Sketch a diagram of a galvanic cell represented by the following shorthand notation: Pb(s)|Pb2+ (aq)||Br2(1), Br (aq)|P...
d. To the right is a diagram of a galvanic cell. Based on the Eº values listed below: i. label the anode and the cathode; ii. draw an arrow indicating the direction of electron flow through the lightbulb; and iii. indicate the direction that the R* and the NO3 in the salt bridge will move. Pb 2 KNO, Aut (aq) + e - Au (s) Eº = 1.692 V Pb2+ (aq) + 2 e - Pb (s) Eº = -0.126...
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
For the electrochemical cell Pt(s) | Sn2+(aq), Sn4+(aq) || Pb2+(aq) | Pb(s), what is the function of the Pt(s)? Pt is the anode and is a reactant in the overall cell reaction. Pt is the anode and does not appear in the overall cell reaction. Pt is the cathode and is a product in the overall cell reaction. O Pt is the cathode and does not appear in the overall cell reaction. O
II Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. 0 |Anode half-reaction: OD PbCl, (s) Pb(s) +201 – Cathode half-reaction: 2.AgCI() 2€ - PbCl,(s) KCl(aq) [ 285(0) AgCl(s) KCl(aq) 2 AgCl(s) Shorthand notation: Ag(s) | Pb(s) PbCl,(s) C1- (aq)] [c1-(aq)] | AgCl(s)) | 2 Ag(s) Answer Bank 2498) Ag(e) PbCly(@) Pb(8) 2.AgCI() CI+(ag) AgCl(s)
6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(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)
Saved Question 8 (1 point) Saved For the cell diagram Pt(s) | Br2(1) | Br-(aq) || Cl-(aq) | Cl2(g) | Pt(s) which reaction occurs at the anode? O Cl2(g) + 2Br (aq) --> 2C1-(aq) + Br2(1) O Br2(l) +2e --> 2Br" (aq) O 2Br"(aq) --> Br2(I) + 2e O Cl2(g) +2e --> 2014(aq) O 2014(aq) --> Cl2(g) + 2e
What is undergoing reduction in the redox reaction represented by the following cell notation? Pb(s) | Pb2+(aq) | | H+(aq) H2 | (g) | Pt A. Pb(s) B. Pt C. Pb2+(aq) D. H2(g) E. H+(aq) We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
8. Using the cell notation Cr3+ (aq, 0.0150 mol/L)/Cr(s)|| Pb(s)|Pb2+ (aq, 0.0355) A. (10 pts) Complete the table below for the cell as written in the above notation. B. (5 pts) What is the balanced net ionic equation represented? C. (10 pts) If the cell is constructed, what is the cell potential initially measured. Assume 25.00°C D. (5 pts) is the reaction spontaneous as written? Why or why not? (10 pts) If the cell is permitted to proceed to equilibrium,...
Suppose the galvanic cell sketched below is powered by the following reaction: Ni(s)+Pb(NO3),(aq) → Ni(NO3)2(aq)+Pb(s) E1 S1 S2 Write a balanced equation for the half-reaction that happens at the cathode of this cell. Write a balanced equation for the half-reaction that happens at the anode of this cell. Of what substance is E1 made? Of what substance is E2 made? What are the chemical species in solution S1? What are the chemical species in solution S2?