Calculate A,G and the equilibrium constant for the following reactions at 298 K. Zn?+ (aq) + Cd(s) 2 Zn(s) + Cd²+ (aq) a. You may need to use the following data: Zn2+ (aq) + 2 e + Zn(s) E° = -0.763 V Cd2+ (aq) + 2 e → Cd(s) E = -0.40 V A,G° = kJ Equilibrium constant = b. Cu(s) + 2 Ag* (aq) 2 Cu²+ (aq) + 2 Ag(s) You may need to use the following data: Ag* (aq) + e → Ag(s) E = +0.799 V Cu+ (aq) + 2 e-+ Cu(s) E° = +0.337 V A,G' =| kJ Equilibrium constant =

Q: A galvanic cell consists of a cathode with a cadmium electrode in a 0.252 M solution of Cd(NO3)2 and…

A: The concentration of cadmium ions at anode is equal to the concentration of cadmium nitrate solution…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn² +] = 0.821 M…

A:

Q: What is the standard free energy change and the equilibrium constant for the following reaction at…

A: Since the half cell reactions taking place are  At Anode (Oxidation) => Sn -----> Sn2+ + 2 e-…

Q: Use the appropriate standard reduction potentials below to determine the equilibrium constant at 326…

A: Given : 1) Net reaction : 4H+(aq) + MnO2 ​(s) + 2Fe2+(aq) -----> Mn2+(aq) + 2Fe3+(aq) + 2H2O(l)…

Q: Given the following standard reduction potentials: Half reaction E° (V) Cr3*(aq) + 3e → Cr(s) -0.740…

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Q: Calculate ΔG for the following cell reaction:  3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s)       where…

A: Concept:  For a cell reaction: The overall cell potential can be calculated by using the equation…

Q: The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3…

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Q: The normal freezing point of a certain liquid X is -5.30 °C, but when 36. g of zinc chloride (ZnCl2)…

A:

Q: Given the following two half-reactions, write the overall reaction in the direction in which it is…

A: The two given half reactions are:-  Pb2+(aq) + 2 e– → Pb(s) E° = –0.126 V Fe3+(aq) + e– → Fe2+(s) E°…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

A: Given : half cell reaction and their reduction potential

Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A: For a cell   Cell potential = E°Reduction half  - E°Oxidation half Species whose reduction potential…

Q: The free energy change for the following reaction at 25 °C, when [Pb²+] = 1.20 M and Zn²+ ] =…

A: Recall the given reaction,                              Pb2+ 1.20 M  +  Zn s  →  Pb s  +  Zn2+…

Q: Calculate E° and Ecell (at 25 °C) for the following cell reaction: Mg (s) + Sn2+ (aq) → Mg2+ (aq)…

A: Given, Sn2+ (aq) → Sn (s)             E°= ‒0.14 V Mg2+ (aq) → Mg  (s)          E°= ‒2.37 V

Q: Predict the products obtained from the electrolysis of a 1 M AlBr3 solution. Note that: 2H2O(l)…

A: The reaction taking place in electrochemical cells always prefers to be non-spontaneous. Anode…

Q: The following half reactions are used for a galvanic cell: Zn2+(aq)+2e-→Zn(s)E°=-0.76V…

A: Nerst Equation:Where,E is the cell potential under non-standard conditions.E∘ is the standard cell…

Q: Calculate the equilibrium constant K for the following reaction at 25°C from standard electrode…

A:

Q: Consider the following standard reduction potentials: Fe3+(aq) + e‒ → Fe2+(aq) E°red = 0.77 V…

A: The standard reduction potential of half cells is given as:Fe3+(aq) + e- → Fe2+ (aq)…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

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Q: Use the tabulated half-cell potentials to calculate ΔG° for the following balanced redox reaction.…

A: Standard Gibbs free energy change, Δ G° can be determined from the standard cell potential, E0 as…

Q: Given the following standard reduction potentials, determine K for the following reaction at 25°C.…

A: Given cell reaction; Pb2+(aq) + SO42−(aq) → PbSO4 (s) The standard reduction potential are: Pb2+(aq)…

Q: What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal…

A: The chemical reaction :  Cu(s) + 2Ag+(aq) ⇌ Cu2+(aq) + 2Ag(s)  The equilibrium constant at 25°C = ?

Q: Given: Zn2+(aq) + 2e–  Zn(s); E° = –0.76 V Cu2+(aq) + 2e–  Cu(s); E° = 0.34 V What is the cell…

A:

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.875 M…

A: The given cell reaction is : Zn2+=0.875 MFe2+=0.0200 M

Q: Chlorine dioxide (CIO,), which is produced by the reaction below, has been tested as a disinfectant…

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Q: 1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) +…

A: As per instruction given in our Q&A guidelines I can answer first question only. This question…

Q: The value of the equilibrium constant for the reaction of nickel(II) ions with cadmium metal is 1.17…

A: Before solving this question we must knowthe folowing concept.suppose an equilibrium reaction :-A(g)…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 2.57x10-³ M and [I₂] =…

A:

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.