2. What is the potential for the following galvanic cell? Pb(s) PbF2(s) F(aq)||CI(aq)| AgCl(s)|Ag(s) The concentration...
6. Consider the following galvanic cell and standard reduction potentials: Ag Pb E° = 0.80 V salt bridge Ag+ (aq) + e → Ag(s) Pb2+(aq) + 2e → Pb(s) E° = -0.13 V 1 M Ag+ 1 M Pb2+ Which one of the following statements is TRUE? a) The cell on the left containing Ag+(aq) is the anode. b) The initial reading on the voltmeter would be 0.67 V. c) Oxidation occurs in the cell on the right containing Pb²+(aq)....
Consider a galvanic cell where one compartment has Br2 (aq) at a concentration of 0.50 M and Br ̄ at a concentration of 0.10 M with a platinum electrode and the second compartment has Cr3+ at a concentration of 0.20 M and a Cr electrode. Use the following reduction potentials to answer the questions: Cr3+ (aq) + e ̄→Cr(s) εo = - 0.73 V Br2(aq) + 2e ̄→2Br ̄ (aq) εo =1.09V a. What is the standard cell potential for...
5. Consider the galvanic cell, Pb(s) Pb(aq) || Cu(aq) Cu(s) What should be done to increase the cell potential (i.e., become more positive)? Be specific when stating which concentration should be increased or decreased. 6. Calculate the cell potential (Ecell) at 25°C for the cell Fe(s) / (Fe*(0.100 M) || Pd**(1.0 * 10M) | Pd(s) Given that the standard reduction potential for Fe* /Fe is -0.45 V and for Pd/Pd is +0.95 V. 8. Balance the following reduction-oxidation reaction in...
Calculate the standard cell potential (∆Eo) for the
galvanic cell:
Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
Separate galvanic cells are made from the following half-cells: cell 1: H+(aq)/H2(g) and Pb2+(aq)/Pb(s) cell 2: Fe2+(aq)/Fe(s) and Zn2+(aq)/Zn(s) Which of the following is correct for the working cells? Standard reduction potentials, 298 K, Aqueous Solution (pH = 0): Cl2(g) + 2e --> 2C1-(aq); E° = +1.36 V Fe3+(aq) + e --> Fe2+(aq); E° = +0.77 V Cu2+(aq) + 2e --> Cu(s); E° = +0.34 V 2H+(aq) + 2e --> H2(g); E° = 0.00 V Pb2+(aq) + 2e --> Pb(s);...
A12a The cell
Ag //AgCl (sat’d), KCl (1.00 M) //NiL2 (0.0250 M), NaL (0.150 M)
//Ni
has a voltage of -0.767 V. What is the overall formation constant
of NiL2?
Given:
AgCl(s) + e Ag(s) + Cl- Eo = +0.222 V Ni2+ + 2e Ni(s)
Eo = -0.257 V
A12b Consider the following standard reduction potential:
Ag+ + e Ag(s) Eo = +0.800 V AgI(s) + e Ag(s) + I- Eo = -0.164
V
Calculate the solubility constant, Ksp at...
A galvanic cell Pb│PbCl2│NaCl (0.0100M)││AgNO3 (0.500 M)│Ag is setup in the lab. Ksp PbCl2 = 87× 10-5. What is the concentration of Pb2+ in the Pb│PbCl2 half-cell? (10 pts.) Calculate Ecell. (20 pts.) E0 red=-0.13 Pb2+ + 2e- --> Pb E0 red= 0.80 Ag+ + e= -->Ag
What is the reduction half-reaction for the following overall galvanic cell reaction? Co2+(aq) + 2 Ag(s) → Co(s) + 2 Ag+(aq) Co2+(aq) + e-Co(s) Co2 (aq) 2 e Co(s) Ag (aq)eAg(s) Ag(s) + e-→ Ag+(aq)
An Ag-Cd electrochemical cell is written as Cd (s) CdCl2 (0.010 M) || AgCl (s) CI- (0.50 M) | Ag E°Cd2+/Ca = 0.403 V and EºACIJAg = 0.222 V 1. Write the half-cell reactions at anode and at cathode. 2. Which is oxidant and which is reductant? 3. Calculate the half-cell potentials at both anode and cathode. 4. Calculate the cell potential. 5. Write the whole-cell reaction. 6. Calculate the equilibrium constant for the whole-cell reaction. For the half –...
Calculate the cell potential for this voltaic cell at 25 °C: Cr(s) Cr3 (aq, 0.43 M) || Cl2 (g, 0.771 atm) CI(aq, 0.133 M), Pt(s) Cas Ze (bp) Cl2(g)+2e 2CI (aq) Cos (aq)+e Co (aq) Co (aq)+2e Co(s) Cr3 (aq)+3e2 Cr(s) Cr3 (aq)+e Cr2 (aq) Cr2 (aq)+ 2e 2Cr(s) +1.358 3+ +1.83 -0.28 -0.744 -0.407 -0.913 AH 0 3e Cr(0H)-(s) C.o 2-(aa)