Use line notation to represent the electrochemical cells for the following UNBALANCED redox EQUATION. Part A NO−3(aq)+Cu(s)→NO(g)+Cu2+(aq) N O 3 − ( a q ) + C u ( s ) → N O ( g ) + C u 2 + ( a q ) Cu2+(aq)|Cu(s)||NO(g)|NO−3(aq),H+ (aq),H2O(l)|Pt(s) C u 2 + ( a q ) | C u ( s ) | | N O ( g ) | N O 3 − ( a q ) , H + ( a q ) , H 2 O ( l ) | P t ( s ) Pt(s)|NO−3(aq),H+(aq),H2O(l)|NO(g)||Cu(s)|Cu2+(aq) P t ( s ) | N O 3 − ( a q ) , H + ( a q ) , H 2 O ( l ) | N O ( g ) | | C u ( s ) | C u 2 + ( a q ) Cu(s)|Cu2+(aq)||NO−3(aq),H+(aq),H2O(l)|NO(g)|Pt(s) C u ( s ) | C u 2 + ( a q ) | | N O 3 − ( a q ) , H + ( a q ) , H 2 O ( l ) | N O ( g ) | P t ( s ) Pt(s)|NO(g)|NO−3(aq),H+(aq),H2O(l)||Cu2+(aq)|Cu(s) P t ( s ) | N O ( g ) | N O 3 − ( a q ) , H + ( a q ) , H 2 O ( l ) | | C u 2 + ( a q ) | C u ( s ) SubmitRequest Answer Part B What is the cell reaction? 2NO(g)+4H2O(l)+3Cu2+(aq)+Pt(s)→2NO−3(aq)+8H+(aq)+3Cu(s) 2 N O ( g ) + 4 H 2 O ( l ) + 3 C u 2 + ( a q ) + P t ( s ) → 2 N O 3 − ( a q ) + 8 H + ( a q ) + 3 C u ( s ) 2NO−3(aq)+8H+(aq)+3Cu(s)→2NO(g)+4H2O(l)+3Cu2+(aq) 2 N O 3 − ( a q ) + 8 H + ( a q ) + 3 C u ( s ) → 2 N O ( g ) + 4 H 2 O ( l ) + 3 C u 2 + ( a q ) 2NO−3(aq)+8H+(aq)+3Cu(s)+Pt(s)→2NO(g)+4H2O(l)+3Cu2+(aq) 2 N O 3 − ( a q ) + 8 H + ( a q ) + 3 C u ( s ) + P t ( s ) → 2 N O ( g ) + 4 H 2 O ( l ) + 3 C u 2 + ( a q ) 2NO(g)+4H2O(l)+3Cu2+(aq)→2NO−3(aq)+8H+(aq)+3Cu(s) 2 N O ( g ) + 4 H 2 O ( l ) + 3 C u 2 + ( a q ) → 2 N O 3 − ( a q ) + 8 H + ( a q ) + 3 C u ( s ) SubmitRequest Answer