view all the answers

Which reaction represents a disproportionation process?

<p>Cl2 + 2NaOH → NaCl + NaClO + H2O (A)</p> Signup and view all the answers

What is the change in oxidation number of Fe in the reaction: 2FeCl3 + H2S → 2FeCl2 + 2HCl + S?

<p>+3 to +2 (A)</p> Signup and view all the answers

Flashcards

Oxidizing agent

A substance that loses electrons and its oxidation number increases.

Reducing agent

A substance that gains electrons and its oxidation number decreases.

Redox reaction

A reaction involving the transfer of electrons, resulting in changes in oxidation numbers.

Reduction

A process in which an atom or ion gains electrons, leading to a decrease in its oxidation number.

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Oxidation

A process in which an atom or ion loses electrons, leading to an increase in its oxidation number.

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Oxidation number

The number assigned to an element in a compound that reflects the number of electrons it has gained or lost.

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Disproportionation reaction

A reaction where a single element undergoes both oxidation and reduction.

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Oxidized species

A substance that gains electrons and is reduced in a reaction.

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Reduced species

A substance that loses electrons and is oxidized in a reaction.

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Oxidation-reduction reaction

A reaction where the oxidation numbers of atoms change.

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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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