Given the following data: Fe2+ + 2e-→Fe    Ered = -0.44 v, Ag+ + e- →Ag   Ered = 0.80 v Answer the following questions with respect to the reaction; Fe2+(aq) + 2 Ag(s) → Fe(s) + 2 Ag+(aq) (a) what is E for the reaction? (b) is the reaction spontaneous at standard state conditions? (c) what is the value of E at equilibrium? (d) what is the value of equilibrium constant at 25○C ? (e) if [Fe2+]=0.100 M and [Ag+] = 0.0100 M , what is the magnitude of E at 25○C?

Q: 3.33 Calculate the standard free energy change for the follow- ing reactions using the standard cell…

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Q: A certain metal M forms a soluble nitrate salt M(NO3), Suppose the left half cell of a galvanic cell…

A: Galvanic cell consists of two half cell, one is called cathode and the other anode. The right side…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.11 M and [Cr3+] =…

A: The considered reaction is, 3 Cu2++ 2 Cr(s) →3 Cu (s) + 2 Cr3+

Q: Calculate ΔG° for each of the reactions What is the value of the equilibrium constant for the…

A: The relationship between Gibbs free energy change ∆Go and standard electrode potential Eocell of the…

Q: Half-Reaction: Cu2+ +2e−→Cu(s) E°(V): 0.34 Half-Reaction: Zn2+ +2e−→Zn(s) E°(V): −0.76 (a) What is…

A: Given: Cu2+(aq) + 2e- ----> Cu(s)      E° = 0.34 V Zn2+(aq) + 2e- ----> Zn(s)      E° = -0.76…

Q: The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.14 M and [Co2+] =…

A: Answer is given has followed

Q: (1)Using the Table, rank the following species from the strongest to the weakest reducing agent:…

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Q: M(NO), Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of…

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Q: Calculate ΔG˚, in kJ, for the following reaction at 25˚C. 3 Cu(s)  2 NO3-(aq) + 8 H+(aq) → 3…

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Q: Calculate the solubility product of AgCl at 25.0 °C, given the following data: AgCits)+eAg(s) +…

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Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.15 M and [Co²+] = 0.00897…

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Q: The nickel-cadmium rechargeable cell follows this overall reaction: Cds) + NiO2(s) + 2H2O + 2OH- ⇌…

A: The objective is to to compute the value of equilibrium constant, K of the reaction. Given…

Q: A certain metalM forms a soluble sulfate salt MSO, Suppose the left half cell of a galvanic cell…

A: Given data :

Q: The free energy available from a 1.10-volt Cu(II)-Zn cell under standard conditions is   -212 kJ…

A: Given that: Standard electrode potential of cell = 1.10 V To find: Standard Gibbs free energy =?

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

A: Given that, an electrochemical cell is Cus|Cu2+0.11 M||Fe2+0.0063 M|Fes. Also, the standard…

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

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Q: A voltaic cell is to be designed at standard state conditions using the following two half-…

A: If the value of cell potential is positive; then the reaction is spontaneous. If the value of cell…

Q: (a) Calculate ΔrG0 for the reactionMg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)Given : E0cell = + 2.71 V,…

A: The reaction is

Q: If the equilibrium constant for a one-electron redox reactionat 298 K is 8.7 x 104, calculate the…

A: Given: Temperature, T = 298 K Equilibrium constant, K = 8.7*104

Q: Determine AG and AG° (in kJ/mol) for the following reaction. (Assume that the Nernst potential is…

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Q: A voltaic cell utilizes the following reaction and operates at 298 K. (a) What is the emf of this…

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Q: (a) Calculate ArG° for the reaction:Mg(s) + Cu22+(aq) > Mg2+(aq) + Cu(s)Given: E°cell = + 2.71 V,…

A: (a) The given reaction is, E◦ cell = 2.71 V Number of electrons transferred, n = 2 1 F = 96500…

Q: S. Given the following reduction half-reactions at 298 K: Half-Reaction E (V) at 298 K Fe" (aq) + e→…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: A voltaic cell was build upon the following redox reaction: 4 Ag (s) + O2 (g) + 4 H+ (aq) →4 Ag (s)…

A: if ∆G° is negative the reaction is spontaneous. if ∆G° is positive the reaction is non spontaneous.

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: Consider the following half-reactions: Half-reaction Ag+ (aq) + e-→→ 2H+ (aq) + 2e Mg2+ (aq) + 2e…

A: In a redox reaction, the compound which gives electrons is called the reducing agent and the one…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.19 M and [Cr3+] =…

A: The cell reaction given is, => 3 Cu2+ (aq) + 2 Cr (s) ↔ 2 Cr3+ (aq) + 3 Cu (s) Given: [Cu2+ ] =…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e → 2Br (aq)|1.080V 2H"(aq) +…

A: To solve this problem we will use the given reduction potential of each species .

Q: Consult a table of standard reduction potentials and determine which of the following reactions are…

A: Standard electrode potential is the electrode potential that is measured under standard conditions…

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

Q: Calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C. (values…

A: The balanced redox reaction is obtained by subtracting the half-cell reaction of Al3+/Al from the…

Q: For the reaction shown below the equilibrium constant is 1.8 × 10¹9 at 25°C: Ni(s) + Hg₂Cl₂(s)→ Ni2+…

A: Equilibrium constant,K = 1.8× 1019 Temperature,T =25°C =298K E°cell= ?

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

A: Given: Co(s) + Fe2+(aq) ----> Co2+(aq) + Fe(s) Eocell = - 0.16 V

Q: Given: Fe+2  +  2e- ?  Fe E red o = - 0.44 V Ag+  +  e-  ?  Ag E red o =  0.80 V Fe+2 (aq)  +…

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Q: A certain metal M forms a soluble nitrate salt MNO, Suppose the left half cell of a galvanic cell…

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Q: (a) Calculate the standard reduction potential Eºcell (b) the equilibrium constant K (at 25°C) for…

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Q: What reactions take place at the cathode and the anode when each of the following is electrolyzed?…

A: Electrolysis of 1.0 M NiBr2 Reaction at Cathode :  Ni+2 + 2 e- --> Ni  Reaction at Anode : 2 Br-…

Q: Write (Definition) and draw a schematic galvanic cell for the following spontaneously reaction;…

A: Galvanic cell (Voltaic cell):  An electrochemical cell that produces electrical energy by using a…

Q: O left right ed to the nificant

A: Galvanic (or voltaic) cells called concentration cells are constructed from two half-cells that have…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.71×10-3 M and [Fe3+] =…

A: First, we need to convert the free energy change (ΔG) from kilojoules to joules because the standard…

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Given: Voltage = 11.6 V Current = 6.0 A mass of chromium (Cr) = 3.91 g molar mass of chromium =…

Q: (2) Using the standard reduction potentials listed in the Table, determine which of the following…

A: The solution is as follows:

Q: Sn(s) 1 Salt bridge 1 M Ag 1 M Sn2+ Sn is the cathode; Ag is the anode; electrons flow from left to…

A: A question based on electrochemistry. A cell diagram with anode and cathode are prescribed for which…

Q: E°cell = 1.66 V for the following cell reaction: P4(8) + 3OH´(aq) + 3H2O(1) → PH3(g) + 3H2PO2¯(aq)…

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Q: Calculate ΔG˚, in kJ, for the following reaction at 25˚C. 3 Cu(s)  2 NO3-(aq) + 8 H+(aq) → 3…

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Q: If the equilibrium constant for a one-electron redox reaction at 298 K is 5.3×104, calculate the…

A: The free energy can be calculated using the equation,