Redox Reaction Identified for an Atom

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In each of the following reactions, identify the atom oxidized, the atom reduced, and balance the equation.

1. KBr + Fe2(SO4)3 -> Br2 + K2SO4 + FeSO4

2. Sn + HNO3 + H2O -> H2SnO3 + NO

3. Cu + AgNO3 -> Ag + Cu(NO3)2

Calculate the cell potential for each of the following reactions and determine whether the reaction is spontaneous.

4. Cr+3 + 3Na -> Cr +3Na+

5. Mn+2 + Cd -> Mn + Cd+2

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In each of the following reactions, identify the atom oxidized, the atom reduced, and balance the equation.

1. KBr + Fe2(SO4)3 -> Br2 + K2SO4 + FeSO4
Here Br- loses an electron to form molecular Bromine. Hence it is getting oxidized.
Fe is gaining an electron since the ionic charge changes from Fe3+ to Fe2+. Hence Fe is getting reduced.
The balanced equation is as below:
2KBr + Fe2(SO4)3 -> Br2 + K2SO4 + 2FeSO4

2. Sn + HNO3 + H2O -> H2SnO3 + NO
Oxidation Number of Sn in H2SnO3: 3*2 - 2*1 = 4
Sn is getting oxidized since its ON is increasing from 0 to +4.
Oxidation Number of N in HNO3: 3*2 - 1 = 5
Oxidation Number of N in NO = 2
HNO3 is getting ...

Solution Summary

The expert examines redox reactions to identify atoms. The cell potentials for each reaction is calculated.

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Balancing Redox Reactions

For the two unbalanced equation below

-Write the unbalanced half-reactions.
-Identify the species oxidized and the species reduced.
-Identify the oxidizing agent and the reducing agent.
-Balance the equation in acid.
-Balance the equation in base.

(a)H2O2(aq)+Ni^2+(aq) --> Ni^3+(aq) + H2O

(b)Cr2o7^2-(aq) +Sn^2+(aq) --> Cr^3+(aq) + Sn^4+(aq)

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