Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to Cd(s) Cd(s) . Cd 2 +(aq)+2 e − ⟶Cd(s) ? ∘ Cd 2+ /Cd =−0.403 V Cd2+(aq)+2e−⟶Cd(s)ECd2+/Cd∘=−0.403 V Calculate the potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0560 M 0.0560 M solution of CdBr 2 . CdBr2. ? Cd = ECd= V V Calculate the potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0330 M NaOH 0.0330 M NaOH solution that is saturated with Cd (OH) 2 . Cd(OH)2. The ? sp Ksp for Cd (OH) 2 Cd(OH)2 is 7.2× 10 −15 . 7.2×10−15. ? Cd = ECd= V V Calculate the potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0200 M Cd ( NH 3 ) 2+ 4 0.0200 M Cd(NH3)42+ and 0.125 M NH 3 0.125 M NH3 solution. The ? 4 β4 for Cd ( NH 3 ) 2+ 4 Cd(NH3)42+ is 3.63× 10 6 . 3.63×106. ? Cd = ECd= V
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Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to Cd(s) Cd(s) . Cd 2...
Two standard reduction potentials are given below. Cd2+(aq) + 2 e− → Cd(s) E⁰red = −0.403 V Al3+(aq) + 3 e− → Al(s) E⁰red = −1.662 V There is only ONE submission for each part. (a) Which is a stronger reducing agent, Cd(s) or Al(s)? Cd(s) Al(s) (b) Which is the most difficult to oxidize, Cd(s) or Al(s)? Cd(s) Al(s) (c) Is Cd(s) able to reduce Al3+(aq) in a spontaneous reaction? is able is not able (d) Is Al(s) able...
Cd2+(aq) + 2 e-←→ Cd (s) Cu (aq) + eCu (s) Ag+(aq) + e-←→ Ag (s) E'=-0.41 V E +0.52 V E +0.80 v 3. Based on the standard electrode potentials given above, which of the following is the stron reducing agent (reducer)? a. Cd(s) b. Cd (aq) c. Cu(s) d. Ag(s) e. Ag'(aq)
HIU Blud cell potential of a galvanic cell based on the following reduction half- reactions at 25 °C Cd + 2e → Cd Eº - -0.403 V Pb2+2e → Pb Eº - -0.126 V where (Cd-) - 0.040 M and (Pb) - 0.400M (13.) A zinc electrode is submerged in an acidic 0.40 M Zn?' solution which is connected by a salt bridge to a 1.50 M Ag' solution containing a silver electrode. Determine the initial voltage of the cell...
What is the concentration of Cd(OH)2(aq) in a solution in which the concentrations of Cd2+ and OH− are fixed at 3.3×10^−5 M? The cumulative formation constant (β2) for Cd(OH)2(aq) in water is 5.0×10^7 [Cd(OH)2]= M
A voltaic cell consists of an Al/Al3+ half-cell and a Cd/Cd2+ half-cell. Calculate {Cd2+} when {Al3+} = 0.306 M and Ecell = 1.27 V. Use reduction potential values of Al3+ = -1.66 V and for Cd2+ = -0.40 V.
Be sure to answer all parts. Consider the following reaction: Cd(s) + Fe2+(aq) → Cd2+(aq) + Fe(s) E o (Fe2+ / Fe) = −0.4400 V, E o (Cd2+ / Cd) = −0.4000 V Calculate the emf for this reaction at 298 K if [Fe2+] = 0.60 M and [Cd2+] = 0.010 M. E =____ V Will the reaction occur spontaneously at these conditions? yes no cannot predict
For the cell shown, the measured cell potential, Ecell, is -0.3629 V at 25 °C. Pt(s) | H,(g, 0.707 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M)| Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e - H (9) E° = 0.00 V Cd2+ (aq) + 2e — Cd(s) E' = -0.403 V Calculate the H+ concentration. M = 0.031 Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3709 V at 25 °C. Pt(s) | H,(g, 0.877 atm) | H+ (aq,? M) || Cd2+ (aq, 1.00 M) Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e H (9) E' = 0.00 V Cd2+ (aq) + 2e - Cd(s) E' = -0.403 V Calculate the H concentration. [HT] = M
For the cell shown, the measured cell potential, Ecell, is -0.3687 V at 25 °C. Pt(s) | H, (8,0.873 atm) | H+ (aq, ? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2e → H, (g) E° = 0.00 v Cd2+ (aq) + 2e- Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+) = .0588 M Incorrect
For the cell shown, the measured cell potential, Ecell, is -0.3711 V at 25 °C Pt(s) H2(g, 0.865 atm) | Ht (aq,? M) || Cd2+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H"(aq) + 2е — H2(g) Eo = 0.00 V Cd2+(aq)2 e - Cd(s) Eo =-0.403 V Calculate the Ht concentration М