The standard cell potential (E° cell) for the reaction below is +1.10 V. The cell potential for this reaction is V when the concentration of [Cu2+] = 1.0 x 10-5 M and (Zn2+ = 3.0M. Zn (s) + Cu 2+ (aq) Cu (s) + Zn 2+ (aq) a. 0.78 O b. 0.94 O c. 1.10 d. 1.42 O e. 1.26

What is the net reaction for the cell?  Is it .44V or .22V?

For the cell: Zn(s) + 2H† (aq) →→ Zn2+(aq) + H2 (g) If [Zn2+] = 1 M, PH2 = 1 atm, and E = 0.123 V what is pH?

Calculate the cell potential of each of the following electrochemical cell at 25oC. a. Pt|H 2 (8.00 atm)|H + (1.00 x 10 -3 M)‖Ag + (0.00549 M)|Agb. Pt|H 2 (1.00 atm)| H + (pH = 5.97 ) ‖ H + (pH=3.47)|H 2 (1.00 atm)|Ptc. Pt|H 2 (0.0361 atm)|H + (0.0175 M)‖H + (0.0175 M)|H 2 (5.98 x 10 -4 atm)|Pt   Please solve and give explanations steps.

An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a. What is the potential of the cell at 25°C if the copper electrode is placed in a solution in which [Cu²+] = 5.9 x 10-4 M? Ecell = V b. The copper electrode is placed in a solution of unknown [Cu²+ ]. The measured potential at 25°C is 0.222 V. What is [Cu²+ ] ? (Assume Cu²+ is reduced.) [Cu²+] = M

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

17. Calculate the cell potential of the cell described below: 2+ Al(s) | Al³+ (aq) (1.00 M) || Pb²+ (aq) (1.00 M) | Pb(s)

Determine the cell potential for the following cell Ni(s) | Ni2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Ni2+(aq) and Ag+(aq) are –0.25 V and +0.80 V, respectively.   A.  1.05 V   B.  1.10 V   C.  1.00 V   D.  1.16 V   E.  0.94 V