he nonspontaneous E0cell for Zn I Zn2+ II Cu2+ I Cu is 1.103 V with the following data: Half-reactions E0(V) E0oxidation +0.763 E0reduction +0.340 True False
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14) The nonspontaneous E0cell for Zn I Zn2+ II Cu2+ I Cu is 1.103 V with the following data:
|
Half-reactions |
E0(V) |
|
E0oxidation |
+0.763 |
|
E0reduction |
+0.340 |
- True
- False
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- Given that ΔrG⦵ = −212.7 kJ mol−1 for the reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) in the Daniell cell at 25 °C, and b (CuSO4) = 1.00 × 10−3 mol kg−1 and b (ZnSO4) = 3.00 × 10−3 mol kg−1, calculate (a) the ionic strengths of the solutions, (b) the mean ionic activity coefficients in the compartments, (c) the reaction quotient, (d) the standard cell potential, and (e) the cell potential. (Take γ+ = γ− = γ± in the respective compartments. Use the Debye–Hückel limiting law.)For the reaction Zn(s) + Cu2+(aq) - 5 Zn2+(aq) + Cu(s), ∆G° at 25°C is -212,300 Jmol-1. Calculate the electromotive force E in volts for the cell Zn(s) | Zn2+(aq,a1) | | Cu2+ (aq,a2) | Cu(s) when the activities a1 and a2 are 0.01450 and 0.0880, respectively.The resistances of a series of aqueous NaCl solutions, formed by successive dilution of a sample, were measured in a cell with cell constant (the constant C in the relation κ = C/R) equal to 0.2063 cm-1 and the following values were found at 25oC: c/(mol dm−3) 0.00050 0.0010 0.0050 0.010 0.020 0.050 R/W 3314 1669 342.1 174.1 89.08 37.14 Find the molar conductance of NaCl at 25oC at infinite dilution from the graph.
- It is desired to assemble a concentration cell with a potential of 120 mV withtwo Zn(s) electrodes immersed, each one, in a ZnSO4 solution. What should be theratio between Zn2+ activities in the two electrodes to reach the desired potential?An ion selective electrode is utilised to determine the concentration of Ca2+ in the presence of Mg2+. The selectivity coefficient for the electrode kij is 0.015. If the concentrations of Ca2+ and Mg2+ are 50 and 500 ppm, respectively, calculate the change in potential (in mV) when the temperature of the measurement cell is increased from 20oC to 40oC.The following data were obtained with a cadmium-selective solid-state electrode. The ionic strength of each solution was 0.30 M, and the reference electrode was a saturated calomel electrode. Determine the concentration of the unknown cadmium ion in the sample. [Cd2+], M 1.00x10-1 8.75x10-3 1.00x10-3 3.16x10-5 3.16x10-6 Unknown E, V -0.115 -0.150 -0.175 -0.213 -0.242 -0.200
- Estimate the mean ionic activity for a 0.0155 molal solution of H3PO4 at 298 K. Assume complete dissociation. (Given A=0.0509) Is hydrogen a better reducing agent in acid or basic solution? Explain your answer.Quinone undergoes a reversible reduction at a dropping mercury electrode. The reaction is C6H4O2 (quinone) + 2H+ + 2 e- <> C6H4 (OH)2 (hydroxyquinone) E°=0.599 V. Assume that the diffusion coefficient for quinine and hydroxyquinone are approximately the same. Calculate the approximate half-wave potential (vs SCE, E=0.244 V) for reduction of hydroxyquinone at a rotating disk electrode from a solution buffered to a pH of 7.0Significant evolution or deposition occurs in electrolysis only if the overpotential exceeds about 0.6 V. To illustrate this criterion calculate the effect that increasing the overpotential from 0.40 V to 0.60 V has on the current density in the electrolysis of 1.0 m NaOH(aq), which is 1.0 mA cm−2 at 0.4 V and 25 °C. Take α = 0.5. Hint: Assume that the current is entirely anodic.
- The standard potentials of Pb2+|Pb and Sn2+|Sn are −126 mV and −136 mV respectively at 25 °C, and the overpotential for their deposition are close to zero. What should the relative concentrations of Pb2+(aq) and Sn2+(aq) be in order to ensure simultaneous deposition from a mixture? You may assume that activities can be approximated by molar concentrations.A 0.2g sample of toothpaste containing fluoride was treated with 50 cm3 of a suitable buffer solution and diluted to 100 cm3. Using a fluoride ion-selective electrode, a 25.00 cm3 aliquot of this solution gave cell potentials of –155.3 mV before and –176.2 mV after spiking with 0.1 cm3 of a 0.5 mg/cm3 fluoride standard. Calculate the pF– corresponding to each cell potential and the percentage by weight of fluoride in the toothpaste.Use the shorthand notation to describe a cell consisting of a saturated calomel reference electrode and a silver indicator electrode for the measurement of (a) pSCN. (b) pI. (c) pSO3 (d) pPO. Then, generate an equation that relates pAnion to Ecell for each of the cells. (For Ag2SO3 Ksp = 1.5 * 10-14; for Ag3PO4, K,p = 1.3 *10-20 ).