Which of the following reactions will NOT occur spontaneously?

Q: Predict the expected sign of ΔS for the following reactions:   Ca(OH)2(s)    Ca2+(aq) + 2 OH-(aq)…

A: Since, you have asked multiple questions, we will solve the first question for you.  Question-1 : In…

Q: Enzo Ferrari is trying to determine the equilibrium constant for the balanced redox reaction between…

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Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) – Zn2*(aq) + Cu(s) the ion concentrations are [Cu2*]…

A: Given reaction is :  Zn (s) + Cu2+ (aq) --------> Zn2+ (aq) + Cu (s)  [Cu2+] = 0.0234 M  [Zn2+] =…

Q: Iron concentrations greater than 5.4 x 10–6 M in water used for laundry purposes can cause staining.…

A: The solubility product is a type of equilibrium constant whose value is temperature dependent.…

Q: 5.) Given the half reactions Cu²*(aq) + 2e → Cu (s) E°red = 0.34 V Pb?* (аq) + 2 е Pb (s) Е ed 3…

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Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) – Zn2-(aq) + Cu(s) the ion concentrations are [Cu2*]…

A: Th Ecell of the cell reaction can be calculated by using Nernst equation as follows -

Q: Calculate A,G and the equilibrium constant for the following reactions at 298 K. Zn?+ (aq) + Cd(s) 2…

A: Given temperature = 298 °K R = 8.314 J/mol-K

Q: Given the standard electrode potentials, which of these is spontaneous? Ag+(aq) + e- ⇌ Ag(s)…

A: In a galvanic cell, reaction is spontaneous when ΔG° is negative. This is the opposite of the cell…

Q: Calculate E° that would be developed by the cells using the following reactions (all concentrations…

A: The cell potential is calculated by the reduction potential of the electrode. If we know the…

Q: Calculate AG° for the following reaction at 315 K. At equilibrium, [HAIOs] = 0.73 M and [10,] = 0.08…

A: Given- [H4IO6] = 0.73 M [IO4-] = 0.08 M T = 315 K   To find- ∆Go   Formula- ∆Go = -RTlnK

Q: 12. If A,G° for the following reaction is -22.2 kJ/mol-rxn, calculate Ecell- Cu²"(aq) + 2 Ag(s) + 2…

A: In order to determine the cell potential (standard) first figure out the number of electrons that…

Q: Use the standard reduction potenitalto calculate equilibrium constantsfor the following reaction.…

A: The reactions given are 1) H2 (g) ------> 2 H+ (aq) + 2 e-…

Q: For the following half reactions AlF63-(aq) + 3e- = Al(s)+6F-(aq)  e°=-2.07V Al3+(aq) + 3e- =…

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Q: There are the following two cells: I. Ag; Ag* (M=1) // Cu** (M= 1); Cu Cu; Cu** (M= 1) // Ag* (M=1);…

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Q: Starting with the standard free energies of formation from the following table, calculate the values…

A: Given,

Q: Mn02(s) + 4 Hag) + 2 Brīag) → Mntaq) + Br21) + 2H20) At what pH is the voltage zero if all other…

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Q: What is the value of K for this aqueous reaction at 298 K? A +B=C+ D AG = 17.70 kJ/mol %3D

A: The relationship between standard Gibbs energy change (∆G°) , temperature (T) and equilibrium…

Q: For a solution in which u = 8.0 X 102, calculate Kp for *(a) AGSCN. (b) Pbl2. "(c) La(IO3)3. (d)…

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Q: of 2 escribe the relationship between the values of AG, Ksp, and the direction that a reaction will…

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Q: Based on the standard Gibbs energies of formation, which of the following reaction: represent a…

A: A reaction is feasible if ∆G° is negative.

Q: In cell reaction: Fe3+ + e- - Fe2+ both Fe3+ and Fe2+ are called anions

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Q: 8. The standard electrode potentials are: 9°(Sn²*/Sn) = -0.137 5 V, q®(Fe*"/Fe") = 0.771 V, qº…

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Q: constant

A: The first step is to calculate the standard potential for the overall reaction. It can be done by…

Q: For a particular reaction, AH = -111.4 kJ and AS = -25.0 J/K. Calculate AG for this reaction at 298…

A: Given data set: For a particular reaction, ∆H= -111.4 KJ ∆S= -25.0 J/K We need to calculate the…

Q: The following reaction has an Eo value of -0.76 V: H2(g) + Zn2+(aq)----->Zn(s) + 2H+(aq) a.…

A: It is given that the E°cell is -0.76 V for the reaction shown below, H2(g) + Zn2+(aq)→Zn(s) +…

Q: b. Calculate the equilibrium constant, K, at 298 K for the reaction using AG° = -RT In K. 4 Ag(s) +…

A: Spontaneous reactions always possess -ve free energy (dGo) and +ve cell potential. For such…

Q: What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell…

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Q: A solution containing an unknown cation reacts spontaneously with both zinc (ɛ°ox = +0.76 V) and…

A: For a spontaneous reaction the emf of the  cell is positive.

Q: Calculate AG for the reaction given below at pH 7.4 and 25 •C, where the concentrations of Acetyl…

A: Given that [Acetyl phosphate] = 5.0 mM = 5.0 × 10–3 M [Acetate] = 0.1 mM = 0.1 × 10–3 M [Pi] = 35 mM…

Q: In a certain zinc-copper cell, Zn(s) + Cu²*(aq) → Zn²*(aq) + Cu(s) the ion concentrations are [Cu²*]…

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Q: Consider the precipitation reactions below:   Fe2+ + S2- --->  FeS Cu2+ + S2- ---> CuS Zn2+ +…

A: The value of ΔG0f of Fe2+, S2-, Cu2+ and Zn2+ is -78.90 kJ/mol, 85.8 kJ/mol, 65.49 kJ/mol and…

Q: Calculate Kp for iron(II) sulfide from the following data: FeS+2e Fe+ S?- E = -1.01 V Fe2+ +2e → Fe…

A: Ksp=5.5 * 10-20

Q: Calculate the Eocell for this reaction occurring under standard conditions: 2 H+ (aq)   +   Fe (s)…

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Q: Which of these is spontaneous? (Using E° cell)

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Q: 5.) Given the half reactions Cu²"(aq) + 2e → Cu (s) E°red = 0.34 V Pb2 (aq) +2 e → Pb (s) E'red =…

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Q: What is the value of the equilibrium constant at 25°C for the reaction between each of the…

A: Here we are required to find the equilibrium constant for the given electrochemical cell reaction.

Q: What is the cell diagram for the reaction: 2A9CI(s) + H2(g) → 2Ag(s) + 2H*(aq) + 2C1 (aq)…

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Q: Which one of the following reactions (as written) should proceed spontaneously under standard…

A: Cell potential is calculated as E°cell = E°cathode - E°anode And is E°cell is positive then the cell…

Q: For the redox reaction Sn2+ + 2Fe+ = Sn+ + 2FE2+, PianyFe) = 0.68V, %3D Saavysac) = 0.14V, is it…

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Q: [Revlew Topics] [References] Calculate the pH of the cathode compartment for the following reaction…

A: Given question is approached using Nerst equation.

Q: Calculate the value of E for each of the following reactions : a) Sn2+ (aq) +2 Ag+ - Sn4+ (aq) + 2…

A: The reactions given are, a) Sn2+ (aq) + 2 Ag+ (aq) ---------> Sn4+ (aq) + 2 Ag (s) b) Fe2+ (aq) +…

Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) –→ Zn²+(aq) + Cu(s) the ion concentrations are…

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Q: cell potential

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Q: or the following redox reaction calculate the Ecell and K at 298 K. 2Na+(aq) + Ca(s)→2Na(s) +…

A: The redox reactions involve simultaneous oxidation and reduction reactions. The electron transfer…

Q: What is the Nernst expression corresponding to the following half-reactions: Zn2+ + 2e- ⇌ Zn(s) Fe3+…

A: Since your question has multiple sub-parts, we will solve only first three sub-parts for you. If you…

Q: #62

A: The overall reaction is as:

Q: In a certain zinc-copper cell, Zn(s) + Cu2+(aq) → Zn2*(aq) + Cu(s) the ion concentrations are [Cu2+]…

A: Given,

Q: Fe? + 2e -> Fe Ag* + e -> Ag Ered- - 0.44 V Ered- 0.80 V 5. Given the following data: Fe* (aq) +…

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Q: O ELECTROCHEMISTRY = Understanding concentration cells 13/5 A certain metal M forms a soluble…

A: This question is solved by using the simple concept of electrochemistry which involves oxidation at…