4. a) Determine Eº for the cell Pt (s) | Cl2 (g) | Cl− (aq) ||
Pb2+ (aq), H+ (aq) | PbO2 (s).
b) What is the Standard Gibbs free energy of this reaction?
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Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
For the following electrochemical cell: Fe(s)| Fe3+(aq) || Cl(aq) | Cl2(g)|| Pt(s) a) Write the Cell Reaction for this Cell. b) Identify the Anode and Cathode.
E6D.3(b) Calculate the standard potential of the cell Pt(s) cystine(aq), cysteine(aq)|| H*(aq)|O2(g)|Pt(s) and the standard Gibbs energy of the cell reaction at 25°C. Use EⓇ =-0.34 V for cystine(aq) + 2 H+(aq) + 2e → 2 cysteine(aq).
e) 20 g 4. Referring to the table of Standard Cell Potentials below, determine the standard cell potential for the following reaction: Pb2+(aq) + 2 Cl(aq) ---> Pb(s) + Cl2 E° -0.126 +1.360 Pb2+ (aq) + 2e ---> Pb (s) Cl2 + 2e- ---> 2 cl-(aq) a) +1.486 b) +1.468 c) +1.234 d) -1.234 e) -1.486
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M a. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each. b. Determine what reaction occurs overall, and calculate the Eo cell for this electrochemical cell. c. Make a drawing of this cell, and label the ANODE and the CATHODE....
What is the shorthand notation that represents the following galvanic cell reaction? Sn2+(aq) + Cl2(g) → Sn3+(aq) + 2 Cl-(aq) A) Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) B) Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) C) Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) D) Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
Question 5 (1 point) For the cell diagram Pt(s) | Br2(1) | Br"(aq) || C1-(aq)| Cl2(g) | Pt(s) which reaction occurs at the cathode? O 2C1-(aq) --> Cl2(g) + 2e- O 2Br (aq) --> Br2(1) + 2e O Br2(l) +2e --> 2Br (aq) O Cl2(g) + 2Br (aq) --> 2C1-(aq) + Br2(1) O C12(g) + 22 --> 2C1“(aq)
Balance each redox reaction occurring in acidic aqueous solution. a. PbO2(s) + (aq) Pb2+(aq) + 12(s) b. SO32-(aq) + MnO4 (aq) — 3042-(aq) + Mn²+(aq) c. S2032-(aq) + Cl2(g) 8042-(aq) + Cl²(aq)
What is the overall cell reaction for the galvanic cell given in shorthand below? Pt(s) i H2(g) | H+(aq) || Cl2(g) CI(aq) Pt(s) A. Pt(s) + H2(g) + CI+(aq) - Pt(s) + 2 H+(aq) + 2 C12(g) B. 2 H+(aq) + 2 C12(g) → 2 HCl(aq) CH2(g) + Cl2() - 2 H+(aq) + 2 CİH(aq) None of these is correct.
Consider the following cell: Ni(s) | Ni2+(aq, 1.00 M) || Cl(aq, ? M) | Cl2(g, (5.100x10^-1) atm) Pt(s) For this cell, E° = +1.59 V and E = + (1.8x10^0) V at 25°C. Calculate the Cl(aq) concentration in the cathode compartment. Note: 10^0 = 1 The red text below just means to enter your final answer in regular scientific notation. Express your answer to two significant figures. Note: Your answer is assumed to be reduced to the highest power possible....