What is the standard cell potential of the following reactions
a. F2 + 2Cl- → 2F- + Cl2
b. 3Fe2+→ Fe(s) + 2 Fe3+
What is the standard cell potential of the following reactions a. F2 + 2Cl- → 2F-...
24) Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.) 26). 3 Cl2(8) +2 Fe(s) - 6 Cl(aq) + 2 Fe3+ (aq) 12(8)+2 e 2Cl(aq) E° 1.36 V 3C1tbe ! Fe3+(aq) + 3 e → Fe(s) 80036V 2Fe > 25€ Ep 3 + the A) 240 V B) 4.16V ) -1.32 V D) -1.40 V E) 1.32 V
Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical 3 C12(a) + 2 Fe(s) - 6 Cr(aq) + 2 Fe3+ (aq) Cl2(g) + 2 + 2 Cl(aq) Fe3+ (aq) + 36 - Fe(s) E' = +1.36 V E' = -0.04 V +1.40 V O-1.40 V 0 +4.16 V O +1.32 V O-1.32 V Submit Resvest Answer
What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2pressure is 2.71×10-4 atm, the F- concentration is 1.43M, and the Pb2+ concentration is 1.33M? F2(g) + Pb(s) ---> 2F-(aq) + Pb2+(aq) The cell reaction as written above is spontaneous for the concentrations given: True or False What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2pressure...
2. Calculate the standard cell emf (cell potential) for electrochemical cells having the following overall cell reactions and predict if they are spontaneous: a) Sn(s) + Pb2+ (aq) → Sn?" (aq) + Pb(s) Eºcell = Volts. Spontaneous? b) 2002 (aq) + Zn?"(aq) → 2Co3+ (aq) + Zn(s) Eºcell__volts; Spontaneous? c) Cl2(g) + 2Br (aq) + 2Cl(aq) + Br2(1); E° = volts; Spontaneous?
What is the standard cell potential for a voltaic cell with the following line notation? Al(s)[A1+ (aq)||Fe3+ (aq) Fe(s) Give your answer to 3 significant figures. Half Reaction Eredº (V) Al3+ + 3e- → AI -1.66 Fe3+ + 3e- → Fe +0.771 Numeric Answer
help with these please Consider the following half-reactions: Half-reaction Eo (V) F2(g)+ 2e 2F (aq) 2.870V Sn2 (aq) + 2e- Sn(s) 0.140V Cr3 (aq) + 3e° _ Cr(s)-0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will F2(g) oxidize Cr(s) to Cr3 (aq)? (6) Which species can be oxidized by Sn2 (aq)? If none, leave box blank. Consider the following half-reactions:...
What is the standard cell potential (Y) for the spontaneous voltaic cell formed from the given half-reactions? Reduction Half-Reaction Ered (V) Anode -0.41 Fe2+ (aq) + 2e Fe(s) Cl2 (8) +20 +2 (aq) Cathode 1.36
Question 7 Using the table of standard reduction potentials shown below, calculate the standard cell potential for a battery based on the following reactions. • Pet2 + 2e + Fe . 2 Li + 2 Li + 2e Reduction Half-Reaction F2 +2e + 2F MnO + 8H+ Se + Mn+2+ 4 H 0 Cl2 + 2e + 20 02 + 4H' + 4e + 2 H2O Ag+ e -- Ag Fet) + e + Fe2 O2 + 2 H2O +...
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
Calculate the equilibrium constant K for the reactions at 298 K. a) Br2(g) + 2Cl-(aq) ---> 2Br-(aq) + Cl2(g) b) A Galvanic Cell with the SHE and Fe+2/Fe(s)