Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq) 2.75 M Cd+2 (aq) 0.0125 M • What is the value of potential for the spontaneous reaction that occurs as the cell operates at 25°C? Ecell = • As the cell operates spontaneously under these conditions, which electrode is the cathode of the cell? Cd Ag • Which Electrode loses mass as the cell operates under these conditions? Ag Cd

4 Consider the voltaic cell: Sn(s) | Sn*2(aq) II Fe*3(aq) | Fe*2(aq) a) Write the overall cell reaction. b) Calculate the standard cell potential at 25°C. c) Calculate the change in free-energy of the reaction at 25°C d) What is the maximum work you can obtain from 25.0 g of nickel? e) What is the value of the equilibrium constant of the reaction? f) Which is the stronger oxidizing agent: Sn*2 or Fe*3? Explain

An electrochemical cell with an overall cell reaction shown below has a standard cell potential of 0.48 V. 2 Al(s) + 3 Mn2*(aq) → 2 Al3+(aq) + 3 Mn(s) i. How many electrons were involved in the overall reaction? ii. What is the AG° of the reaction? iii. What is the Keq of the reaction? iv. What is the new cell potential at 25°C if the initial concentrations of the ions are [Al3+] = 1.50 M, and [Mn2+] = 0.50 M?

What is the potential of the reaction?

O ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e → 2 Br (aq) =+1.065 V (red 2 H,O(1)+2e Н, 9)+2ОН (аq) -0.83 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. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 3 significant digits. Explanation Check

35. Calculate the equilibrium constant at 25 °C using standard cell potential data, Sn(s) + CuSO4(aq) = Cu(s) + SnSO4 (aq)

A chemist designs a galvanic cell from the following two half-reactions Ered = +0.96 V NO3(aq) + 4H+ (aq) + 3e¯ → NO(g) + 2H₂O (1) Ered +0.153 V Cu²+ (aq) + e¯ → Cut (aq) The standard cell potential for this galvanic cell is [Select] The standard free energy for this galvanic cell is AG [Select] The equilibrium constant (K) for this galvanic cell is [Select] = V.

Consider the following voltaic cell at 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? The overall cell reaction is Al3+(0.20 M, ag) Al3*(0.75 M, ag) and Ecell = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) AI3+(0.20 M, ag) and Ecell = +0.0113 V. None of these The overall cell reaction is Al3+(0.20 M, aq) Al3*(0.75 M, ag) and Ecell = +0.0113 V. There is no overall cell reaction and Ecell 0.00 V. %3D The overall cell reaction is Al3+(0.75 M, aq) Als*(0.20 M, aq) and Ecell = -0.0113 V.

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 21 (aq) + Cl2(g) → 2(s) + 2CI(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate v the Cl2 electrode v the I electrode. Anions migrate v the salt bridge v the Cl2 compartment.

Sn(s) | Sn2+ (aq, 1.8 M) || Agt(aq, 0.055 M) | Ag(s) Consider the cell notation of a galvanic cell given above and the following reduction potentials: Sn- (aq) + 2e- → Sn(s) E° = -0.14 V Ag (aq) + e- → Agis) ED=0.80 V 1. The number of electron transferred in the net reaction is [Select] 2. The E is [Select] 3. The value for Q is (Select] 4. The cell potential for the cell is [Select] V.