Consider the following reaction at 298K. 2Fe3+(aq) + 2I-(aq)------>2Fe2+(aq) + I2(s) The standard Gibbs free energy change for this reaction is -45.548 kJ. Use the Gibbs free energy change to calculate the standard cell potential for this reaction.

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

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

A: To calculate the electrode potential of the given electrochemical cell solving only the first…

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

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Q: free energy change

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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: The cell reaction of the “Bunsen cell” is Zn(s) + 2NO3-(aq) + 4H+(aq) Zn+2(aq) + 2H2O(l) + 2NO2(g).…

A: Zn(s) + 2NO3-(aq) + 4H+(aq) --> Zn+2(aq) + 2H2O(l) + 2NO2(g)2NO3- + 4H+(aq)  +2e  -->2NO2 +…

Q: Consider the following reaction at 298K. 2Fe³+ (aq) + Fe(s) 2Fe2+ (aq) + Fe²+ (aq) The standard…

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

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Q: me standard The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E…

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Q: Consider the following reaction at 298K. Hg2+ (aq) + Co(s)→→→ Hg(t) + Co²+ (aq) The standard Gibbs…

A: Given-> ∆G° = -219.06 KJ = -219.06 × 1000 J = -219060 J

Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

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

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Q: Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the…

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Q: Calculate ΔG° for the electrochemical cell Pb(s) | Pb ⁺²(aq) || Fe ⁺³(aq) | Fe ⁺²(aq) | Pt(s) A)…

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

A: It is an example of electrochemical reaction  Here we are required to find which of 3 quantities are…

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: Consider the following galvanic cell at 25°C:Pt|Cr2+(0.30M),Cr3+(2.0M)||Co2+(0.20M)|CoThe overall…

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Q: . The reaction Si(s) + 2 H2(g) ⇌ SiH4(g) is spontaneous at 298 K. The standard enthalpy of reaction…

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

A: The objective of the question is to check for the incorrect values in the given table.Standard EMF…

Q: The free energy

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Q: The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.17 M and [Ni2+] =…

A: The energy which are used in reaction  to  do work is known as Gibbs free energy.

Q: Given the reaction: 2 H₂O(l) → 2 H₂(g) + O₂(g) for which AH°25°c = +571.7 kJ. Determine the cell…

A: 2H2O(l) = H2(g) + O2(g) Required cell representation Reaction at cathode : O2 + 2H2O + 4e- = 4OH-…

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] =…

A: We know from the relation that ∆G=-nFEcell where ∆G=Free energy change F=Faraday constant Ecell=Cell…

Q: • The siandard reaction free energy AG". • The equilibrium constant K at 25.0 °C. • The cell…

A: Gibbs free energy of a reaction is related with its equilibrium constant K  by the equation, ∆G =…

Q: The free energy change for the following reaction at 25 °C, when [Ag+] = 1.13 M and [Fe2+] =…

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Q: what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The…

A: The solution is as follows :

Q: Consider the electrochemical cell reaction of hydrogen gas and chlorine gas to produce 1 mol of HCI…

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Q: consider the following tin-permanganate cell: Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq)…

A: The cell given is Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq) (0.022 M) | MnO2 (s).

Q: The free energy change for the following reaction at 25 °C, when Sn2+ = 0.00776 M, is -133 kJ: Sn²+…

A: Spontaneous reaction : It is the reaction which favours the product reaction that is it supports the…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 56.48 ℃ with the…

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Q: Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) + Zn(s) – Fe(s) + Zn?+(aq) AG' =…

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Q: A voltaic cell is set up with an aluminum electrode in a 0.025 mol/L AlI(NO3)3 aqueous solution and…

A: A numerical problem based on determination of cell potential.

Q: Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you…

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Q: Consider the following reaction at 298K. Hg2+ (aq) + Ni(s)→→→→→ Hg(l) + Ni²+ (aq) The standard Gibbs…

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

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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.