For the cell shown, the measured cell potential E cell -0.365; V at 25 degrees * C . Pr(s)|H 2 (g,0.803 am)|H^ + (aq,?M)||Cd^ 2+ (aq,1.00 M)|Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values E ^ o are 2H^ + (aq)+2e^ - longrightarrow H 2 (g) E ^ o = 0.00V Cd^ 2+ (aq)+2e^ - longrightarrow Cd(s) E ^ o= - 0.403V Calculate the H^ + concentration.

For the cell shown, the measured cell potential, Ecell, is –0.3525 V at 25 °C. Pt(s) | H, (g, 0.851 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H* (аq) + 2е H, (g) E° = 0.00 V Cd²+(aq) + 2 e¯ → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H*] =

Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 2+ (a) Ni(s) | Ni (ag) || Ag" (ag) | Ag(s) V 2+ (b) Zn(s) | Zn (ag) || Co 2+ (ag) | Co(s) 2- 2+ (c) Zn(s), ZnS(s) | s´ (ag) || Sn" (ag) | Sn(s)

Using the values from the table of standard reduction potentials, calculate the cell potentials of the following cells: (a) Ga(s) | Ga³"(aq) || Ag*(aq) | Ag(s) (b) Zn(s) | Zn²-(aq) | Cr**(aq) | Cr(s) (c) Fe(s), FeS(3) | S² (aq) | Sn²*(aq) | Sn(s) Calculate the standard free energy change of the following reactions using the standard cell potentials for the half reactions that are involved: (a) Fe(s) + Hg;*"(aq) →F²²*(aq) + 2 Hg(4) (b) Fe*"(aq) + Ag(s) + CI (aq) → Fe²"(aq) + AgC(s) Use the Nernst equation to calculate the cell potential of the given cell at 298K: 12 Ag"(aq)(0.50 M) + Ni(s) → 2 Ag(s) + Ni²^(aq)(0.20 M) Write the equilibrium expressions for each of the following reactions: (a) CaCO,(s) 2C2²*(aq) + CO,²-(aq) (b) Mg;(PO4);(s) 23 Mg²*(aq) + 2 PO,"(aq) (c) CO(g) + NO;(g)=C0;(g) + NO(g) Which of the following is more likely to precipitate the sulfate ion? (a) PbSO4(9) Pb²*(aq) + SO,²"(aq) K= 1.8 × 10 (b) CASO,(s) #Ca²*(aq) + SO,²-(aq) K=9.1 × 10-6

Consider the same diagram of a galvanic cell as in previous question,                        where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as follows:              Ag+(aq)   +  e–   -->  Ag(s);    Eo =   0.80 V             Ni2+(aq)  +  2e–  -->  Ni(s);     Eo = – 0.23 V          What is the Ecell at 25oC when the electrolyte concentrations are: [Ag+] = 1.3 x 10–5 M and [Ni2+] = 0.10 M.            (A) 1.15 V          (B) 1.30 V          (C) 0.76 V          (D) 0.91 V

Calculate Ecell for the following cell: Pt(s) | H2(g) | H *(aq) || Pb2*(aq) | PBSO4(s) | Pb(s) given the following standard reduction potentials. 2H*(aq) + 2 e ® H2(g) PbSO4(s) + 2 e ® Pb(s) + SO42-(aq) Oa. +0.712 V Ob. +0.356 V Oc. -0.712 V Od.-0.178 V Oe. -0.356 V

The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the Ht concentration. Pt(s) | H, (g, 0.807 bar) | H*(aq, ? M) || Cď²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell and their respective standard reduction potential values, E", are given. 2 H*(aq) + 2 e- Cd2+ (aq) + 2 e- E' = 0.00 V E° = -0.403 V H, (g) Cd(s) %3D [H*] = M

For the cell shown, the measured cell potential, Ecell, is –0.3521 V at 25 °C. Pt(s) | H,(g, 0.785 atm) | H* (aq, ? M) || Cd²*(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H* (aq) + 2e- - H, (g) E° = 0.00 V Cd²* (aq) + 2e" - Cd(s) E° = -0.403 V Calculate the H* concentration. [H*] = M

26. Given the following electrode (reduction) potentials: Ag* + e --> Ag; E° = 0.80 V Zn2+ + 2e --> Zn; E° = -0.76 V For a Voltaic cell represented by the cell notation: Zn(s)|Zn2*(aq)||Ag*(aq)|Ag(s), what is the cell potential (Ecell) when the electrolyte concentrations are as follows: [Ag*] = 1.3 x 10-5 M, and [Zn2*) = 1.0 M ? (A) 2.36 V (B) 1.56 V (C) 0.84 V (D) 0.04 V

Using these metal ion/metal standard reduction potentials: Cd2+ (aq)| Cd(s): -0.38 V; Zn2+ (aq) Zn(s): -0.78 V; Ni2+ (aq) |Ni (s): -0.29 V; Cu2+ (aq)| Cu(s): 0.30 V. Calculate the standard cell potential in V for the cell reaction Cu²+ (aq) + Cd(s)→Cd²+ (aq) + Cu(s) Report your answer with 2 places past the decimal point. Do not put unit in your answer. Type your answer...