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6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard...
Consider the following electrochemical cell at 298.15 K: Cd(s) | Cd(NO3)2 (aq, m = 0.200) ||...
Consider the following electrochemical cell at 298.15 K: Cd(s) | Cd(NO3)2 (aq, m = 0.200) || KCl (aq, m = 0.0150) | Ag(s) | AgCl(s) A) Write the overall reaction. B) Calculate the standard cell potential and ∆GR°. C) Calculate the cell potential and ∆GR assuming activity coefficients are 1.00. D) Calculate the cell potential and ∆GR using the Debye-Huckel limiting law for the mean ionic activity coefficients. E) Is the cell reaction spontaneous as written? F) How much electrochemical...
Write the half-reactions as they occur at each electrode and the net cell reaction for this...
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing copper and silver: Cu(s)|Cu2 (aq)||Ag (aq)|Ag(s) Anode? Cathode? Net cell reaction?
One electrode of a spontaneous electrochemical cell contains a piece of lead metal dipped into saturated...
One electrode of a spontaneous electrochemical cell contains a piece of lead metal dipped into saturated solution of PBSO4 in 1.00 M SO4. The other electrode is a standard hydrogen gas electrode. a) Draw and label all aspects of the electrochemical cell. b) Write the half reactions and the overall electrochemical reaction. c) Determine the emf (Ecell ) for the cell. 1.7 x 10% Ksp PbSO4 Pb (aq) 2 e Note: 2+ E -0.13 V Pb (s)
Write the half-reactions as they occur at each electrode and the net cell reaction for this...
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmiunm anode: In (aa)+3eInls) cathode: Cd (aq)+2e cals) net cell reaction:21n (aq+3Cdls)2lnls)+3cd (aq)
Write the half-reactions as they occur at each electrode and the net cell reaction for this...
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium: ln(s)|ln^3+ (aq)||Cd^2+ (aq)|Cd(s) anode: Ln rightarrow Ln^3+ + 3e^- cathode: Cd^2+ + 2e^- rightarrow Cd net cell reaction: 2ln + 3ed^2+ rightarrow 3ed + 2ln^3+
Consider the following cell at 25°C. Pt | Hg(l) | Hg2Clz(s) | HCl(aq,0.500 mol kgr) |...
Consider the following cell at 25°C. Pt | Hg(l) | Hg2Clz(s) | HCl(aq,0.500 mol kgr) | Cl2(g) | Pt (i) Write the appropriate reduction half-reactions for the system above.(4) (i) Write the Nemst equation for the cell reaction. (ii) Assuming that the Debye-Hückel Limiting Law holds at the given concentration, calculate the potential E for the cell. (iv) Calculate for the cell reaction.
Consider an electrochemical cell based on the following reaction: Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq)...
Consider an electrochemical cell based on the following reaction: Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq) + H2(g) All dissolved species are at 2.5 x 10-3 M; pressure of H2 is 1 bar (standard state) Use the Nernst equation to calculate E.
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M LiCl electrolyte solution, Pb electrode in a IM Pb(NOsh electrolyte solution. The standard half-cell reduction...
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M LiCl electrolyte solution, Pb electrode in a IM Pb(NOsh electrolyte solution. The standard half-cell reduction potentials are given below: Volts 3.05 0.13 Li+(aq) Li(s) 1e + → Write a balanced chemical equation representing the redox chemistry for this galvanic cell. Remember the reaction needs to be spontaneous. a.
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M...
For the following half reactions and the partially complete image for an electrochemical cell: Indicate the...
For the following half reactions and the partially complete image for an electrochemical cell: Indicate the direction of electron flow and then complete the cell diagram. bar Cl₂'g) . 4 . e Ci(m) Pt(s) Cl2(g) CI-(aq) Ni2+(aq) Ni(s) Ered/v 1.358 C12(g) + 2e → 201(aq) Ni2+ lag) + 2 → Ni(s) -0.257 electrochemical cell: am. -Ibar Claig) . > > SI cí (im) Eredly 1.358 ) -0.257
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) +...
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) + + OH (24) +1e UO2 (aq) +H2O Ered = -0.48 V Ti* (aq) + 1 e -Ti) Ered = -0.52 V a. Give the balanced net redox reaction in the spontaneous direction. (2 marks) b. What is Eºcell? (2 marks) c. In the working electrochemical cell applying the net redox reaction in the spontaneous direction under standard conditions of concentration, what material must the...
One electrode of a spontaneous electrochemical cell contains a piece of lead metal dipped into saturated solution of PBSO4 in 1.00 M SO4. The other electrode is a standard hydrogen gas electrode. a) Draw and label all aspects of the electrochemical cell. b) Write the half reactions and the overall electrochemical reaction. c) Determine the emf (Ecell ) for the cell. 1.7 x 10% Ksp PbSO4 Pb (aq) 2 e Note: 2+ E -0.13 V Pb (s)
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmiunm anode: In (aa)+3eInls) cathode: Cd (aq)+2e cals) net cell reaction:21n (aq+3Cdls)2lnls)+3cd (aq)
Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium: ln(s)|ln^3+ (aq)||Cd^2+ (aq)|Cd(s) anode: Ln rightarrow Ln^3+ + 3e^- cathode: Cd^2+ + 2e^- rightarrow Cd net cell reaction: 2ln + 3ed^2+ rightarrow 3ed + 2ln^3+
Consider the following cell at 25°C. Pt | Hg(l) | Hg2Clz(s) | HCl(aq,0.500 mol kgr) | Cl2(g) | Pt (i) Write the appropriate reduction half-reactions for the system above.(4) (i) Write the Nemst equation for the cell reaction. (ii) Assuming that the Debye-Hückel Limiting Law holds at the given concentration, calculate the potential E for the cell. (iv) Calculate for the cell reaction.
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M LiCl electrolyte solution, Pb electrode in a IM Pb(NOsh electrolyte solution. The standard half-cell reduction potentials are given below: Volts 3.05 0.13 Li+(aq) Li(s) 1e + → Write a balanced chemical equation representing the redox chemistry for this galvanic cell. Remember the reaction needs to be spontaneous. a.
1. A galvanic cell was composed from the following redox chemistry: Li electrode in a 1M...
For the following half reactions and the partially complete image for an electrochemical cell: Indicate the direction of electron flow and then complete the cell diagram. bar Cl₂'g) . 4 . e Ci(m) Pt(s) Cl2(g) CI-(aq) Ni2+(aq) Ni(s) Ered/v 1.358 C12(g) + 2e → 201(aq) Ni2+ lag) + 2 → Ni(s) -0.257 electrochemical cell: am. -Ibar Claig) . > > SI cí (im) Eredly 1.358 ) -0.257
2. An electrochemical cell is prepared to apply the following half reactions: HUO 3+ (aq) + + OH (24) +1e UO2 (aq) +H2O Ered = -0.48 V Ti* (aq) + 1 e -Ti) Ered = -0.52 V a. Give the balanced net redox reaction in the spontaneous direction. (2 marks) b. What is Eºcell? (2 marks) c. In the working electrochemical cell applying the net redox reaction in the spontaneous direction under standard conditions of concentration, what material must the...
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