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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