7H2O + 2 Cr³+ + 3 Cl2 = Cr2O,²- + 6 Cl¯ + 14H+ e° = 0.03 V cell a. AG° = kJ K = Cu²+ (aq) + Ba(s) = Ba²+ (aq) + Cu(s) ɛ° = 3.24 V b. AG° = kJ K = Cl2 (g) + 2 Br¯ (aq) = Br2 (g) + 2 Cl¯ (aq) e° = 0.27 V

Q: Give the standard line notation for each cell. (a) 2 103 (ад) + 10 Cr2+ (аg) + 10 H* (аq) — 10 Crst…

A:

Q: The Gibbs energy for a reaction Cu(s) + 2 H*(aq) → Cu2+ (aq) + H₂(g) at a particular temperature is…

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Q: Calculate ECELL and indicate whether the cell is galvanic or electrolytic. 8. Zn | 0.0364 M Zn+2 ||…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: . For the following reaction: Fe(s) + 2Co3+(aq) → Fe2+(aq) + 2Co2+(aq) Calculate the standard Gibbs…

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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: A galvanic cell consists of an Mg electrode in 1 M Mg(NO3)2 solution, and an Ag electrode in 1 M…

A:

Q: give proper explanation.

A: The objective of this question is to calculate the change in Gibbs free energy (ΔG°) for the given…

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: The cell potential and the equilibrium.10 :constant at 298.15 K for the cell Pt, H2 (g)|H*(aq)(a =…

A: A Galvanic cell is made up of an anode and a cathode. Reduction reaction occurs at cathode whereas…

Q: Determine AG° for the reaction N2O4(g) = 2 NO2(g) (K= 0.144 at 298 K).

A: Given :- K = 0.144                T = 298 K  To be calculated :- ∆G° (in kJ/mol)    Formula :- ∆G° =…

Q: The cell SCE || Ag, CrO, (sat 'd), CrO, (M) Ag is used for the determination of pCrO4. Calculate…

A: Recall the given cell notation,                     SCE  || Ag2CrO4 sat'd, CrO42- x M | AgThe cell…

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A: Given:Determine the standard electrode potential of the couple.The standard electrode potential…

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

A:

Q: Consider the following reaction and standard cell potential: N2H4(aq) + O2(g) → N2(g) + 2H2O(I)…

A: N2H4(aq) + O2(g) -----> N2(g) + 2H2O(l) Standard cell potential (E°cell) = 1.56 V = 1.56…

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 2 (s) + 2 Br (aq) --> 21…

A: To find :  E°cell = ? Formulae used :  ∆G° = -nFE°cell  ∆G° = - RT lnK  Thus,  -nFE°cell = - RT lnK…

Q: The Cell whose cell diagram is                                         Pb(s) | PbCl2(s) || KCl(aq)…

A: Formula used : ∆G° = -nFE° ∆G° = ∆H° - T∆S° ∆G° = -RT ln Keq

Q: 12. A concentration cell consists of two hydrogen electrodes: Pt(s) | H2(g, 1 bar) | H+(aq, pH = ?)…

A: The standard electrode potential is zero for the concentration cell because the same substance gets…

Q: Calculate the Gibbs free energy change for…

A:

Q: Calculate K for the following reaction

A: Standard Gibbs free energy and equilibrium constant (K) relation is  ∆Go = - 2.303 R T logK…

Q: Calculate the standard Gibbs energy change for the following reactions at 25oC: (a) C2H5OH(l) +…

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Q: Consider these metal ion/metal standard reduction potentials Cd2+(aq)|Cd(s): -0.40 V;…

A: ->The species which has high reduction potential that tends to reduce itself and oxidize other…

Q: Calculate the standard Gibbs free energy change, AG°, at 25 C for the following reaction. E°cu"/cu =…

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Q: Electrochemical cell Pt | H2(g) | Hl(aq) || Agl(s) | Ag(s)has electromotive potential of 0.52 V at…

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Q: Consider these metal ion/metal standard reduction potentials Cd2+ (aq)| Cd(s): -0.40 V; Zn2+ (aq)|…

A:

Q: 11.)

A: We have given that From representation of the cell reaction  Oxidation half reaction :  Zn(s)…

Q: Calculate the cell potential at 25°C for the reaction Fe(s)| Fe^3+ (aq,0.0952 M)|| C12(g,7.62 atm)…

A: Given -> T = 25°C  Fe(s)/Fe3+(aq,0.0952M)//Cl2(g,7.62atm)/Cl-(aq,0.0577M)/pt(s) E°cell = 1.396 V…

Q: What is the value of K for this aqueous reaction at 298 K? A + B C+D AG° = 14.82 kJ/mol %3D K =

A: The Gibbs free energy and the equilibrium constant are related by the following equation:…

Q: Co2+(aq) + 2e- --> Co(s)  -0.30 V Cd2+(aq) + 2e- --> Cd(s)  -0.44V [Co2+(aq)] = 0.0010 M…

A:

Q: Calculate K for the following reaction Cu (s) + 2 Ag+ (aq) ⟶ 2 Ag (s) + Cu2+ (aq);…

A:

Q: Give the standard line notation for each cell. (а) 2 I03 (ад) + 10 Cr?+ (aq) + 10 H* (аq) — 10 Cr+…

A: Given reactions are :

Q: Calculate the standard reaction enthalpy A,H of this reaction. 400 450 3.98 x 10-4 1.41 x 10-2 1.86…

A: Van't Hoff equation shows the relation between equilirbium constant and temperature of that…

Q: An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid…

A: First, we need to identify the reactions occurring at the anode and cathode. The hydrogen electrode…

Q: 20. Use the data given below to find the equilibrium constant for the following reaction at 46 °C:…

A: Data given,  The equilibrium reaction given is,  Br2 (l) + 2 I– (aq) ⇌ 2 Br– (aq) + I2 (s)  The…

Q: Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) +…

A:

Q: An electrochemical cell consists of a hydrogen electrode (p(H2) = 1 bar) immersed in an acid…

A: First, we need to identify the reactions occurring at the anode and cathode. The hydrogen electrode…

Q: Consider the cell Pb(s)│PbX2(s)│X¯(aq) (AX-=0.04) ║ Y¯(aq) (AY-=0.10)│AgY(s)│Ag(s) PbX2 (s) +…

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Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a.)

Q: Calculate the cell potential. Is the cell galvanic or electrolytic?   Pt|Fe3+(5.00 x 10-4 M), Fe2+…

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Q: cell potential

A:

Q: For cell schematic notation    Zn(s) | ZnCl2 (1.0 M )| | CuSO4 ( 2.0 M ) | Cu(s)…

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Q: 28 Calculate standard electrode potential and Gibbs free energy of the cell: Ga | Ga³+ || Ag* | Ag

A: For the given cell  with the anode on the left and the cathode on the right, we can calculate the…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l)  ; E° = 1.51 V  Fe3+(aq) + e- ---> Fe2+(aq)…

Q: 16) Using these metal ion/metal standard reduction potentials: Fe2+ (aq) Fe(s) Zn²+ (aq)|Zn(s) -0.44…

A: We know Oxidation occurs at anode and reduction occurs at cathode .  Cell potential is an intensive…

Q: 3. The following redox reaction was attempted at 25.0°C. 2H₂O(1) + 4Fe³+ (aq) → O₂(g) + 4H*(aq) +…

A:

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: Standard reduction potential of nickel = -0.257 V  Standard reduction potential of silver = 0.7996 V…

Q: For the cell shown, the measured cell potential, Ecet, is -0.3715 V at 25 °C. P(s) | H,(g.0.857 atm)…

A: Given- Ecell =-0.3715V  PH2=0.857atm Concentration of Cd2+=1.00M

Q: 43. What is the cell diagram? O None of the given. O Ag(s) | Ag+(aq) || Fe³+ (aq), Fe²+ (aq) | Fe(s)…

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Q: At 298 K. AG°=+20.9 kJ/mol for the reaction CH;CO,H (aq) =H (aq) + CH;CO2 Calculate AG for this…

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Q: 1. (a) Balance the following simple redox reaction. Fe (s) + O₂(g) + 2H₂O (1)→ Fe³+ + 4 OH (b) If…

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