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3. Calculate the cell potential for the voltaic cell based on the following half reactions at...
Draw the voltaic cell that will give the most positive cell potential choosing from the following...
Draw the voltaic cell that will give the most positive cell potential choosing from the following half reactions: Eo (vs. SHE) Zn2+ (aq) + 2e- Zn (s), Eo= -0.76 Al3+ (aq) + 3e- Al (s), Eo= -1.66 Cr3+ (aq) + 3e- Cr (s), Eo= -0.74 Co2+ (aq) + 2e- Co (s), Eo= -0.28
Use the following half-reactions to write 3 spontaneous reactions, calculate E°cell for each reaction, what is...
Use the following half-reactions to write 3 spontaneous
reactions, calculate E°cell for each reaction, what is
the n number (number of electrons transferred).
Au+ (aq) + e− → Au
(s) E° = 1.69
V
N2O (g) + 2H+ (aq) + 2 e− →
N2 (g) + H2O (l) E° =
1.77 V
Cr3+ (aq) + 3 e− → Cr
(s) E° = -0.74 V
Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
Calculate the E of the cell based on the following half reactions: VO2+ (aq) + 2H+...
Calculate the E of the cell based on the following half reactions: VO2+ (aq) + 2H+ (aq) + e- ----> VO2+ (aq) + H2O (l) Zn (s) --->Zn2+ (aq) + 2e- Under the following condition: T = 25°C [VO2+] = 2.0 M [H+] = 0.5 M [VO2+] = 1.0 x 10-2 M [Zn2+] = 0.10 M
A voltaic cell is set up with a beaker on the left containing 1.0 M AgNO...
A voltaic cell is set up with a beaker on the left containing 1.0 M AgNO 3 and a silver electrode, and a beaker on the right containing 1.0 M Cr(NO 3) 3 and a chromium electrode. Given the following standard reduction potentials, answer the 3 questions below: Eº Ag+(aq) + 1e → Ag(s) +0.80 V Cr3+(aq) + 3e → Cr(s) -0.73V Part a. Write out the half-cell reaction that occurs at the anode of the voltaic cell. Part...
What is the E cell for the cell represented by the combination of the following half-...
What is the E cell for the cell represented by the combination of the following half- reactions? 2Hg2+(aq) + 2e" =Hg22+(aq); E°= 0.92 V Cr3+ (aq) + 3e Cr(s); E°= -0.74 V O 1) -0.18 V O2) 0.18 V 03) 1.28 V 4) 1.66 V 05) 2.12 V
A voltaic cell is based on the following half reactions at 25°C: Ag + e- →...
A voltaic cell is based on the following half reactions at 25°C: Ag + e- → Ag E = 0.8V H2O2 + 2H+ + 2e - → 2H20 E° = 1.78V Predict whether E cell is larger or smaller than Eºcel for the following cases. (a) (Ag +) = 1.0 M, (H2O2) = 2.0 M, [H*] = 2.0 M (b) (Ag +) - 2.0 M, (H2O2) = 1.0 M, [H) - 1.0 x 10'M
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M)...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction...
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe(s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn(aq) +2Cr(s) →2Cr" (aq) +35n²+ (aq)
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) +...
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) + 2e- Fe () -0.440 Fe3+ (aq) + e- → Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. Cr (s) + 3Fe3+ (aq) + 3Fe2+ (aq) + Cr3+ (aq) A) -1.45 B) +2.99 C) +1.51 D) +3.05 E) +1.57
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard...
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
Use the following half-reactions to write 3 spontaneous
reactions, calculate E°cell for each reaction, what is
the n number (number of electrons transferred).
Au+ (aq) + e− → Au
(s) E° = 1.69
V
N2O (g) + 2H+ (aq) + 2 e− →
N2 (g) + H2O (l) E° =
1.77 V
Cr3+ (aq) + 3 e− → Cr
(s) E° = -0.74 V
Question 7 0.36 pts Use the following half-reactions to write 3 spontaneous reactions, calculate Eºcell for...
What is the E cell for the cell represented by the combination of the following half- reactions? 2Hg2+(aq) + 2e" =Hg22+(aq); E°= 0.92 V Cr3+ (aq) + 3e Cr(s); E°= -0.74 V O 1) -0.18 V O2) 0.18 V 03) 1.28 V 4) 1.66 V 05) 2.12 V
A voltaic cell is based on the following half reactions at 25°C: Ag + e- → Ag E = 0.8V H2O2 + 2H+ + 2e - → 2H20 E° = 1.78V Predict whether E cell is larger or smaller than Eºcel for the following cases. (a) (Ag +) = 1.0 M, (H2O2) = 2.0 M, [H*] = 2.0 M (b) (Ag +) - 2.0 M, (H2O2) = 1.0 M, [H) - 1.0 x 10'M
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)
2. Using the information provided, calculate the standard cell potential, Eºcell, for the reaction below: Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe(s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn(aq) +2Cr(s) →2Cr" (aq) +35n²+ (aq)
Table 20.2 Half-reaction E° (V) Cr3+ (aq) + 3e- → Cr (s) -0.74 Fe2+ (aq) + 2e- Fe () -0.440 Fe3+ (aq) + e- → Fe2+ (s) +0.771 Sn4+ (aq) + 2e- Sn2+ (aq) +0.154 The standard cell potential (Eºcell) for the voltaic cell based on the reaction below is V. Cr (s) + 3Fe3+ (aq) + 3Fe2+ (aq) + Cr3+ (aq) A) -1.45 B) +2.99 C) +1.51 D) +3.05 E) +1.57
Use the half-reactions below to produce a voltaic cell with the given standard cell potential. Standard Cell Potential Co- (aq) + e-Cot (aq) E = +1.82 V 1.53 V 2H(aq) + 2e-H2(g) E = +0.00 V Pb2+ (aq) + 2e-Pb(s) E = -0.13 V Fe (aq) + e-Fel+ (aq) E = +0.77 V Ag (aq) + e-Ag(s) E = +0.80 V Sn* (aq) + 2e Sne (aq) 20.13 V Cu- (aq) + e- Cu(aq) E = +0.15 V Zn²+ (aq)...
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