Given the following notation for an electrochemical cell Pt(s) | Sn²+(aq), Sn 4+ (aq) || Cl2(g) | Cl¯¯(aq) | Pt(s) what is the balanced overall (net) cell reaction? Pt(s) + Cl2(g) + Sn²+(aq) = Sn 4+ (aq) + Cl¯(aq) + Pt(s) Sn 4+ (aq) + 2 Cl¯(aq) ⇒ Cl2(g) + Sn²+(aq) Pt(s) + Sn4+(aq) + 2 Cl¯(aq) ⇒ Cl2(g) + Sn²+(aq) + Pt(s) Pt(s) + Sn 4+ (aq) + Cl¯(aq) Cl2(g) + Sn²+(aq) + Pt(s) Cl2(g) + Sn2+(aq) Sn 4+ (aq) + 2 Cl¯(aq)

What is the balanced chemical equation for this galvanic cell reaction? Cr(s) | Cr3*(aq), 1M || CI- (aq), 1 M| Cl2(1), 1 atm | Pt(s)

Write the overall cell reaction for the galvanic cell given below. Pt(s) | Sn2+(aq), Sn4+(aq) || Fe3+(aq) | Fe(s)

Cr(s) | Cr^3+(aq) || VO2+(aq), H+(aq), VO^2+(aq) | Pt(s)   Calculate the equilibrium constant associated with this cell under standard conditions

What is the cell reaction for the following voltaic cell? AI(s) | AI³*(aq) || Br"(aq) | Br2(g) | Pt(s) O A(s) + Al3* (aq) → Br (aq) + Br2(g) O AI(s) + 2 Br (aq) → Br2(g) + A13+(aq) O 2 AI(s) + 3 Br2(g) → 2 Al3+ (aq) + 6 Br (aq) O 2 A13* (aq) + 6 Br¯(aq) → 2 AI(s) + 3 Br2(g) O Al(s) + 3 Br2(g) → Al3+(s) + 2 Br (aq)

[Fe3+]= 2.0×10−3 M; [Mg2+]= 3.15 M   Express your answer in units of volts.

3.2 calculate the standard cell potential of the following cell at 250 Sn(s)|Sn*(aq)||Cu*(aq)|Cu(s) 2+ 2+

In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s)

Give the standard line notation for each cell. (a) 2 IO3(aq) + 10 Fe²+ (aq) + 10 H+ (aq) 10 Fe³+ (aq) + I₂ (aq) + 5 H₂O(1) Pt(s) | Fe³+ (aq), I₂ (aq) || Fe²+ (aq), IO3¯(aq), H+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), Fe³+ (aq) || IO3(aq), H+ (aq), I₂ (aq) | Pt(s) Pt(s) | IO3(aq), H+ (aq), I₂ (aq) || Fe²+ (aq), Fe³+ (aq) | Pt(s) Pt(s) | Fe²+ (aq), IO3¯¯(aq), H+ (aq) || Fe³+ (aq), I₂ (aq) | Pt(s) (b) (c) (d) Zn(s) + 2 Ag+ (aq) = Zn²+ (aq) + 2 Ag(s) Ag(s) | Zn²+ (aq) || Ag+ (aq) | Zn(s) Zn(s) | Zn²+ (aq) || Ag+ (aq) | Ag(s) Ag(s) | Ag+ (aq) || Zn²+ (aq) | Zn(s) Zn(s) | Ag+ (aq) || Zn²+ (aq) | Ag(s) H₂O₂ (aq) + 2 H+ (aq) + 2e → 2 H₂O(l) O2(g) + 2 H+ (aq) + 2 e¯ → H₂O₂ (aq) Pt(s) | H₂O₂ (aq) | Pt(s) ○ Pt(s) | O₂(g) | H₂O₂ (aq), H+ (aq) || H₂O₂ (aq), H+ (aq) | Pt(s) Pt(s) | H₂O₂ (aq), H+ (aq) || O₂(g) | H₂O₂ (aq), H+ (aq) | Pt(s) ○ Pt(s) | H₂O₂ (aq) | O₂(g) || H+ (aq) | Pt(s) Mn²+ (aq) + 2 e → Mn(s) Fe³+ (aq) + 3e → Fe(s) Fe(s) | Mn²+ (aq) || Fe³+ (aq) | Mn(s) Mn(s) | Mn²+ (aq) || Fe³+ (aq) | Fe(s)…

calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C Fe(s) | Fe3+ (aq, 0.0011M) || Fe3+(aq, 2.33M) | Fe(s)