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
An electrochemical cell is based on the following twohalf-reactions:oxidation: Sn(s)→Sn2+(aq,1.60 M) +2e-reduction: ClO2(g,...
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
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: 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.
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
יי Review 1 Constants l Periodic Table An electrochemical cell is based on these two half-reactions Ox: Sn(s) → Sn2+ (aq, 1.80 mol L i) + 2 e- Eanode-_0.14 (V) Red. CO2 (g, 0.110 bar) + e-→ Cio, (aq, 1.55 mol L i) E cathode = 0.95 (V) Part A Compute the cell potential at 25 C Express your answer to two decimal places and include the appropriate units
Selective Reduction The standard reduction potential for the half-reaction: Sn4+ + 2e - Sn2+ is +0.15 V. Consider data from the table of standard reduction potentials for common half-reactions, in your text. For a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. no yes yes yes yes yes Fe — Fe2+ + 2e- Sn2+ Sn4+ + 2e- Sn Sn2+...
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
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 Part A Part complete An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.017M)+2H+(aq,1.3M)+e−→→Ni2+(aq,2.5M)+2e−VO2+(aq,2.5M)+H2O(l) Calculate the cell potential under these nonstandard concentrations.
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
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...