Question

In: Chemistry

a) Calculate the cell potential at 25°C for the cell Fe(s) I (Fe2+ (0.100 M) II...

a) Calculate the cell potential at 25°C for the cell

Fe(s) I (Fe2+ (0.100 M) II Pd2+ (1.0 × 10-5 M) I Pd(s)

given that the standard reduction potential for Fe2+/Fe is -0.45 V and for Pd2+/Pd is +0.95 V. - Please show the steps

b) Based on the half-reactions and their respective standard reduction potentials below, the strongest reducing agent is ________, and the strongest oxidizing agent is ________.

      Ag+ (aq) + e- → Ag(s)            0.80 V

            2 H+ (aq) + 2 e- → H2 (g)       0.00 V

            Cd2+ (aq) + 2 e- → Cd(s)        -0.40 V

The answer is

Cd, Ag+

Can you please explain to me why this is the right answer.

Solutions

Expert Solution


Related Solutions

Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for...
Co(s) → Co2+(aq) + 2e Fe2+(aq) + 2e-→ Fe(s) b) Calculate the standard cell potential for this voltaic cell. c) Calculate the cell potential for this voltaic cell at 298 K if it is constructed using solutions of 0.14 M Co(NO3)2 and 0.27 M Fe(NO3)2. d) When looking at the magnitude of this potential, what can be concluded about the electrochemical cell?
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 89 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.110 M . Part A: What is the value for the reaction quotient, Q, for the cell? Part B: What is the value for the temperature, T, in kelvins? Part C: What is the value for n? Part D: Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 73 ∘C , where [Fe2+]= 3.70 M and [Mg2+]= 0.310 M...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 73 ∘C , where [Fe2+]= 3.70 M and [Mg2+]= 0.310 M . What is the value for the reaction quotient, Q, for the cell? What is the value for the temperature, T, in kelvins? What is the value for n? Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s)
Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell =...
Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell = 1.21 V, calculate ?G? for the reaction. b.) If E?cell=1.21V, calculate the equilibrium constant for the reaction. c.) Use the Nernst equation to determine the potential for the cell: Fe(s)|Fe2+(aq,1.0�10-3M)||Fe3+(aq,1.0�10-3M),Fe2+(aq,0.10M)|Pt(s)
Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If...
Consider the following cell reaction: Fe(s) + 2 H+(? M) Fe2+(1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.236 volts, what is the pH of the hydrogen electrode? A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ()= 1atm) immersed in a solution of unknown [H+]. If the cell potential is 0.202 V, what is the pH of the unknown solution at 298...
Suppose you construct the following galvanic cell: Fe(s)|Fe2+(aq)||NAD+(aq)|NADH(aq) Fe2+ + 2e- → Fe Eo = -0.44V...
Suppose you construct the following galvanic cell: Fe(s)|Fe2+(aq)||NAD+(aq)|NADH(aq) Fe2+ + 2e- → Fe Eo = -0.44V NAD+ + 2e- + 2H+ → NADH + H+ Eo' = -0.320V (note the different standard states) A) Will the cell generate current at biochemical standard state? At chemical standard state? At T = 4 oC, pH = 7? At T = 97 oC, pH = 7? Justify your answers. B) How many protons can be moved across a membrane from pH 7.5 to...
A galvanic cell Fe(s)|Fe2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Fe electrode that weighs...
A galvanic cell Fe(s)|Fe2+(aq) || Pb2+(aq)|Pb(s) is constructed using a completely immersed Fe electrode that weighs 35.6 g and a Pbelectrode immersed in 510 mL of 1.00 M Pb2+(aq) solution. A steady current of 0.0672 A is drawn from the cell as the electrons move from the Fe electrode to the Pb electrode. (a) Which reactant is the limiting reactant in this cell? Enter symbol (b) How long does it take for the cell to be completely discharged? -------- s...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
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. 1.) [Fe3+]= 1.1×10−3 M ; [Mg2+]= 2.60 M 2.) [Fe3+]= 2.60 M ; [Mg2+]= 1.1×10−3 M
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
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 a)[Fe3+]= 1.0×10−3 M ; [Mg2+]= 2.00 M b)[Fe3+]= 2.00 M ; [Mg2+]= 1.0×10−3 M
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
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. A) [Fe3+]= 1.9×10−3 M ; [Mg2+]= 2.80 M B) [Fe3+]= 2.80 M ; [Mg2+]= 1.9×10−3 M
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT