Multi Consider a galvanic cell consisting of the following two redox Ag (0.010 M

Question

Multi Consider a galvanic cell consisting of the following two redox Ag (0.010 M) er Agos E +0.80 v no a. Write the equation for the halfreaction occurring at the Ag (0.010 M) Cra (0.010 M) b. Write the equation for the halfreaction occurring at the anode. c. Write the equation for the cell reaction. d. What is the standard cell potential, Eel, for the cel? e. Realizing the nonstandard concentrations, what i the actual cellpotential, Eau for the cell? See equation 32.6. Hint: What is the value of n in the Nernst equation? .6. The extent corrosion in the steel reinforcing rods (rebar) of concrete is measured by the galvanic cell shown in the of diagram of the instrument. The half-cell of the probe is usually a AgCI/Ag redox couple: AgCl e Ag +Cl (1.0 M) E- +0.23 V Multimeter Corrosion is said to be severe if the cell potential is measured at greater than 0.41 V. Under these conditions, what is the iron (II) concentration on the rebar? See equation 32.6. E -0.44 V AgCl+ e --Ag CT AgCl 364 Fe Fe2+ 2 e c the Nernst Equation cels,

Explanation / Answer

a) Ag(s) Ag+ + 1e-                                    Eored value = .80 V   

Reduction occurs at the cathode

b) Cr3+(aq) + 3e Cr                                       E0 = -0.74V oxidation at anode

c)   Cell reaction : 3Ag(s)+ Cr3+ 3Ag+ + Cr

d)   E0cell = E0(cathode) – E0(anode) = .80 V - (- 0.74 V   ) = 1.54 V

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