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Which chemical species is reduced in a voltaic cell represented by the the following cell diagram?...
1a) In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Zn(s)|Zn2+(aq)||H+(aq)|H2(g)|Pt(s) Select one or more: Zn/Zn2+ is the anode Eºcell is positive H+/H2 is the cathode Zn/Zn2+ is the cathode H+/H2 is the anode Eºcell is negative
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
Question 20 2.75 pts Write a balanced chemical equation for the overall reaction represented by the cell notation below. Zn(s)| Zn2+(aq) || H(aq)| H2(g)| Pt(s) O 2 H+ (aq) + Zn2+(aq) - H2(g) + Zn(s) 2 H+ (aq) + Zn(s) ZnH2(s) 2 H*(aq) + Zn(s) - H2(g) + Zn2+(aq) O H2(g) + Zn2+ (aq) → 2H+ (aq) + Zn(s) H2(g) + Zn(s) - 2 H(aq) + Zn2+(aq)
For a voltaic cell based on the reaction below, which statement is correct? Zn(s)+2H+(aq)→Zn2+(aq)+H2(g) Zn2+(aq) is oxidized at the anode. H+(aq) is reduced at the cathode. Zn2+(aq) is reduced at the anode. H2(g) is the oxidizing agent.
Choose the overall chemical reaction that takes place in a voltaic cell represented by the the following cell diagram Cr(s)| Cr3+(aq) || Fe3+(aq), Fe2+(aq) | Pt(s). Cr3+(aq) + 3Fe2+(aq) → Cr(s) + 3Fe3+(aq) O Cr(s) + 3Fe3+(aq) → Cr3+(aq) + 3Fe2+(aq) O Cr(s) + Fe2+(aq) → Cr3+(aq) + Fe3+(aq) Cr(s) + 3Fe2+(aq) → Cr3+(aq) + 3Fe3+(aq) O Cr(s) + 2Fe3+(aq) → Cr3+(aq) + 2Fe2+(aq)
What is the correct cell notation (cell diagram) for a voltaic cell based on the following reaction? 2 O2(g) + 4 H*(aq) + Zr(s) → 2 H2O2(aq) + Z4(aq) Zr(s) I ZA+(aq) || H(aq), H2O2 (aq) | O2(g) | Pt(s) O2(g) H+(aq), H2O2(aq) || ZAA+(aq) | Zr(s) Zr(s) I ZA+(aq) || H+(aq), H2O2(aq) | O2(9) Pt(s) 1 O2(g) (H*(aq) || Zr4+(aq) Zr(s)
Consider a voltaic cell al 25 degree Celsius in which the reaction is: Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2(g) It is found that the voltage (think Ecell) is +0.560 V when [Zn2+1 -0.85 M and PH2 = = 0.988 atm. What is the pH in the H2-H half-cell?
Consider the cell represented by the following line notation: Zn(s) | Zn2+ (aq) || ClO2 (aq)| ClO2(g) | Pt(s) Assuming standard conditions, calculate Eºcell: Zn2+ (aq) + 2e - Zn(s) E' = -0.76 V ClO2(g) + e - ClO2 (aq) F° = 0.95 V Express your answer to two decimal places. Eºcell
1. Identify the anode, the cathode, the reduced species and the oxidized species for the following electrochemical cells. Write the half reactions for the anode and cathode, the overall reaction. Calculate the total cell potential. a) Fe (8)| Fe (aq) (0.2 M) || Ni” (aq) (0.1 M) | Ni(s) b) Zn (s) | Zn? (aq) (1.0 x 10' M)||Cl(aq)(0.3 M) CI, (g) (0.100 bar) Pt (S) c) Pb (s) Pb2(aq) (1.0 x 10ʻM) || Cu (aq) (1.0 x 10M) Cu...
In a test of a new reference electrode, a chemist constructs a voltaic cell consisting of a Zn/Zn2 half- cell and an H2/H half-cell under the following conditions: [Zn2] = 0.042 M [H]- 19 M partial pressure of H2 =0.37 atm. Calculate Ecell at 298 K (enter to 3 decimal places). Zn2 (aq) + 2e +2H (aq) + 2e1 Eo-0.76 V E 0.00 V Zn(s) H2(g)