6. In class we went through a semi-empirical derivation of the i(t)-Eappi Curve expected in a voltammetry experiment involving a reversible redox reaction, 0.0592, -log- 0.0592, Flog mo. m (t) – i(t)) i(t) Eapol E mR Eq. 2-1 Show how to rearrange Eq. 2-1 to yield an expression to calculate the current i(t) for a particular Egppl value, i(1) = f(E appl ) -
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- Complete and balance the following half-reaction in basic solution. Be sure to include the proper phases for all species within the reaction. Zn(s) → Zn(OH)4² (aq) 1 + 2 e Reset H₂O ñ 02 03 3 4 ( ) 0²- OH 5 U 05 H+ ☐²+ Ï 3+ 7 8 H3O+ OH- 4+ • x H₂O 9 0 (s) (1) (g) (aq) 口口。 H Zn DeleteCalculate Ecell in V at 25°C for the redox reaction indicated by the following line notation. Pt(s) | H: (1.5 atm) | H" (0.50M) || Ag* (2.0M) | Ag(s) 5 6 Half Reaction Ag* laa) s + Ag () +0.799 2H* (alt e H2 le) 7 8 +/- x 100 3. 2. 1, 4.J R = 8.314 mol·K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H"(aq) + 4 e 2 H20 (1) 1.229 |Z2 (s) + 2 e → 2Z° (aq) 0.426 3+ (aq) + 3 е A' → A (s) 0.292 2 H20 (I) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 G2+ (aq) + 2 e G (s) - 1.245 (aq) + 2 e¯ → M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 MMZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 11 The electrode connected to the red wire (negative terminal on the battery) will... o produce bubbles and the pH will increase. o produce M (s) on the electrode and the pH will not change. o produce bubbles and the pH will decrease. o produce M (s) on the electrode and the pH will decrease. Question 12 The electrode…
- AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.6D.4 The potential of the cell Pt(s)|H,(g,p®)[HCI(aq,b)|Hg,Cl,(s)|Hg(1) has been measured with high precision with the following results at 25°C: b/(mmolkg") 1.6077 5.0403 3.0769 7.6938 10.9474 E/V 0.600 80 0.568 25 0.543 66 0.522 67 0.505 32 Determine the standard cell potential and the mean activity coefficient of HCI at these molalities. (Make a least-squares fit of the data to the best straight line.)Chem101 b My Questions | bartleby à app.101edu.co Question 14 of 20 * What is E° for the cell Mn | Mn2*(aq) || Ag*(aq) | Ag? Standard Reduction E° (V) Potentials | v Ag+(aq) + e Ag(s) +0.80 1 Mn2+(aq) + 2e- Mn(s) -1.18 7 8 +/- MacBook Pro
- 3) Which reaction occurs at a saturated calomel electrode (SCE) a) H* (aq) + e- ---------> ½/2 H2 (g) b) AgCl (s) + e- ----------> Ag (s) + Cl- (aq) c) Fe³+ (aq) + e -----------> Fe²+ (s) d) CuCl2 (s) + 2e --------> 2 Cu (s) + 2 Cl(aq) e) Hg2Cl2 (s) + 2e --------> 2 Hg (1) + 2 Cl (aq)The E°cell = 0.135 V for the reaction %3D 312(s) + 5Cr20,2(aq) + 34H*(aq) → 6103 (aq) + 10Cr³+(aq) + 17H2O What is Ecell if [Cr2072] = 0.044 M, [H*] = 0.16 M, [IO3] = 0.00016 M, and [Cr3*] = 0.0041 M? Ecell = i VPt|H; (1.6 atm)|H (0.80 M) || C,Hs O2 (0.20 M), AgC,HO2 (s)|Ag The cathode is essentially a silver electrode, Ag+ (ag)|Ag. However, the cathode solution is saturated with silver acetate, so that the silver-ion concentration is determined by the solubility product of AgC, H, O, (K, = 2.0 x 10). Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half Reaction Standard Potential, E (V) 2H* (ag) + 2e H2 (9) 0.00 Ag* (ag) +e Ag(s) 0.80 Cell potential
- Consider the following half-reactions: Half-reaction I(s) + 2e" NP*(aq) + 2e" - AP*(aq) + 3e - E° (V) - 21 (aq) 0.535V Ni(s) |-0.250V - Al(s) |-1.660V (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 L(s) oxidize Al(s) to AF* (aq)? ( (6) Which species can be oxidized by Ni*(aq)? If none, leave box blank.What is the schematic representation of a cell with a saturated calomel electrode as the reference electrode and a silver indicator electrode to measure the p-function of [CrO4²-]? SCE | Ag2CrO4(sat'd), CrO42-(x M)| Ag O SCE || Ag2 CrO4(s), CrO4²-(x M)| Ag SCE ||Ag2 CrO4(sat'd), CrO4²-(x M) | Ag SCE || Ag2CrO4(s), CrO4²-(x M) | AgWrite the Nernst equations for the variation of half-cell potentials with activities of species in the following half-cells: (a) Cr₂O,2-, Cr³+ | Pt; (b) saturated calomel electrode; (c) quinone, hydroquinone | Pt; (d) H* | CH4, CO₂, Pt.