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An electrochemical cell is set up with the following two half-reactions: Oxidation half-reaction: 31- (aq) 213(aq)...
An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+...
An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.70 M)+2e reduction: CIO2(g, 0.265 atm )+e+C10(aq, 2.00 M) You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Compute the cell potential at 25°C. Express the cell potential to three significant figures. ME PO ΑΣΦ ? Ecco V Submit Request Answer
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...
MISSED THIS? Read Section 20.6 (Page) An electrochemical cell is based on the following two half-reactions:...
MISSED THIS? Read Section 20.6 (Page) An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.80 M )+2e reduction: C1O2(g, 0.210 atm )+e- +C10] (aq, 1.70 M) Compute the cell potential at 25°C. Express the cell potential to three significant figures. ΤΕΙ ΑΣφ ? Ecell = .839 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Provide Feedback
please show all work. thank you 4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic...
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.26 M )+2e- Red:...
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.26 M )+2e- Red: MnO-4(aq, 1.50 M )+4H+(aq, 2.7 M )+3e-→MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C.
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │...
Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │ Pt(s) all gases 1 atm, all solutions 1.0 M a. Write the respective reduction half-reactions occurring on each side of the salt bridg, and from some reference, get the half-cell potential (in volts) for each. b. Determine what reaction occurs overall, and calculate the Eo cell for this electrochemical cell. c. Make a drawing of this cell, and label the ANODE and the CATHODE....
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the...
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the following half-reactions at equilibrium. In addition, determine ΔG° (in kJ mol-1 to two decimal places) for the reaction under standard conditions (i.e. all concentrations are 1.0 M) and predict the magnitude of K (e.g. very small, very large, etc.) E (o)0.34 V; E red) 0 9 = 1.68 V oxidation : Cu (s) → Cu2+ (aq, .010 M) + 2e- Reductin: MnO4 (aq, 2.0...
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?
Consider an electrochemical cell constructed from the following half cells, linked by an...
Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge.?• an Al(s) electrode in 1.0 M Al(NO3)3 solution? • a Pb(s) electrode in 1.0 M Pb(NO3)2 solution?The balanced overall (net) cell reaction isA. Pb(s) + Al3+(aq) ? Pb2+(aq) + Al(s).B. 3Pb(s) + 2Al3+(aq) ? 3Pb2+(aq) + 2Al(s).C. 3Pb2+(aq) + 2Al(s) ? 3Pb(s) + 2Al3+(aq).D. Pb2+(aq) + Al(s) ? Pb(s) + Al3+(aq).Can you explain and show steps of how to...
Draw a functioning electrochemical cell that uses any two of the following half reactions shown below....
Draw a functioning electrochemical cell that uses any two of the following half reactions shown below. Include a graphite electrode. Label the anode, cathode, direction of electron flow, direction of ALL ion/metals, and expected cell voltage. Write a balanced electrochemical reaction for your cell in neutral conditions).
An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.70 M)+2e reduction: CIO2(g, 0.265 atm )+e+C10(aq, 2.00 M) You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Compute the cell potential at 25°C. Express the cell potential to three significant figures. ME PO ΑΣΦ ? Ecco V Submit Request Answer
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...
MISSED THIS? Read Section 20.6 (Page) An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.80 M )+2e reduction: C1O2(g, 0.210 atm )+e- +C10] (aq, 1.70 M) Compute the cell potential at 25°C. Express the cell potential to three significant figures. ΤΕΙ ΑΣφ ? Ecell = .839 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Provide Feedback
please show all work. thank you
4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
19. Calculate EceLL (in V to two decimal places) for an electrochemical cell based on the following half-reactions at equilibrium. In addition, determine ΔG° (in kJ mol-1 to two decimal places) for the reaction under standard conditions (i.e. all concentrations are 1.0 M) and predict the magnitude of K (e.g. very small, very large, etc.) E (o)0.34 V; E red) 0 9 = 1.68 V oxidation : Cu (s) → Cu2+ (aq, .010 M) + 2e- Reductin: MnO4 (aq, 2.0...
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?
Draw a functioning electrochemical cell that uses any two of the following half reactions shown below. Include a graphite electrode. Label the anode, cathode, direction of electron flow, direction of ALL ion/metals, and expected cell voltage. Write a balanced electrochemical reaction for your cell in neutral conditions).
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