Balancing Redox Reactions - Examples 1 & 2
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Balancing Redox Reactions - Examples 1 & 2

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Questions and Answers

Identify the oxidizing agent in the reaction between SO32- and MnO4-.

MnO4-

What is the final balanced equation for the reaction involving sulfite and permanganate ions?

5SO32- + 2MnO4- + 6H+ -> 5SO42- + 2Mn2+ + 3H2O

In acidic solutions, how are the oxygen atoms balanced in redox reactions?

Oxygen atoms are balanced using H2O molecules.

What is the purpose of including H+ ions in balancing redox reactions under acidic conditions?

<p>H<sup>+</sup> ions are used to balance hydrogen atoms in the half-reactions.</p> Signup and view all the answers

Identify the change in oxidation state for sulfur in the reaction from SO32- to SO42-.

<p>+4 to +6</p> Signup and view all the answers

How many electrons are involved in the oxidation of SO32- to SO42-?

<p>2 electrons</p> Signup and view all the answers

In the example involving cyanate, what is the oxidized form of CN-?

<p>OCN<sup>-</sup></p> Signup and view all the answers

What is the reduction reaction when MnO4- is involved?

<p>MnO<sub>4</sub><sup>-</sup> -&gt; MnO<sub>2</sub></p> Signup and view all the answers

Explain the importance of mass and charge balance in redox reactions.

<p>Mass and charge balance ensure the conservation of atoms and electrical charge in the reaction.</p> Signup and view all the answers

What role do intermediates like H2O play in balancing redox reactions?

<p>Intermediates like H<sub>2</sub>O help achieve equal numbers of oxygen and hydrogen atoms in half-reactions.</p> Signup and view all the answers

What is the role of H2O in balancing the oxygen atoms in the half-reaction of cyanate?

<p>H<sub>2</sub>O is added to balance the oxygen atoms by providing additional oxygen to the left side of the oxidation half-reaction.</p> Signup and view all the answers

How do you convert the acidic half-reaction of MnO4- into its basic form?

<p>Add H<sub>2</sub>O to both sides and OH<sup>-</sup> ions to the side with H<sup>+</sup> to neutralize the acid.</p> Signup and view all the answers

What do you need to do to balance the charge in the half-reactions?

<p>You introduce electrons (e<sup>-</sup>) to balance the charges on both sides of the oxidation and reduction half-reactions.</p> Signup and view all the answers

What is the significance of adding both H2O and OH- during the conversion from acidic to basic conditions?

<p>Adding H<sub>2</sub>O and OH<sup>-</sup> helps to maintain the balance of both atoms and charge in the reaction.</p> Signup and view all the answers

When balancing the final equation, what is meant by 'removing e-' from both sides?

<p>It means eliminating the electrons that were added for charge balance, simplifying the equation to its final stoichiometry.</p> Signup and view all the answers

How is the final balanced equation written, and what does it represent?

<p>The final equation is written as 2MnO<sub>4</sub><sup>-</sup> + 3CN<sup>-</sup> + H<sub>2</sub>O -&gt; 2MnO<sub>2</sub> + 3OCN<sup>-</sup> + 2OH<sup>-</sup>, representing the complete stoichiometry of the reaction under basic conditions.</p> Signup and view all the answers

What are the steps taken to balance the hydrogen atoms in both half-reactions?

<p>Hydrogen atoms are balanced by adding H<sup>+</sup> to the oxidation half-reaction and then converting it to OH<sup>-</sup> during the basic conversion.</p> Signup and view all the answers

In the verification process, what must you check regarding charge and atoms?

<p>You must verify that the charges balance on both sides (in this case, -5) and ensure that the number of each type of atom is equal on both sides.</p> Signup and view all the answers

Explain the function of the cyanate ion (OCN-) in the reduction step of the overall reaction.

<p>OCN<sup>-</sup> is formed as a product of the oxidation of cyanate and participates in the overall stoichiometry of the reaction.</p> Signup and view all the answers

The starting equation of the first example involves SO32- and ______.

<p>MnO<sub>4</sub><sup>-</sup></p> Signup and view all the answers

In the oxidation half-reaction, SO32- is transformed into ______.

<p>SO<sub>4</sub><sup>2-</sup></p> Signup and view all the answers

The reduction half-reaction involves the conversion of MnO4- to ______.

<p>Mn<sup>2+</sup></p> Signup and view all the answers

To balance oxygen atoms, ______ is added to the oxidation half-reaction.

<p>H<sub>2</sub>O</p> Signup and view all the answers

To balance hydrogen atoms, ______ ions are included in the reduction half-reaction.

<p>H<sup>+</sup></p> Signup and view all the answers

The final balanced equation includes 5SO32- and ______.

<p>2MnO<sub>4</sub><sup>-</sup></p> Signup and view all the answers

The skeletal equation for the reaction involving cyanate includes CN- and ______.

<p>MnO<sub>4</sub><sup>-</sup></p> Signup and view all the answers

When balancing redox reactions, it is important to verify both mass and ______ balance.

<p>charge</p> Signup and view all the answers

The ______ of sulfur changes during the reaction from SO32- to SO42-.

<p>oxidation state</p> Signup and view all the answers

In the example involving manganese, the reduction process results in ______ manganese oxide.

<p>MnO<sub>2</sub></p> Signup and view all the answers

In a redox reaction, the formula for cyanate is ______.

<p>OCN^-</p> Signup and view all the answers

To balance oxygen in the oxidation half-reaction, ______ is added.

<p>H2O</p> Signup and view all the answers

In the reduction half-reaction, ______ ions are used to balance hydrogen atoms.

<p>H+</p> Signup and view all the answers

When converting from acidic to basic conditions, ______ is added to each side of the equation.

<p>H2O</p> Signup and view all the answers

In a balanced chemical equation, the total charge should be ______ on both sides.

<p>equal</p> Signup and view all the answers

The final balanced equation shows 2MnO4^- reacting with 3CN^- and ______.

<p>H2O</p> Signup and view all the answers

In the oxidation half-reaction, 2e^- need to be ______ to balance the charge.

<p>removed</p> Signup and view all the answers

During the balancing process, 4OH^- is added to the reduction reaction involving ______.

<p>MnO4^-</p> Signup and view all the answers

The final equation must balance both the ______ and atoms on each side.

<p>charge</p> Signup and view all the answers

The oxidation of CN^- involves it being converted to ______.

<p>OCN^-</p> Signup and view all the answers

In the oxidation half-reaction, CN- is transformed into ______.

<p>OCN<sup>-</sup></p> Signup and view all the answers

To balance oxygen atoms in the oxidation half-reaction, ______ is added.

<p>H<sub>2</sub>O</p> Signup and view all the answers

The reduction half-reaction involves the conversion of MnO4- to ______.

<p>MnO<sub>2</sub></p> Signup and view all the answers

When converting from acidic to basic conditions, ______ is added to each side of the equation.

<p>H<sub>2</sub>O</p> Signup and view all the answers

In the final balanced equation, the total charge is ______ on both sides.

<p>-5</p> Signup and view all the answers

During the balancing process, 6e- are needed to balance the overall charge, which includes ______ from the oxidation half-reaction.

<p>3CN<sup>-</sup></p> Signup and view all the answers

The final balanced equation shows 2MnO4- reacting with 3CN- and ______.

<p>H<sub>2</sub>O</p> Signup and view all the answers

To balance hydrogen atoms in the reduction half-reaction, ______ ions are included.

<p>H<sup>+</sup></p> Signup and view all the answers

Each side of the final equation must balance both mass and ______.

<p>charge</p> Signup and view all the answers

In the oxidation reaction, CN- is oxidized to ______.

<p>OCN<sup>-</sup></p> Signup and view all the answers

The starting equation of the second example involves CN- and ______.

<p>MnO<sub>4</sub><sup>-</sup></p> Signup and view all the answers

In the oxidation half-reaction, SO32- is transformed into ______.

<p>SO<sub>4</sub><sup>2-</sup></p> Signup and view all the answers

The reduction half-reaction involves the conversion of MnO4- to ______.

<p>Mn<sup>2+</sup></p> Signup and view all the answers

To balance oxygen atoms, ______ is added to the oxidation half-reaction.

<p>H<sub>2</sub>O</p> Signup and view all the answers

To balance hydrogen atoms, ______ ions are included in the reduction half-reaction.

<p>H<sup>+</sup></p> Signup and view all the answers

The final balanced equation includes 5SO32- and ______.

<p>2Mn<sup>2+</sup></p> Signup and view all the answers

When balancing redox reactions, it is important to verify both mass and ______ balance.

<p>charge</p> Signup and view all the answers

The ______ of sulfur changes during the reaction from SO32- to SO42-.

<p>oxidation state</p> Signup and view all the answers

In a redox reaction, the formula for cyanate is ______.

<p>OCN<sup>-</sup></p> Signup and view all the answers

During the balancing process, 4OH- is added to the reduction reaction involving ______.

<p>MnO<sub>4</sub><sup>-</sup></p> Signup and view all the answers

Study Notes

Balancing Redox Reactions - Example 1

  • The reaction is between sulfite and permanganate in an acidic solution.
  • The redox reaction is: SO32- + MnO4- -> SO42- + Mn2+
  • The oxidation half reaction is: SO32- + H2O -> SO42- + 2H+ + 2e-
  • The reduction half reaction is: MnO4- + 8H+ + 5e- -> Mn2+ + 4H2O
  • The final balanced equation is: 5SO32- + 2MnO4- + 6H+ -> 5SO42- + 2Mn2+ + 3H2O
  • Both sides of the equation have the same number of atoms and charges.

Balancing Redox Reactions - Example 2

  • The reaction is between cyanide and permanganate in an aqueous basic solution.
  • The redox reaction is: CN- + MnO4- -> MnO2 + OCN-
  • The oxidation half reaction is: CN- + 2OH- -> OCN- + H2O + 2e-
  • The reduction half reaction is: MnO4- + 2H2O + 3e- -> MnO2 + 4OH-
  • The final balanced equation is: 2MnO4- + 3CN- + H2O -> 2MnO2 + 3OCN- + 2OH-
  • Both sides of the equation have the same number of atoms and charges.

Balancing Redox Reactions - Example 1

  • The initial equation is SO32- + MnO4- -> SO42- + Mn2+
  • Sulfite (SO32-) is oxidized to sulfate (SO42-).
  • Permanganate (MnO4-) is reduced to Mn2+.
  • The redox reaction is balanced in acidic solution.
  • The final balanced equation is: 5SO32- + 2MnO4- + 6H+ -> 5SO42- + 2Mn2+ + 3H2O
  • The equation is balanced with 5 sulfur atoms, 2 manganese atoms, 23 oxygen atoms, and 6 hydrogen atoms on each side.
  • The equation also has a charge balance of -6 on each side.

Balancing Redox Reactions - Example 2

  • The initial equation is CN- + MnO4- -> MnO2 + OCN-.
  • Cyanide (CN-) is oxidized to cyanate (OCN-).
  • Permanganate (MnO4-) is reduced to manganese dioxide (MnO2).
  • The redox reaction is balanced in basic solution.
  • The final balanced equation is: 2MnO4- + 3CN- + H2O -> 2MnO2 + 3OCN- + 2OH-
  • The equation is balanced with 2 manganese atoms, 3 carbon atoms, 3 nitrogen atoms, 9 oxygen atoms, and 2 hydrogen atoms on each side.
  • The equation also has a charge balance of -5 on each side.

Balancing Redox Reactions - Example 1

  • Sulfite (SO32-) is oxidized to sulfate (SO42-)
  • Permanganate (MnO4-) is reduced to manganese(II) (Mn2+)
  • The oxidation half-reaction occurs in acidic solution
  • Oxygen is balanced by adding H2O to the products side for the oxidation reaction and reactants side for the reduction reaction
  • Hydrogen is balanced by adding H+ to the reactants side of the oxidation reaction and the products side of the reduction reaction.
  • Electrons are balanced by adding 2e- to the products side of the oxidation reaction and 5e- to the reactants side of the reduction reaction.
  • The oxidation half-reaction is multiplied by 5 and the reduction half-reaction is multiplied by 2 to ensure the number of electrons gained and lost are equal.
  • The resulting balanced redox reaction is: 5SO32- + 2MnO4- + 6H+ -> 5SO42- + 2Mn2+ + 3H2O
  • The final equation is verified by ensuring mass balance and charge balance.

Balancing Redox Reactions - Example 2

  • Cyanide (CN-) is oxidized to cyanate (OCN-)
  • Permanganate (MnO4-) is reduced to Manganese(IV) oxide (MnO2)
  • The redox reaction occurs in basic solution
  • Oxygen is balanced by adding H2O to the products side of the oxidation reaction and reactants side of the reduction reaction
  • Hydrogen is balanced by adding H+ to the reactants side of the oxidation reaction and the products side of the reduction reaction.
  • The acidic solution is then converted into basic solution by adding sufficient H2O to both sides of the equation.
  • For each H+ added, OH- is added to the same side of the equation.
  • H2O is added to the opposite side of the equation.
  • Electrons are balanced by adding 2e- to the products side of the oxidation reaction and 3e- to the reactants side of the reduction reaction.
  • The oxidation half-reaction is multiplied by 3 and the reduction half-reaction is multiplied by 2 to ensure the number of electrons gained and lost are equal.
  • The resulting balanced redox reaction is: 2MnO4- + 3CN- + H2O -> 2MnO2 + 3OCN- + 2OH-
  • The final equation is verified by ensuring mass balance and charge balance.

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PF1009 2024 12A Balancing Redox Equations PDF

Description

This quiz provides examples of balancing redox reactions, including reactions between sulfite and permanganate in acidic conditions and cyanide with permanganate in basic conditions. Participants will learn to identify oxidation and reduction half-reactions and achieve balanced equations for each scenario.

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