An electrochemical cell is constructed using 0.50 M NiSO4 and a solid nickel electrode in one half cell and 2.0 M ZnCl2 and a solid zinc electrode in the other half cell. The cell is run at 25oC. What voltage would be expected from this cell? Enter the response to 2 significant figures.

Eocell for the reaction ZnBr2(aq) Zn(s) + Br2(aq) is 1.8491 V. What voltage would you expect from a battery at 25 oC, with [ZnBr2] = 0.833 M and [Br2] = 0.450 M? Please enter your answer with three sig figs.

One-half of an electrochemical cell consists of a pure nickel electrode in a solution of Ni2+ ions; the other half is a cadmium electrode immersed in a Cd2+ solution. Use the following standard emf series Table (if required). Standard Electrode Electrode Reaction Potential, V" (V) Au³+ + 3e → Au +1.420 O2 + 4H+ + 4e Pr2+ + 2e 2H2O +1.229 Pt -+1.2 Ag+ + e Fe+ + e → Ag Fe2+ +0.800 +0.771 Increasingly inert (cathodic) O2 + 2H,O + 4e Cu²+ + 2e 4(OH) +0.401 Cu +0.340 2H* + 2e Pb2+ + 2e H2 0.000 Pb -0.126 Sn2+ + 2e Sn -0.136 Ni2+ + 2e Ni -0.250 Co2+ + 2e Cd²+ + 2e Fe+ + 2e Co -0.277 Cd -0.403 Fe -0.440 Cr+ + 3e Cr -0.744 Increasingly active (anodic) Zn2+ + 2e¯ Zn -0.763 AF+ + 3e Al -1.662 Mg²+ + 2e Mg -2.363 Na+ + e –→ Na -2.714 K* + e -→ K -2.924 If the cell is a standard one, write the spontaneous overall reaction and calculate the voltage that is generated. Ni2+ + Cd ---> Ni + Cd2+ and +0.153 V Ni + Cd2+ ---> Ni2+ + Cd and +0.153 V Ni2+ + Cd ---> Ni + Cd2+ and -0.153 V Ni + Cd2+ Ni2+ + Cd…

A voltaic cell is constructed from a standard Cu²+ Cu half cell (E° red 0.337V) and a standard Br2 |Br half cell (E° 1.080V). red (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: + + The cathode reaction is: + The spontaneous cell reaction is: + The cell voltage is V. + + ↑