Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.41 V; Zn²+ (aq) |Zn(s): -0.73 V; Ni2+ (aq) | Ni(s): -0.34 V; Cu2+ (aq)| Cu(s): 3.17 V. Calculate the standard cell potential in V for the cell reaction Cu2+ (aq) + Cd(s)→Cd²+ (aq) + Cu(s) Report your answer with 2 places past the decimal point. Do not put unit in your answer.

Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M X2+ solution using the table of reduction potentials and Eq. 6 at 25 degrees C. Answer with the unit V, to two decimal places. The standard reduction potential of X is -0.24 volts.

Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG = -408.0 kJ/mol Calculate the standard cell potential, E for the reaction. E = V cell Calculate the equilibrium constant, K, for the reaction. K =

Using values from the table of standard reduction potentials, calculate the cell potential (in V) of the following cells. 2+ + (a) Fe(s) | Fe (aq) || Ag (aq) | Ag(s) V 2+ (b) Cd(s) | Cd²+ (aq) || Cr³+ (aq) | Cr(s) 2- 2+ (c) Cd(s), CdS(s) | S (aq) || Sn (aq) | Sn(s) V

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test solution)|H2(1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn²+ is -0.76 V. (Enter your answer to two significant figures.) pH = %3!

Consider the following galvanic cell at 25°C. Pt | Cr²+ (0.25 M), Cr³+ (2.0 M) || Co²+ (0.17 M) | Co The overall reaction and equilibrium constant value are given below. 2 Cr²+ "(aq) + Co2+ Calculate the cell potential & for this galvanic cell and AG for the cell reaction at these conditions. + (aq) → 2 Cr³+ (aq) + Co(s) K = 2.79x107

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Consider the following cell: Ni(s)|Ni2+(aq, 0.100 M)||Cl–(aq, 0.200 M)|Cl2(g, 1.50 atm)|Pt If the standard voltage for this cell is 1.59 V at 25oC, calculate the voltage of this cell.