List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you...
List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you expect given electrochemical cell to be spontaneous or nonspontaneous? Explain your answer. Pb | Pb(NO3)2 | |Zn| Zn(NO3)2
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List the measured potential for Cell 3: Zn|Zn(NO3)2 ||
Pb(NO3)2|Pb. Based on your observations, do you...
EXPERIMENT 1: List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations,...
EXPERIMENT 1: List the measured potential for Cell 3: Zn|Zn(NO3)2 || Pb(NO3)2|Pb. Based on your observations, do you expect given electrochemical cell to be spontaneous or nonspontaneous? Explain your answer. Pb|Pb(NO3)2||Zn|Zn(NO3)2 EXPERIMENT 1: What would happen to the measured cell potentials if 30 mL solution was used in each half-cell instead of 25 mL? EXPERIMENT 1: Calculate the theoretical standard cell potential for the electrochemical cell that includes the reaction. Mn+Pb2+⟶Mn2++Pb The standard reduction potentials for each half reaction are...
data collected Cu(NO3)2 | Zn(NO3)2 = 0.999 V Pb | 1.0 M Pb(NO3)2 || 1.0 M...
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
thank you for your help! Based on the sign of the standard cell potential, Ecell, classify...
thank you for your help!
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Au (aq) + 3 Ag() — Au(s) + 3 Ag+ (aq) 1,(s) + Cu(s) -21"(aq) + Cu+ (aq) Zn2+ (aq) + Sn(s) - Zn(s) + Snº+ (aq) Answer Bank Incorrect Arrange these species by their ability to act as...
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb concentration is 1.04 M and the Zna* concentration is 9.44x10-M? Pb2+ (aq) + Zn(s) — Pb(s) + Zn²+ (aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Submit Answer
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or...
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Au + (aq) + 3 Ag(s) Au(s) + 3 Ag* (aq) 1,(s) + Cu() — 21(aq) + Cu2+ (aq) Ni2+ (aq) + Pb(s) Ni(s) + Pb2+ (aq)
What is the calculated value of the cell potential at 298K for an electrochemical cell with...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 1.38 M and the Zn2+ concentration is 9.41*10-4 M? Pb2+(aq) + Zn(s) —— Pb(s) + → Pb(s) + Zn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Based on the sign of the standard cell potential, Eco, classify these reactions as spontaneous or...
Based on the sign of the standard cell potential, Eco, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Spontaneous as written Nonspontaneous as written Au + (aq) + 3 Ag(s) + Au(s) + 3 Ag+ (aq) Ni²+ (aq) +52- (aq) Ni(s) +S(s) Pb2+ (aq) + H, (g) → Pb(s) + 2 H+ (aq) Answer Bank
A voltaic cell is based on two lead half cells: Pb+2(aq) + 2 e- → Pb(s)...
A voltaic cell is based on two lead half cells: Pb+2(aq) + 2 e- → Pb(s) Eo = -0.13 v One half-cell has [Pb(NO3)2] = 0.25 M and one half-cell has [Pb(NO3)2] = 0.0020 M What is the initial potential produced by the voltaic cell. Express your answer in units of volts with 2 significant digits, but do not include the units on the submitted answer.
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as...
During part B of your lab, you measured electrochemical cell potentials with a Cu2+/Cu couple as the anode. Predict the results you would observe if Ag+/Ag were the anode. half-cell predicted potential difference in V Cu2+/Cu Ag+/Ag Pb2+/Pb Zn2+/Zn
data collected
Cu(NO3)2 | Zn(NO3)2 = 0.999 V
Pb | 1.0 M Pb(NO3)2 || 1.0 M Zn(NO3)2 | Zn = 0.396 V
PART B: REDUCTION POTENTIALS 1. Report the measured cell potential for each galvanic cell and state which electrode corresponds to the cathode and which to the anode. 2. Given E = -0.76 V for the Zn/Zn half-cell, and your measured Ecell, calculate the reduction potential at the Cu and Pb electrodes and write the redox half- 6 reactions...
thank you for your help!
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Au (aq) + 3 Ag() — Au(s) + 3 Ag+ (aq) 1,(s) + Cu(s) -21"(aq) + Cu+ (aq) Zn2+ (aq) + Sn(s) - Zn(s) + Snº+ (aq) Answer Bank Incorrect Arrange these species by their ability to act as...
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb concentration is 1.04 M and the Zna* concentration is 9.44x10-M? Pb2+ (aq) + Zn(s) — Pb(s) + Zn²+ (aq) Answer: The cell reaction as written above is spontaneous for the concentrations given: Submit Answer
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Au + (aq) + 3 Ag(s) Au(s) + 3 Ag* (aq) 1,(s) + Cu() — 21(aq) + Cu2+ (aq) Ni2+ (aq) + Pb(s) Ni(s) + Pb2+ (aq)
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Pb2+ concentration is 1.38 M and the Zn2+ concentration is 9.41*10-4 M? Pb2+(aq) + Zn(s) —— Pb(s) + → Pb(s) + Zn2+(aq) Answer: V The cell reaction as written above is spontaneous for the concentrations given:
Based on the sign of the standard cell potential, Eco, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Spontaneous as written Nonspontaneous as written Au + (aq) + 3 Ag(s) + Au(s) + 3 Ag+ (aq) Ni²+ (aq) +52- (aq) Ni(s) +S(s) Pb2+ (aq) + H, (g) → Pb(s) + 2 H+ (aq) Answer Bank
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
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