Calculate the cell potential difference, Eºcell (Ecell = Eºcathode - Eanode), given the standard reduction potential...
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?
nF 30. The standard cell potential (Ecell) of the reaction below is +0.126 V. The value of AG° for the reaction is kJ/mol. Pb2+ (aq)+ H2 (g) Pb (s)2H (aq) E) -50.8 D)+12.6 C)-12.6 B) +24.3 A) -24.3
Calculate Ecell for the following electrochemical cell at 25 degreeC Pt(s) | H2(g, 1.00 atm) | H+ (aq, 1.00 M) || Pb2+(aq, 0.150 M) | Pb(s) given the following standard reduction potentials. Pb2+(aq) + 2 e– --> Pb(s) Edegree = –0.126 V 2 H+ (aq) + 2 e– --> H2(g) Edegree = 0.000 V (Please show the steps)
please help the standrad reduction provided down What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cu2+ concentration is 9.24x10 + M and the Cr3+ concentration is 1.47 M? 3Cu2+ (aq) + 2Cr(s) Answer: 3Cu(s) + 2Cr +(aq) v The cell reaction as written above is spontaneous for the concentrations given: What is the calculated value of the cell potential at 298K for an electrochemical cell with the...
Given the measured cell potential, Ecell, is-0.3583 V at 25 °C in the following cell, calculate the Ht concentration Pt (s)|H2lg, 0.795 atm)lH (aq, ? M)l|Cd2 (aq, 1.00 M)|Cd (s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are as follows. 2H+(aq) + 2e- H2(g) E0.00 V E-0.403 V ? 2 + Number H0.21
The standard reduction potential of the Pb2+|Pb electrode is –0.13 V and the standard potential of the cell Zn(s) | Zn2+(aq) || Pb2+(aq) | Pb(s) is +0.63 V. What is the standard reduction potential of the Zn2+|Zn electrode? Question 9 options: –0.76 V –1.52 V +0.76 V –0.50 V +0.50 V
12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction written, under standard conditions at 25°C? Eºcell = Eºcathode -Eanode a. Zn2+(aq) + 2Fe2+(aq) → Zn(s) + 2Fe+(aq) b. Ni2+(aq) + Pd(s) - Ni(s) + Pd" (aq)
For the cell shown, the measured cell potential, Ecell is -0.3605 V at 25℃.Pt(s)|H₂(g, 0.881 atm)| H⁺(aq, ? M) || Cd²⁺(aq, 1.00 M) | Cd(s)The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are2 H⁺(aq)+2e- ⟶ H₂(g) E⁰=0.00 VCd²⁺(aq)+2e- ⟶ Cd(s) E⁰=-0.403 VCalculate the H⁺concentration.
For the cell shown, the measured cell potential, Ecell is -0.3719 V at 25℃.Pt(s)|H₂(g, 0.865 atm)| H⁺(aq, ? M) || Cd²⁺(aq, 1.00 M) | Cd(s)The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are2 H⁺(aq)+2e- ⟶ H₂(g) E⁰=0.00 VCd²⁺(aq)+2e- ⟶ Cd(s) E⁰=-0.403 VCalculate the H⁺concentration.
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)