Calculate the G in kJ for the following cell: Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s)  Eocell=+1.59 V Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Group of answer choices -473 -374 -158 -734 -658

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.18 minutes for a current…

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Q: For a given reaction associated with an electrochemical cell, K = 0.00134 and Q = 8.75.  Use the…

A: The objective of the question is to determine the relationship between Eºcell and Ecell for a given…

Q: Consider an electrochemical Given that the Ksp of FeCO3 is 3.5 x 10-11, what would be the expected…

A: Interpretation - In the given question here we have to determine the Ecell  of the given…

Q: Find the cell potential for the following: Al(s)| Al3+ (1 M) || Fe2+ (1 M) | Fe(s) Given: Al3+…

A: Given: Al3+ (aq) + 3 e- → Al (s) E = -1.662V Fe2+(aq) + 2e- → Fe(s) E = -0.45V

Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0120 V and n =…

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Q: Calculate values for the galvanic cells desch (a) Cr³+ (aq) + Cl₂(g) = Cr₂0,2 (aq) + Cl(aq) V (b)…

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Q: 1. Find ΔG in J for: X5+(aq) + 5e- → X(s) E = -0.56 V 2.  2Al(s) + 6H+(aq) → 2Al3+(aq) + 3H2(g)…

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Q: The free energy change for the following reaction at 25 °C, when [Zn“]= 6.68×10³ M and [H"]= 1.17 M,…

A: The relationship between the cell potential,Ecell  and free energy change is given by  ΔG = -nFEcell…

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: Calcule el potencial estándar para la celda dados la siguiente información: Cr* (ac) + 3 e - Cr (s),…

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Q: Calculate the emf of the following cell at 298 K:Fe(s) | Fe2+(0.001 M) 11 H+ (1 M) | H2(g) (1 bar),…

A: Introduction :  We have to calculate Ecell  Given :  E°cell = -0.44 V

Q: The standard electrode potential (E°) for Daniel cell is +1.1 V. Calculate the ΔG° for the…

A: Gibbs free energy is the difference between enthalpy and product of entropy.

Q: The following electrochemical notation represents correctly the spontaneous concentration cell for…

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Q: Calculate AG° (in kJ) for the following reaction: 31, (s) + 2Fe(s) →2FE** (aq) +6I¯(aq) 232 O -111 O…

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Q: -0.28 V and EFe2* IFe Co(s) | Co2*(aq, 0.15 M) || Fe*2(aq, 1.94 M) | Fe(s). Given: Eco* /co -0.447 V…

A: Co(s)|Co^2+(aq 0.15M)||Fe^+2(aq1.94M)|Fe(s) E°(Co^+2/Co)=-0.28V E°(Fe^+2/Fe)=-0.447V E

Q: The free energy change for the following reaction at 25 °C, when (Sn2+] = 1.17 M and [Fe2+]…

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Q: 19.53 Write the overall cell reaction for the following vol- taic cell. Fe(s)|Fe²*…

A: Cell notation always depicts the reaction that gets occurred in any electrochemical cell. Left part…

Q: 17.45. Calculate the E the reaction cell value at 25°C for the cell based on Fe³+ (aq) + Cr2+ (aq) →…

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Q: Calculate the non-standard cell potential (in V) for the following reaction at 94.68 °C with the…

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Q: For the following electrochemical cell: Ag(s) | Ag+(aq) | | Fe2+(aq) | Fe(s) A. Calculate the Ecell…

A: To determine the deltaG° value , first we will determine the value E°Cell.   The reaction between…

Q: Determine AG 298 for the reaction: 2NaHCO3(s) → Na₂CO3(s) + CO2 (g) + H₂O(g) Then calculate the…

A: Feasibility of any reaction can be determined by the standard gibbs free energy value.

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

A: Given:   Sn4+/Sn2+ = 0.154 V(in terms of reduction)  Or Sn2+/Sn4+ = -0.154 V(in terms of oxidation)…

Q: A galvanic cell is powered by the following redox reaction: 2 10, (aq) + 12H"(aq) + 10 Fe"(aq) I(s)…

A: In given redox reaction iron oxidised and iodine reduced.

Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0230 V and n =…

A: Equilibrium constant is calculated by help of standard Gibbs free energy change

Q: what is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0140 V and n =…

A: Given ,

Q: Home Work 11: p.230 Q2: (b) , (c) & (f) & Q4 6. 2. Compute the voltage of each of the following…

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Q: cell potential

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Q: Consider the voltaic cell with a standard cell potential of 2.89 V: Sr(s)|Sr²+ (1.0 M)||H* (1.0…

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Q: What is the maximum amount of work that is possible for an electrochemical cell where E = 1.05 V and…

A: Given that : Cell potential (E) = 1.05 V Number of moles of electrons exchanged (n) = 2 Faraday's…

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

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Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 1.13 M and [Cr³+] =…

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Q: Calculate ΔG for the following reaction:…

A: The cell reaction given is Cu2+(1M, aq) + Zn (s)→ Cu (s)+ Zn2+(1M, aq)

Q: Consider the voltaic cell with a standard cell potential of 2.37 V: Mg(s) Mg2+ (1.0 M)||H† (1.0…

A: The change in gibbs free energy is related to both Ecell and equilibrium constant.

Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0280 V and n =…

A: Electrode potential of the cell (E )

Q: (Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 3.67×10-3 M and [Ag+] =…

A: Answer:- This question is answered by using the simple concept of calculation cell potential using…

Q: Consider the following half-cells:    (1)  AgCl(s) | Ag(s), Cl–(aq)                E°red = +0.22 V…

A: In this question, we will Identify which combination produces Highest voltage.  How we can identify…

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: 2Cr(s) + 3Ni²+ (aq) 2Cr³+ (aq) + 3Ni(s) Ecell 0.51V =

A: The given redox reaction is  2 Cr(s) + 3 Ni2+(aq) →2 Cr3+(aq) + 3Ni(s), E°cell = 0.51 V The measured…

Q: Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂ (aq) + Cu (s)…

A: Temperature = 25 °C = 298 K  As per standard data :  E°Cu+2 /Cu = +0.34 V  E°Zn+2 /Zn = -0. 76 V  R…

Q: Calculate ΔG° (kJ/mol) for the following electrochemical cell: Cd(s) | Cd2+(aq) || Ni2+(aq)| Ni(s)…

A: The cell given is, => Cd(s) | Cd2+(aq) || Ni2+(aq)| Ni(s)

Q: Chemistry 19.10.-Calculate the standard potential, „E°, for this reaction from its AG° value.…

A: Given, X(s) + Y4+(aq) → X4+(aq) + Y(s)  ∆Go = 31.0 KJ = 31000 J

Q: Calculate AG° for the following cell reaction: TI(s) | TI* (aq) || Ni²+ (ag) | Ni(s) From AG°,…

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Q: . Given the following notation for an electrochemical cell: Pt(s) | H₂(1 atm) | H⁺(1 M) | | Cu²⁺(1…

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Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0135 V and n =…

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Q: (Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction…

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Q: What is the equilibrium constant K at 25°C for an electrochemical cell when E° = +0.0360 V and n =…

A: The equilibrium constant (K) of the redox (reduction-oxidation) reaction in an electrochemical cell…

Q: Calculate AG° for the electrochemical cell Fe(s) I Fe²*(aq) |I Snª*(aq) | Sn²"(aq) I Pt(s). 4+…

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Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.