4. a. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr. b. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of molten NaBr in the presence of molten MgF2. State clearly which ion is oxidized at the anode and which ion is reduced at the cathode. c. Write a balanced equation to represent the overall reaction you would expect to occur in the electrolysis of aqueous NaBr. Hint: remember overvoltage: 2H2O(1) → O2(g) + 4H*(aq)+ 4e¯ 2H2O(1) + 2e¯ → H2(g) + 2OH´(aq) E° = 0.82V, ~1.4V with overvoltage (oxidation) E° = -0.42V, ~ -1V with overvoltage (reduction) d. Clearly explain why the products of the three processes are not the same.

6. Consider a galvanic cell consisting of an Al electrode placed in a 1 M Al(NO3)3 solution and a Ag electrode placed in a 1 M AgNO3 solution. a.)Write the half-reaction which occurs at the anode. b.)Write the half-reaction which occurs at the cathode c.)Write a balanced net ionic equation for the galvanic cell. d.)Calculate the standard emf of the cell e.)Give the cell diagram for the reaction occurring in this galvanic cell. f.)What is oxidized? g.)What is the oxidizing agent?

Element A has a standard reduction potential of +0.74V, whereas Element B has a standard reduction potential of -1.15V. Which of the following statements is correct with respect to building a Galvanic cell with these two elements? A. A will be the cathode, B will be the anode, and the cell potential will be positive. B. A will be the cathode, B will be the anode, and the cell potential will be negative. C. A will be the anode, B will be the cathode, and the cell potential will be positive. D. A will be the anode, B will be the cathode, and the cell potential will be negative. E. The anode, cathode, and cell potential must all be experimentally determined.

A student contructs an electrochemical cell consisting of a silver electrode in a 0.10 M solution of AgNO3 connected through a salt bridge to a zinc electrode in a 0.10 M solution of Zn(NO3)2. The potential across the electrochemical cell was measured as 1.52 V. a. Write the half reactions for the cathode and the anode. b. Use standard notation to represent this electrochemical cell.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ MnO₂(s)+4H(aq) +2e → Mn(aq) + 2 H₂O(1) Zn²+ (aq)+2e Zn(s) Answer the following questions about this cell. standard reduction potential E=+1.23 V red E =-0.763 V red

3. Write the equation for the oxidation of water, 4. Write the equation for the reduction of water. 5. Calculate the mass of zinc that will be deposited if a current of 0.40 Amps is applied for 25 minutes to a ZnSO4 solution.

7. Fig. 7.1 shows a simplified diagram of the electrolysis of sodium chloride solution, used to produce chlorine in industry. concentrated sodium chloride solution anode cathode gas 111 chlorine gas permeable membrane hydrogen Fig. 7.1 The balanced equation for the overall chemical change that occurs in the process shown in Fig. 7.1 is 2NaCl + 2H₂O → 2NaOH + Cl₂ + H₂ a. Show that the relative formula mass of sodium chloride is 58.5 sodium hydroxide solution b. Calculate the number of moles in 234g of sodium chloride. Show your working. Number of moles= Volume= c. Calculate the volume of chlorine molecules produced at room temperature and pressure, when 234g of sodium chloride are electrolysed. (1 mole of chlorine molecules has a volume of 24 dm³ at room temperature and pressure). Show your working

10. A galvanic cell was set up using zinc and tin. The set up is shown below. Zn Sn Salt Bridge 1.0 M Sn²+ 1.0 M Zn²+ Choose 2 of the following statements to explain. Be sure to include balanced equations as part of your response. a. Using the reduction potential table, predict the cell voltage for this cell. b. What is the reaction at the cathode? c. Which electrode do you expect will lose mass? d. What is the direction of the movement of ions and the electron flow?

A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential Exed half-reaction 2 H2O(1)+2e → H2(g)+2OH (aq) Ε red -0.83 V 2+ Zn(aq)+2e →>> Zn(s) E = = -0.763 V 'red Answer the following questions about this cell.