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.
Homework Answers
without knowing the correct temperature the nernst equation can not be applied
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Consider an electrochemical cell based on the following
reaction: Zn(s) + 2H2O(l) + 2OH-(aq) ⇄ [Zn(OH)4]2-(aq)...
Consider an electrochemical cell with the following cell reaction; Zn(s)+ Cu (aq) Zn2 (aq)+ Cu(s) where...
Consider an electrochemical cell with the following cell reaction; Zn(s)+ Cu (aq) Zn2 (aq)+ Cu(s) where [Cu+2] 0.01, [Zn+9-0.1 M. What will be the e.mf?
6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard...
6. Consider the following electrochemical cell: Write electrode half-reactions and the cell reaction. Determine the standard emf E for this cell from standard potential data in the Data Section of your textbook. Calculate the standard Gibbs energy and the equilibrium constant for the cell reaction at 25°C. Write the Nernst equation for the cell and calculate its emf E given that the pressure of H:(g) p = 1 bar, the molality of HCI(aq) b = 0.01 mol kg.. and the...
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is...
Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized to Zn2+(aq)and a cathode where Cr3+(aq) is reduced to Cr2+(aq) at a platinum electrode . Assume all aqueous solutions have a concentration of 1 mol/L. Write the cell notation for an electrochemical cell consisting of an anode where H2(g) is oxidized to H+(aq) at a platinum electrode and a cathode where H+(aq) is reduced to H2(g) at a platinum electrode . Assume all...
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e
Classify the half‑reactions as reduction half‑reactions or oxidation half‑reactions. H2(g)⟶2H+(aq)+2e−H2(g)⟶2H+(aq)+2e− 12O2(g)+2H+(aq)+2e−⟶H2O(g)12O2(g)+2H+(aq)+2e−⟶H2O(g) Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e−Cd(s)+2OH−(aq)⟶Cd(OH)2(s)+2e− 2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq)2NiO(OH)(s)+2H2O(l)+2e−⟶2Ni(OH)2(s)+2OH−(aq) Fe(s)⟶Fe2+(aq)+2e−Fe(s)⟶Fe2+(aq)+2e− oxidation reduction reduction oxidation reduction
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq)...
(2 pts.) For the following electrochemical cell at 25°C: Zn(s) | Zn2+ (aq) || H+ (aq) | Pt,H2 (g) (P=1.00 atm) calculate DG° in kJ calculate Ecell for [H+] = 0.8 M and [Zn2+] = 0.5 M calculate K at 25°C
1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). A. If...
1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). A. If the concentration of Sn2+ in the cathode compartment is 1.30 M and the cell generates an emf of 0.25 V , what is the concentration of Pb2+ in the anode compartment? B. If the anode compartment contains [SO2−4]= 1.30 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4? 2. A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). A. What is the emf...
Part A Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2Li(s)+2H2O(l)→H2(g)+2OH−(aq)+2Li+(aq) Express your answer...
Part A Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2Li(s)+2H2O(l)→H2(g)+2OH−(aq)+2Li+(aq) Express your answer to three significant figures and include the appropriate units. Part B Is the reaction spontaneous?
Consider an electrochemical cell, starting with standard state conditions, based on the following reaction. 2 H*(aq)+...
Consider an electrochemical cell, starting with standard state conditions, based on the following reaction. 2 H*(aq)+ Cd(s) Cd2+(aq) H2g) Ecell 0.40v Which of the following actions would increase the measured cell potential? Reducing the [H'] in the hydrogen cell O Increasing the mass of the solid Cd electrode Reducing the Cdion concentration O Increasing the pressure of hydrogen gas in the hydrogen cell O None of these
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s)...
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s) | Tl+(aq, 0.50 mol L−1) || H+(aq, x mol L−1) | H2(g, 1 atm) | Pt(s) The concentration of H+ is unknown and the pressure of H2 is kept constant at 1 atm. The cell voltage is initially measured as 0.139 V, with the Pt | H2 | H+ half-cell acting as the cathode. (a) (6 marks) Write out the oxidation and reduction half...
Consider an electrochemical cell with the following cell reaction; Zn(s)+ Cu (aq) Zn2 (aq)+ Cu(s) where [Cu+2] 0.01, [Zn+9-0.1 M. What will be the e.mf?
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Consider an electrochemical cell, starting with standard state conditions, based on the following reaction. 2 H*(aq)+ Cd(s) Cd2+(aq) H2g) Ecell 0.40v Which of the following actions would increase the measured cell potential? Reducing the [H'] in the hydrogen cell O Increasing the mass of the solid Cd electrode Reducing the Cdion concentration O Increasing the pressure of hydrogen gas in the hydrogen cell O None of these
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