Podcast Beta
Questions and Answers
What is the reduced form of manganese in the given reaction?
In the balancing process, how is oxygen represented?
What is the final coefficient of water (H2O) in the completed balanced equation?
What is the charge on MnO4 in the reaction?
Signup and view all the answers
What is the net change in oxidation state for carbon in the conversion from CN- to OCN-?
Signup and view all the answers
How many electrons are involved in the oxidation half-reaction of CN-?
Signup and view all the answers
What happens to H+ when converting an acidic equation to a basic one in this process?
Signup and view all the answers
What is the final balanced form of the reduction half-equation?
Signup and view all the answers
Which of the following elements is being oxidized in the final equation?
Signup and view all the answers
How is charge balanced in the overall reaction?
Signup and view all the answers
In the redox reaction involving SO32- and MnO4-, what is the oxidation state of manganese in the product Mn2+?
Signup and view all the answers
What is the purpose of adding H2O in the oxidation half-reaction?
Signup and view all the answers
In balancing redox reactions in acidic solutions, what is generally added to balance the hydrogen ions?
Signup and view all the answers
What is the final balanced equation for the first example of the redox reaction provided?
Signup and view all the answers
Which species is oxidized in the reaction involving cyanate and permanganate?
Signup and view all the answers
What type of solution are the redox reactions provided performed in?
Signup and view all the answers
During the oxidation of SO32-, how many electrons are lost?
Signup and view all the answers
How many moles of water are produced in the final balanced equation for the first redox reaction?
Signup and view all the answers
What is the charge on the sulfate ion produced in the oxidation of SO32-?
Signup and view all the answers
Study Notes
Balancing Redox Reactions
- The redox reaction of sulfite (SO32-) with permanganate (MnO4-) in acidic solution produces sulfate (SO42-) and manganese (II) ions (Mn2+).
- Redox reactions can be balanced by separating them into oxidation (OX) and reduction (Red) half-reactions.
- To balance redox reactions, follow these steps:
- Balance metals or elements other than O and H.
- Balance oxygen by adding H2O to the appropriate side.
- Balance hydrogen by adding H+ to the appropriate side.
- Balance charges by adding electrons (e-) to the appropriate side.
- Multiply the half-reactions by appropriate factors to make the number of electrons equal in both equations.
- Combine the half-reactions and cancel out the same components on opposite sides.
- In basic solutions, convert acidic solutions by adding OH- and H2O to balance charges and H+ ions.
-
Example 1
- The final balanced equation is: 5SO32- + 2MnO4- + 6H+ -> 5SO42- + 2Mn2+ + 3H2O
- Verify the equation by checking the atom and charge balance on both sides.
-
Example 2
- The oxidation of cyanide (CN-) with permanganate (MnO4-) in basic solution produces cyanate (OCN-) and manganese (IV) oxide (MnO2).
- The final balanced equation is: 2MnO4- + 3CN- + H2O -> 2MnO2 + 3OCN- + 2OH-
- Again, verify the equation by checking the atom and charge balance on both sides.
Studying That Suits You
Use AI to generate personalized quizzes and flashcards to suit your learning preferences.
Related Documents
Description
This quiz focuses on the steps to balance redox reactions, specifically using the reaction of sulfite and permanganate in acidic solutions. Participants will learn how to separate these reactions into oxidation and reduction half-reactions and apply systematic steps to balance them effectively.
