Reference no: EM131755663

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 E^o_cell 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 E_cell if the unknown solution in the half-cell on the left has pH = 5.72?

(b) What is E_cell if the unknown solution in the half-cell on the left is 0.02020 M HCl?

(c) What is E_cell if the unknown solution in the half-cell on the left is 0.362 M HA, where HA represents a weak acid with K_a = 1.8x10^-5?

Question 4: Use the Nernst equation and data from Appendix D to calculate E_cell 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 E_cell 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 E_cell? (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