P6B.10 Fuel cells show promise as power sources for automobiles. Hydrogenand carbon monoxide have been investigated for use in fuel cells, so theirsolubilities, s, in molten salts are of interest. Their solubilities in a moltenNaNO,/KNO, mixture were found to fit the following expressions:768log(s,/molcm³bar")=-5.39-K980log(sco/molcm³bar)=-5.98-KCalculate the standard molar enthalpies of solution of the two gases at 570 K.

Given: Temperature, T = 570 K The expressions for their solubilities are given below, s is the…

Answered: P6B.10 Fuel cells show promise as power…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 38QRT

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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
The electromotive force of the cell Pb(s) PbSO4(s) Na2SO4.10H₂O(aq)|Hg2SO4(s) Hg() is 0.9647 V at 25 °C. The temperature coefficient is 1.74 x 10-4 V K-¹. What is the AH for the reaction in kJ mol-¹? Express your answer in four significant figures.
Part B Now, calculate the ArG for the same reaction, based on the Standard Gibbs Energies of formation: ArG NO= 87.6 kJ - mol ArGN3O4 = 99.8 k.J - mol A,G° = -75.4 k.J · mol Submit Prevlous Answeга Completed Part C Using two very different method to solve for A:G", your answers from part A and part B will be the same. Why? O The reaction is spontaneous under all conditions O Gibbs Energy is a state function O Gibbs Energy is independent of temperature O The reaction is at equilibrium under standard conditions
The value of pOH of HCI solution at 25 °C if cell potential of the cell is 1.6655 v 3+ Pt/ H2(g. 1.0 bar.)/ HCl(x M)// Au³+ (0.01 M)/Au, is.
Consider the cell Pt|H,(g) HCI(aq)|AgCl(s)JAg, for which the cell reaction is 2 AgCl(s) + H,(g) and a molality of HCI of 0.020 mol kg', Ecell = +0.4658 V. (i) Write the Nernst equation for the cell reaction. (ii) Calculate A,G for the cell reaction. (iii) → 2 Ag(s) + 2 HCI(aq). At 25 °C Assuming that the Debye-Hückel limiting law holds at this concentration, calculate E'(CI, AgCl, Ag).
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.
Calculate the standard cell potential at 25°C for the following cell reaction from standard free energies of formation: 2AI(:) + ЗHg2* (ад) —» 2AB (аq) + ЗHg() Standard Free Energy of Formation Ion AG; (kJ/mol) Al+ (ag) -485.0 Zn²+ (ag) -147.0 Co+ (aq) -54.4 Ni²+ (aq) -45.6 2+ (ag) -24.39 Cu²+ (aq) 65.52 Hg²+ (aq) 164.4 Fe?+ (ag) -78.87 V Standard cell potential =
Calculate the standard Gibbs energy change for the following reactions at 25oC: (a) C2H5OH(l) + O2(g) -> CH3COOH(l) ─+ H2O(l) (b) 2 CO2(g) -> 2 CO(g) + O2(g) Which of the above reactions, as written, is spontaneous at the standard state? Answer: [─ 362.1; +514.4]
5. The oxidation of ferrous iron (Fe2+) to ferric ion (Fe³+) by molecular oxygen can be described by the following reaction: 4Fe²+ (aq) + O₂(aq) + 4H*(aq) = 4Fe³+ (aq) + 2H₂O(l) (1) Using free energies of formation, calculate the equilibrium constant for this reaction at 25 deg C. (2) For a water in equilibrium with the atmosphere, a pH of 2.0, and a total soluble iron concentration of 1 mg/L, calculate the concentrations of Fe2+(aq) and Fe³+(aq).
5. Erina observed that the borax she uses to clean the house is only partially soluble with water. She found on the internet that borax is composed of sodium tetraborate (Na,B,0;(OH), • 8H,0) and wanted to analyze its solubility. The dissolution of borax is: Na,B,0;(OH), • 8H20(9 = 2 Na (aq) + B40;(OH), (aq) + 8 H20o A 50.0 mL saturated solution was prepared for the experiment. After filtering the solution, a 5.00 mL aliquot was transferred to a 25.0 mL Erlenmeyer flask and was titrated using pre-standardized 0.4320 M HCI. The endpoint was reached after the addition of 4.73 mL titrant. Since the tetraborate anion (B,0;(OH),?) is a weak base, the tetraborate ion reacts with HCI by the reaction: B,0,(OH), (aq) + 2 H*(aq) + 3 H,0g = 4 H;BO3(aq) a. Write the K, expression for the dissolution process.
13.38 For the cell at 25°C and 1 bar Pt|Ag|AGCI(s)|HCI(aq)|Hg,Cl,(s)|Hg|Pt' (a) write the cell reaction; (b) use Table 13.1 to find the emf if the HCl molality is 0.100 mol/kg; (c) find the emf if the HCl mo- lality is 1.00 mol/kg. (d) For this cell, (8E/aT)p = 0.338 mV/K at 25°C and 1 bar. Find AG°, AH°, and ASº for the cell reaction at 25°C.
Consider the following half-reactions: Half-reaction E° (V) I2(s) + 2e → 21 (aq) 0.535V |2H (aq) + 2е — Н,(g)||0.000V Cr3+ (aд) + Зе- Cr(s)|-0.740V (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 Cr*(aq) oxidize I(aq) to I2(s)? (6) Which species can be oxidized by H*(aq)? If none, leave box blank.

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