What element is oxidized in the following equation and what element is reduced? $\mathrm { Sn } ^ { 2 + }$ + 2 Ag ? Sn + 2 Ag?
A)The tin ion, $\mathrm { Sn } ^ { 2 + }$ ,is oxidized,while the silver,Ag,is reduced.
B)The tin ion, $\mathrm { Sn } ^ { 2 + }$ ,is reduced,while the silver,Ag,is oxidized.
C)Both the tin ion, $\mathrm { Sn } ^ { 2 + }$ ,and the silver,Ag,are reduced.
D)Both the tin ion, $\mathrm { Sn } ^ { 2 + }$

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The Answer of What element is oxidized in the following equation and what element is reduced? $\mathrm { Sn } ^ { 2 + }$ + 2 Ag ? Sn + 2 Ag?
A)The tin ion, $\mathrm { Sn } ^ { 2 + }$ ,is oxidized,while the silver,Ag,is reduced.
B)The tin ion, $\mathrm { Sn } ^ { 2 + }$ ,is reduced,while the silver,Ag,is oxidized.
C)Both the tin ion, $\mathrm { Sn } ^ { 2 + }$ ,and the silver,Ag,are reduced.
D)Both the tin ion, $\mathrm { Sn } ^ { 2 + }$

What Element Is Oxidized in the Following Equation and What Sn2+\mathrm { Sn } ^ { 2 + }Sn2+

What Element Is Oxidized in the Following Equation and What $\mathrm { Sn } ^ { 2 + }$