The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76 V: Zn(s) + 2H+ (aq) → Zn2+ (aq) + H2(g) With PH2 = 1.0 atm and [Zn2+] = 1.0 M, the cell potential is 0.66 V. The concentration of H+ in the cathode compartment is ________ M.   A. 1.0 × 10-12 B. 2.0 × 10-2

Construct a galvanic cell from MnO4- (aq)/MnO2 (s) and H2 O2 (aq)/H2 O (l).a) Write a balanced equation for the cell.b) What is the value of E°cell?    standard Ni (s) | Ni2+ (aq) || Ag+ (aq) | Ag (s) is constructed and the standard cell potential is1.03 V.a) Write a balanced reaction for the cell.b) What is ∆G° for the cell?

Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn(s)+Cu2+(aq)⟶Cu(s) +Zn2+(aq)          Eocell=1.1032 V What is the cell potential for a cell with a 2.214 M solution of Zn2+(aq) and 0.1456 M solution of  Cu2+(aq) at 437.7 K?

Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these

Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣  Au3+(aq,? M) ∣ Au (s)Determine the standard cell potential and if the cell is more spontaneous or less spontaneous at standard conditions.

Calculate AG for the following cell reaction: Tl(s) | Tl+ (aq) || Ni²+ (aq) | Ni(s) From AG, determine the standard potential for the half-reaction Tl+ (aq) + e → Tl(s) AG; for Tl+ (aq) is -32.4 kJ/mol. 2+ AG; for Ni²+ (aq) is -45.60 kJ/mol. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction Ni²+ (aq) + 2e Ni(s) AG = J Standard Potential, E° (V) -0.23 Standard reduction potential for the half-reaction = V

Name: NetID: 5. Determine the standard cell potential (in V to two decimal places) for the following redox reactions. 2+ (a) Al(s) | Al³+ (aq, 1 M) || Cu²+ (aq, 1 M) | Cu(s) (b) Al(s) + NO3(aq) + 4H+ (aq) - Al³+ (aq) + NO(g) + 2H₂O(1) 13+ A: 2.00 A: 2.62

If an alkaline battery produces a cell potential of 1.66 V, what is the value (in kj) of ΔGcell? The half-reactions in alkaline batteries are: ZnO(s) + H2O(l) + 2e^-  --------> Zn(s) + 2OH^- (aq) 2MnO2(s) + H2O(l) + 2e^-  -----------> Mn2O3(s) +  2OH^- (aq)

What is the overall cell reaction and the standard cell potential of a galvanic cell employing the following half-reactions ? NiO 2(s) +2H 2 O+2e^ -. ---> Ni(OH) 2(s) +2OH^- (aq) E ^ 0 = 0.49V   Fe(OH) 2(s) +2e^ - ----> Fe (s) +2OH^- (aq) E ^ 0 = - 0.88 V

What is the calculated value of the cell potential at 298 K for an 2+ Cu²+ concentration is 3.83 × 10-4 M and the A1³+ concentration is 1.12 M? Ecell electrochemical cell with the following reaction, when the 2+ 3Cu²+ (aq) + 2Al(s) → 3Cu(s) + 2A1³+ (aq) V The cell reaction as written above spontaneous nonspontaneous for the concentrations given.