For the electrochemical cell 2 Al(s) + 3 Mn2 (aq)→ 2 Al (aq) + 3 Mn(s) (E° = 0.48 V, [A3] = 1.0 M), what is the value of E when [ Mn2'] = 0.060 M? Assume T is 298 K %D %3D

For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M), what is the value of E when [ Mn²⁺] = 0.089 M? Assume T is 298 K

For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M), what is the value of E when [ Mn²⁺] = 0.018 M? Assume T is 298 K

A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e¯ → Ag(s) + Cl¯(aq) E°red = 0.2223 V And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0903 V. What is the standard cell potential for this cell in V?

For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the ratio [Fe²⁺]/[Cd²⁺] when E = 0.001 V? Assume T is 298 K

At 298 K, what is E (in V) for the electrochemical cell below when [Cd2+] = 4.500 M and [Cu2+] = 0.009 M ?  Cd(s) | Cd2+(aq) || Cu2+(aq) | Cu(s) Cu2+ (aq) + 2e– →  Cu(s) 0.34 Cd2+ (aq) + 2e– →  Cd(s) –0.40

Consider the following electrochemical cell at 298 K where the source of Cu2+ (aq) is the sparingly soluble salt CuX. Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s) Zn2* + 2e = Zn E° = -0.76 V Cu2+ + 2e = Cu E° = 0.34 V If the potential created from this cell = 1.03 V, what is Ksp for CuX? O 1.9x10-9 3.8x10 12 4.6x10 6 2.0x10 7

For the electrochemical cell 2 Al(s) + 3 Mn2*(aq) – 2 Al**(aq) + 3 Mn(s) (E° = 0.48 V, [AI3*] = 1.0 M), what is the value of E when [ Mn2*] = 0.091 M? Assume T is 298 K %3D

For the electrochemical cell 2 Al(s) + 3 Mn²+ (aq) → 2 Al³+ (aq) + 3 Mn(s) (E° = 0.48 V, [A1³] = 1.0 M), what is the value of E when [Mn²+] = 0.026 M? Assume T is 298 K

Predict the products at the anode and the cathode obtained from electrolysis of a 1 M Znl2 solution. Note that 2 H20(1) + 2e → H2(g) + 2 OH(aq) E°red = -0.83 V O2(g) + 4 H*(aq) + 4e¯ → 2 H20(1) I2(s) + 2e → 2 I'(aq) Zn2*(aq) + 2e* → Zn(s) E°re = +1.23 V red E°red = +0.54 V E°, -0.76 V red = (Show work for full or partial credit.) The product at the anode is 12(s). The product at the cathode is Zn(s). The product at the anode is O2(g) and H*(aq). The product at the cathode is Zn(s). None of these The product at the anode is Zn(s). The product at the cathode is O2lg) and H*(aq). The product at the anode is O2lg) and H*(aq). The products at the cathode are H2(g) and OH (aq). The products at the anode are H2(g) and OH"(aq). The product at the cathode is O2(g) and H*(aq). The product at the anode is Zn(s). The product at the cathode is I2(s).