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An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+...
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
An electrochemical cell is based on the following two half-reactions:oxidation: Sn(s)→Sn2+(aq,1.60 M) +2e-reduction: ClO2(g, 0.130 atm )+e−→ClO2-(aq, 1.55 MM )Compute the cell potential at 25°C
A voltaic cell employs the following redox reaction: 2 Fe3+ (aq) + 3 Mg(s) + 2 Fe (s) + 3 Mg2+ (aq) Calculate the cell potential at 25 °C under each of the following conditions. Part B You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. [Fe3+] = 2.5x10-3 M ; [Mg2+] = 2.85 M Express your answer in units of volts. ΟΙ ΑΣΦ ? Ecell V Submit Request Answer Part C [Fe3+] =...
An electrochemical cell based on the following reaction has astandard cell voltage (Eocell) of 0.48 V Sn (s) + Cu2+ (aq) ---> Sn2+ (aq) + Cu (s) What is the standard reduction potential of tin? Sn2+ (aq) +2e- ---> Sn(s) a. -0.14 V b. 0.14 V c. -0.82 V d. 0.82 V e. none of the above
A voltaic cell is based on the following two half-reactions: Cd2 (ag) +2e-> Cd (s) Sn2(aq)+ 2e Sn (s) Calculate the standard cell potential. Use the date from the attached table.SRP2.docx Oa 0.13 Ob 042 Oc.027 Od-0.27
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. You may want to reference (Pages 865 - 869) Section 19.6 while completing this problem. Part A standard conditions Express your answer in units of volts. Ecell = V Part B [Fe3+]= 1.2×10−3 M ; [Mg2+]= 1.70 M Express your answer in units of volts. Ecell = V SubmitRequest Answer Part C [Fe3+]= 1.70 M ; [Mg2+]=1.2×10−3 M...
Consider the following electrochemical cell shown below. Sn(s)|Sn2 (aq, 0.0155 M)lIAg (aq, 3.50 M)IAg(s) Based on this cell write the net cell equation. Phases are optional. Do not include the concentrations. Calculate the following values at 25 °C using standard potentials as needed. Number cell Number cell
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.
An electrochemical cell is set up with the following two half-reactions: Oxidation half-reaction: 31- (aq) 213(aq) +2 e Reduction half-reaction: 13(aq) + 2 e 221 (aq) At 298 K, the overall reaction is as follows and has the given standard cell potential: 12 (aq) + (aq) 13 (aq) & cell = 0.014 V Rank the following conditions for the above reaction from the one producing the highest (most positive) voltage to the one producing the lowest (least positive or most...
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...