Suppose that a hydrogen fuel cell, as described in the text, is to be operated at 75° C and atmospheric pressure. We wish to estimate the maximum electrical work done by the cell using, only the room-temperature data at the back of this book. It is convenient to first establish a zero-point for each of the three substances, H2 O2, and H20. Let us take G for both H2 and O2 to be zero at 25°C, so that G for a mole of H20 is -237 kJ at 25°C.(a) Using these conventions, estimate the Gibbs free energy of a mole of H2 at 75°C. Repeat for O2 and H20.(b) Using the results of part (a), calculate the maximum electrical work done by the cell at 75°C, for one mole of hydrogen fuel. Compare to the ideal performance of the cell at 25°C.

Q: Calculate e values for the galvanic cells based on the following overall reactions. Assume that all…

A: Given reactions are : (a). Cr3+ (aq) + Cl2 (g) <--------------> Cr2O72- (aq) + Cl- (aq)   (b).…

Q: What is the equilibrium constant K at 25 °C for an electrochemical cell when E° = +0.0205 V and n =…

A: The objective of the question is to calculate the equilibrium constant (K) for an electrochemical…

Q: Given that E = 1.88 V. calculate the standard Gibbs energy for the cell at 25 °C. O 538 kJ mol O…

A: Given: E°cell = 1.86 V

Q: For the following system predict whether the reaction would be spontaneous or non- spontaneous. A.…

A: Given cell reaction is : A cell at 27°C containing U | U3+ (0.01 M) || Mg2+ (3.4 M) | Mg Reaction is…

Q: Look at the electrochemical cell noted below , it has a KCl(aq) salt bridge: Zn(s) | ZnCl2(aq) ||…

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Q: Calculate the emf at 298 K generated by a voltaic cell in which the reaction isCr2O72-(aq)+ 14…

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Q: Consider the following reaction at 298K.Sn2+ (aq) + 2 Fe2+ (aq)  Sn (s) + 2 Fe3+ (aq)Which of the…

A: First, we need to determine whether the reaction is product-favored or reactant-favored. This can be…

Q: Calculate the standard free-energy change at 298K for the zinc-copper voltaic cell, which has a…

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Q: What is the maximum amount of work that is possible for an electrochemical cell where E = 1.82 V and…

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Q: 3. Consider when 0.025 M Cu2+ ions are used at the cathode and 0.750 M Fe2+ ions are used at the…

A: Given Reaction:-  Cu+2(aq) + Fe(s) -------> Fe+2(aq) + Cu(s) Reaction at Anode:- Fe(s)…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -7.4 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

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Q: The following reaction is spontaneous as written when the components are in their standard states:…

A: Answer:Galvanic cell is a type of cell that converts chemical energy into electrical energy via…

Q: Calculate quantity of charge and maximum work from a battery. The discharge reaction for a…

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Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -4.5 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

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Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -5.9 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

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Q: The standard EMF for the cell using the overall cell reaction below is +0.80 V: 2AI (s) + 312 (s) →…

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Q: The standard EMF for the cell using the overall cell reaction below is +0.57 V: 2AI (s) + 312 (s)…

A: Answer:Relation between standard Gibbs free energy change and standard cell potential will be used…

Q: A certain metal M forms a soluble sulfate salt M, (SO4), Suppose the left half cell of a galvanic…

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Q: What is the maximum amount of work that can be done by an electrochemical cell where E° = 2.23 V and…

A:

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -3.9 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: Given- ∆G°= -3.9kJ/mol = -3900 J/mole (1KJ = 1000J) n=3 F=96500 J/(V.mol)

Q: Consider the following reaction at 298K. 2+ Hg (aq) + H2(g) Hg(f) + 2H*(aq) The standard Gibbs free…

A: Hg2+ (aq)  +  H2(g)   →  Hg(l)  + 2H+ (aq)Oxidation half cellH2(g)   →2 H+(aq)+ 2 e-Reduction half…

Q: 4.19. What is the maximum amount of electrical (that is, non-pV) work that can be obtained by…

A:

Q: nitrate, Ni(NO3)2 undergoes electrolysis in order to plate on a sink faucet requiring 2.00 hours…

A: Given,  Time(t)  = 2.0 hrs = 7200 seconds  Current(i) = 2.80 amp Faraday's constant(F)  = 96, 485…

Q: What is the maximum amount of work that is possible for an electrochemical cell where E = 1.22 V and…

A: Work done = -nFE°cell

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -5.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: The objective of this question is to calculate the standard cell potential (E°) for a galvanic cell…

Q: At 125 °C, 1 mol O2 and 2 mol H₂ in a chamber have a total pressure of 3 atm. A current is run…

A: At constant temperature and volume, the pressure of a gas depends on the number of moles of the gas…

Q: Calculate the standard Gibbs free energy for the following reaction at 25 °C and 1 atm. Based on…

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Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -6.6 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: ∆G°= -6.6 kJ/mol = -6.6×103 J/mol n = 3 F = 96500 J/V.mol E°=?

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -6.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: Given,  ∆G° = -6.1 kJ/mol and n = 3. (F = 96,500 J/(V･mol) □G° = -nFE°

Q: ΔrG° for the reaction.

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Q: What is the equilibrium constant K at 25.0 °C for an electrochemical cell when E° = +0.120 V and n =…

A: Given,The standard cell potential ( Eo ) =+0.120 VNumber of moles of electrons (n) =2( F…

Q: Determine E° for a galvanic (voltaic) cell if ∆G° = -3.3 kJ/mol and n = 3. (F = 96,500 J/(V･mol))

A: The question is based on the concept of electrochemistry. we have to calculate standard reduction…

Q: If the equilibrium constant for a one-electron redox reaction at 298 KK is 8.3×1048.3×104, calculate…

A: Equilibrium constant of the reaction is 8.3×104. Temperature of the reaction is 298 K. ∆G˚rex can be…

Q: A student made measurements on some electrochemical cells and calculated three quantities: • The…

A: We know that,∆G0= -RTlnKWhereGibbs free energy change (ΔG0), the universal gas constant (R) ,…