Answer only part 3 and 4 Answer the following questions related to the given ele
ID: 1005766 • Letter: A
Question
Answer only part 3 and 4
Answer the following questions related to the given electrochemical cell.
1. Answer the following questions under standard conditions
(a) The half-cell containing Ag2+/Ag3+ is the cathode .
(b) The half-cell containing H+/H2 is the anode .
(c) What is E°cell (in V)? Report your answer to three decimal places in standard notation (i.e., 0.123 V). 1.800 V
2. (a) Which one of the following balanced chemical reactions describes the process occurring in the electrochemical cell?
Correct: 2Ag3+(aq) + H2(g) 2H+(aq) + 2Ag2+(aq).
(b) What is G° (in kJ/mol) for the process that is occurring in the electrochemical cell? Report your answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol). -3.47×102 kJ/mol
3. The electrochemical cell is comprised of a Pt electrode in a 5.63 × 10-2 M solution of Ag3+ and 6.33 × 10-1 M solution of Ag2+ coupled to a Pt electrode where the [H+] is 6.00 M and the partial pressure of H2(g) is 1.610 atm. The temperature of this cell is held constant at 298.15 K
(a) Under these conditions, the half-cell containing Ag2+ and Ag3+ is the anode cathode .
(b) Under these conditions, the half-cell containing H+ and H2 is the anode cathode .
(c) What is Ecell (in V) for this electrochemical cell? Report your answer to three decimal places in standard notation (i.e., 0.123 V).
4. Answer the following questions under the conditions described in question 3.
(a) Which one of the following balanced chemical reactions describes the process occurring in the electrochemical cell?
2Ag3+(aq) + 2H2(g) 4H+(aq) + 2Ag2+(aq).
2Ag3+(aq) + H2(g) 2H+(aq) + 2Ag2+(aq).
4H+(aq) + 2Ag2+(aq) 2Ag3+(aq) + 2H2(g).
2H+(aq) + 2Ag2+(aq) 2Ag3+(aq) + H2(g).
(b) What is the value of G (in kJ/mol) for the process occurring in this electrochemical cell under the conditions described in Part B? Report your answer to three significant figures in scientific notation (i.e., 1.23e2 kJ/mol)
Ag3+(aq) + e Ag2+(aq)E° = 1.800 V 2H+(aq) + 2e H2(g)
E° = 0.000 V
Explanation / Answer
Q.3: (a):Under these conditions, the half-cell containing Ag2+ and Ag3+ is the cathode .
(b) Under these conditions, the half-cell containing H+ and H2 is the anode.
(c): The balanced chemical reaction occuring is
2Ag3+(aq) + H2(g) ------- > 2H+(aq) + 2Ag2+(aq).
E(cell) = E0(cell) - (0.0591 / n) x log([Ag2+(aq)]2 x[H+(aq)]2)/ ([Ag3+(aq)]2 xP(H2))
=> E(cell) = 1.800 V - (0.0591 / 2) x log[(0.633)2 x (6.00)2 / (0.0563)2x1.610 ]
=> E(cell) = 1.698 V (answer)
Q.4:
(a): The balanced chemical reaction occuring is
2Ag3+(aq) + H2(g) ------- > 2H+(aq) + 2Ag2+(aq)
(b): deltaG = - nFE(cell)
=> deltaG = - 2 x 96500 x 1.698 = - 327.7 kJ/mol
=> deltaG = - 3.28x102 kJ/mol (answer)