write a balanced overall reaction from these unbalanced half reactions cu cu2 ag ag
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Question “write a balanced overall reaction from these unbalanced half reactions cu cu2 ag ag”
Write a balanced overall reaction from these unbalanced half-reactions. Cu rightarrow cu2+ Ag+ rightarrow Ag balanced overall reaction: For a particular redox reaction NO is oxidized to and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional. NO+ Ag+ rightarrow + Ag Balance the following equation in basic conditions. Phases are optional. CoCI2 + Na2O2 rightarrow Co(OH)3+C1-+ Na+
Write a balanced overall reaction from these unbalanced half-reactions. Cu rightarrow cu2+ Ag+ rightarrow Ag balanced overall reaction: For a particular redox reaction NO is oxidized to and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional. NO+ Ag+ rightarrow + Ag Balance the following equation in basic conditions. Phases are optional. CoCI2 + Na2O2 rightarrow Co(OH)3+C1-+ Na+
Answer
General guidance
Concepts and Reason
Half-reaction can balance a redox reaction. Below are the steps required to balance a chemical reaction for a redox (in a basic solution).
1. Identify the species under oxidation or reduction. Separate the reactions into oxidation/half reaction and reduction/half reaction.
2Balance all atoms, except hydrogen and oxygen.
3 Add protons to balance hydrogens
4 Add electrons to balance charge as follows:
5 Scale half-reactions so that the number of electrons in each half-reaction is equal.
6 Cancel the electrons after the addition of the two reactions.
7.Add {\\rm{O}}{{\\rm{H}}^ - }
8.Combine {{\\rm{H}}^ + }
Fundamentals
The law of conservation is that matter cannot be created or destroyed. The number of atoms on each side must be equal.
Step-by-step
Step 1 from 3
Part 1
As follows:
The overall balanced reaction is:
Part 1
Below is the overall reaction:
Common mistakes
The following redox reaction can be balanced:
1.Recite the half-reactions like this
2. Copper’s oxidation state increases from 0 up to $math_tag_2
3.Balance electrons in equations by multiplying half-reaction silver by two as follows:
Add the two reactions as follows:
5. To achieve the balanced redox reaction:
Balance Ag atoms on both sides of equation.
Identify the species that is reduced or oxidized by the given redox reaction.
Step 2 from 3
Part 2
Below is the overall balanced reaction:
Part 2
Below is the overall balanced equation:
Common mistakes
You can balance the given redox reaction using half-reaction as follows:
1. Write the following redox reaction:
2.Nitrogen from NO is oxidized starting at + 2
3.All atoms, except oxygen, are equal; add {{\\rm{H}}_{\\rm{2}}}{\\rm{O}}
4 Add protons to balance hydrogens
5 Add electrons to balance charge as follows:
6. Multiply the silver-reaction half-reaction by three to equal the number of electrons in the two half-reactions.
7. Cancel the electrons after the addition of the two reactions.
8.Add {\\rm{O}}{{\\rm{H}}^ - }
9.Combine {{\\rm{H}}^ + }
Balance without adding {\\rm{O}}{{\\rm{H}}^ - }
Identify the species that is reduced or oxidized by the given redox reaction.
You can balance the given redox reaction using half-reaction as follows:
1. Write the following redox reaction:
2.Cobalt has been oxidized and oxygen has been reduced by the given redox reactions. {\\rm{C}}{{\\rm{l}}^ - }{\\rm{C}}{{\\rm{o}}^{2 + }} + {\\rm{O}}_2^{2 - } \\to {\\rm{C}}{{\\rm{o}}^{3 + }} + {\\rm{3O}}{{\\rm{H}}^ - }
3.Separate redox reaction into half-reactions, as follows:
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