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Questions and Answers
The cyanate ion is represented as ______.
OCN-
In balancing redox reactions, one must balance oxygen with ______.
H2O
To balance hydrogen, we use ______.
H+
In basic conditions, H+ ions are converted by adding ______.
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The balanced oxidation half-reaction involves ______ and hydroxide ions.
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The redox equation involves the reduction of ______ ions.
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The final equation presents a balance of ______ and hydrogen.
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To achieve charge balance, the half-reactions require the addition of ______.
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The final balanced equation includes ______ molecules.
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Charge balance in the overall reaction results in a total charge of ______ on both sides.
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The starting equation for the first example is SO32- + MnO4- -> SO42- + Mn______
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In an acidic solution, the oxidation process of SO32- involves the formation of SO4______
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To balance the reaction for the oxidation of SO32-, water is added to the left side in order to balance the ______
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In the reduction half-reaction, MnO4- is reduced to Mn______
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In total for the redox equation, 16H______ was added to balance the hydrogens.
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The final balanced equation includes 5 molecules of SO32-, 2 molecules of MnO4-, and 6H______.
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Cyanate is represented by the formula CN______ in the second example.
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In the second example, the oxidation process involves CN______ being converted to OCN-.
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The redox equations from the second example show that MnO4- is reduced to ______.
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After balancing, the number of sulfur atoms on both sides of the equation remains ______.
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Study Notes
Balancing Redox Reactions
- Sulfite (SO32-) is oxidized to sulfate (SO42-)
- Permanganate (MnO4-) is reduced to Manganese (II) (Mn2+)
- The redox reaction occurs in acidic conditions
- To balance the oxygen atoms in the half-reactions, H2O is added
- Hydrogen atoms are balanced by adding H+
- To balance the charge in each half reactions, electrons are added
- The electrons are cancelled out from the half-reactions by multiplying each half-reaction by a suitable factor
- Mass balance: 5xS, 2xMn, 23xO, 6xH
- Charge balance: -6 on both sides of the equation
Balancing Redox Reactions - Example 2
- Cyanate (CN-) is oxidized to cyanate (OCN-)
- Permanganate (MnO4-) is reduced to manganese dioxide (MnO2)
- The redox reaction takes place in an aqueous base
- To balance the hydrogen atoms, H+ is added to each side
- The acidic reaction is converted to basic by adding OH- to the same side as the H+ ions, and H2O to the opposite side
- Charges are balanced by adding electrons to each side of the equation
- After balancing charges, multiply by an appropriate factor to remove electrons from the equations
- Mass balance: 2xMn, 3xC, 3xN, 9xO, 2xH
- Charge balance: -5 on each side of the equation
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Description
Test your understanding of balancing redox reactions in both acidic and basic conditions. This quiz covers the oxidation of sulfite to sulfate and the reduction of permanganate, alongside practical examples involving cyanate. Challenge yourself with half-reaction procedures and charge balancing.
