Question 1: The standard electrode potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Use the data in Appendix D to determine which of the following is capable of reducing Eu3+(aq) to Eu2+(aq) under standard state conditions?
(a) ln(s)
(b) La(s)
(c) Sn2+(aq)
(d) HCN(aq)
Question 2: Determine Eocell for each of the following voltaic cells:
Enter your answer with 3 significant digits.
Enter scientific notation as 1.23E4.
(a) F2(g) is reduced to F- (aq) and Fe(s) is oxidized to Fe2+(aq).
(b) Cu2+(aq) is reduced by Zn(s).
(c) MgI2(aq) is produced from Mg(s) and I2(s).
Question 3: Answer the following questions regarding the cell diagram shown in the figure below.
Enter part (a), (c) with 2 significant digits and part (b) with 3 significant digits. Enter scientific notation as 1.23E4.
(a) What is Ecell if the unknown solution in the half-cell on the left has pH = 5.72?
(b) What is Ecell if the unknown solution in the half-cell on the left is 0.02020 M HCl?
(c) What is Ecell if the unknown solution in the half-cell on the left is 0.362 M HA, where HA represents a weak acid with Ka = 1.8x10-5?
Question 4: Use the Nernst equation and data from Appendix D to calculate Ecell for each of the following cells.
Enter your answer with 3 significant digits. Enter scientific notation as 1.23E4.
(a) Mn(s) | Mn2+(0.24) M || Cr3+(0.27 M), Cr2+(0.12 M) | Pt(s)
(b) Mg(s) | Mg2+(0.050) M || [Al(OH)4]-(0.46 M), OH-(0.0100 M) | Al(s)
Question 5: Calculate Ecell for the oxidation of Cl-(aq) to Cl2(g) by PbO2(s) in an acidic solution for the following values of [H+] or pH. Assume the amounts of all other reactants and products, except for H+, are in their standard states.
Round your answer to 3 decimal places. Do not use scientific notation.
(a) [H+] = 4.7 M
(b) pH = 4.02
Question 6: A concentration cell is constructed from two hydrogen electrodes connected by a salt bridge. The pressure of H2 is 1.00 atm in each hydrogen electrode. One electrode is immersed in a solution with [H+] = 1.0 M and the other in a solution with 0.15 M NH3. What will be the value of Ecell? (Hint: First, determine the [H+] in the NH3 solution by considering the equilibrium problem.)
Enter your answer with 3 significant digits. Enter scientific notation as 1.23E4.
Question 7: Determine the quantity indicated for each of the following electrolyses. Enter scientific notation as 1.23E4.
(a) [Cu2+] remaining in 506 mL of a solution that was originally 0.563 M CuSO4, after passage of 2.02 A for 4.40E2 s and the deposition of Cu at the cathode. (Note: 1 A = 1 C s-1)
(b) The time required to reduce [Ag+] in 392 mL of AgNO3(aq) from 0.180 to 0.122 M by electrolyzing the solution between Pt electrodes with a current of 4.01 A. (Note: 1 A = 1 C s-1)
Question 8: Suppose that a fully charged lead-acid battery contains 2.72 L of 5.00 M H2SO4. What will be the concentration of HSO4- in the battery after 2.13 A of current is drawn from the battery for 2.7 h?
Pb(s) + PbO2(s) + 2H+(aq) + 2HSO4-(aq) → 2PbSO4(s) + 2H2O(l)
Enter your answer with 3 significant digits.
Attachment:- Assignment File.rar