An electrochemical cell is set up with the following configuration: Hg|Hg2+||Mn2+|Mn.  The solutions are, respectively, 0.1 M Hg(NO3)2 (aq) and 0.1 M Mn(NO3)2 (aq).  A voltmeter connected between the two electrodes reads -2.16 V.  b.    The standard reduction potential for Mn2+ + 2e- ® Mn is E° = -1.18 V.  Using this value as a reference, what is the standard reduction potential for Hg2+ ® Hg according to this experiment? c.     Which metal and metal ion from this system will react spontaneously when combined?

Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.

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

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

Calculate Eu for the following cell: Pt(s) | H₂(g) | H *(aq) || Pb2+ (aq) | PbSO4(s) | Pb(s) given the following standard reduction potentials. 2 H(aq) + 2e →→ H₂(g) PbSO4(s) + 2e →→ Pb(s) + SO42 (aq) O a. -0.712 V O b. +0.356 V O c. -0.356 V O d. +0.712 V O e. -0.178 V E° = 0.000 V E = -0.356 V

Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś

Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=

What statement about a galvanic cell constructed with Cut/Cu and Fe2+/Fe is correct? Standard Reduction Potentials E°red / V Cu* + e→ Cu +0.52 Fe2* + 2e-→ Fe -0.44 а. Fe(s) will reduce Cu*(aq). b. Fe(s) is a stronger oxidizing agent than Cu(s). С. The standard cell potential (E°cell) is +1.40 V. d. Fe<+(aq) is reduced at the cathode.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.

Calculate the theoretical cell potential for the following galvanic cell: Mg | Mg2+ ( 1 M) || Cu2+ (2 M) | Cu