Calculate the equilibrium constants of the following reactions at 25 °C from standard potential data:(a) Sn(s) + Sn4+(aq) ⇌ 2 Sn2+(aq)(b) Sn(s) + 2 AgBr(s) ⇌ SnBr2(aq) + 2 Ag(s)(c) Fe(s) + Hg(NO3)2(aq) ⇌ Hg(l) + Fe(NO3)2(aq)(d) Cd(s) + CuSO4(aq) ⇌ Cu(s) + CdSO4(aq)(e) Cu2+(aq) + Cu(s) ⇌ 2 Cu+(aq)(f) 3 Au2+(aq) ⇌ Au(s) + 2 Au3+(aq)

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of…

A: Given cell reaction: 3Co(s)+2NO3-(aq)+8H+→3Co+2(aq)+2NO(g)+4H2O(l)

Q: Calculate the standard cell potential for the reaction below, and note whether the reaction is…

A: Given, Mg(s)+Ni2+(aq)⟶Mg2+(aq)+Ni(s)   Ni2+(aq)+2e−⟶Ni(s) −0.257 Mg2+(aq)+2e−⟶Mg(s) −2.372

Q: Consider a galvanic cell with the following components: A platinum electrode in 0.20 M Fe2+ (aq) and…

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Q: Consider the cell: Pt(s) | H2(g, 0.100 bar) | H+(aq, pH = 2.54) || Cl−(aq, 0.200 M) | Hg2Cl2(s) |…

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Q: The standard reduction potential of the Pb2+/Pb electrode is -0.13 V and the standard cell potential…

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Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: Calculate the value of AGn for the following reaction at 280 K. Ką= 2.9 × 10-8 and assume Ka does…

A: Given K = 2.9 × 10-8 T = 280°K

Q: calculate the equilibrium constant for each of the reactions below Pb2+(aq)+Mg(s)→Pb(s)+Mg2+(aq)…

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Q: Given the reaction    4 Al(s) + 3O2(g) ===>  2Al2O3(s), write the half reactions and calculate…

A: The reaction given is, => 4 Al (s) + 3 O2 (g) --------> 2 Al2O3 (s)

Q: Determine the equilibrium constant, Keq, at 25°C for the reaction 2Br (aq) + L₂(s) ⇒ Br₂(1) + 2I¯…

A: The reaction given is ->  2Br- (aq) +  I2(s) --> Br2(l) + 2I-(aq)  Temperature 25°C

Q: Calculate the standard Gibbs energy in kJ/mol change for the following voltaic cell A(s) | A3+(aq)…

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Q: Calculate the standard cell potential (E∘cell�cell∘) for the reaction…

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Q: An electrochemical cell has a Cu wire dipped in 0.10 M CUSO4 on one side of the cell and a Ag wire…

A: Cell potential of an electrochemical cell at a given temperature is the difference in the potential…

Q: The redox reaction is 2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq) Calculate the following for…

A: Given,   2 SmCl3(aq) + 6 Li(aq) → 2 Sm(s) + 6 LiCl(aq)   We need to Calculate the following for the…

Q: Which of the following reactions has the largest equilibrium constant (K) at Standard Conditions?…

A: Keq = [Product]/[Reactant] However, the concentration of liquid and solid is taken as 1.

Q: What is the value of the equilibrium constant for the reaction between Sn(s) and Pb2+(aq) at 25°C?…

A: Equilibrium constant is defined products concentration divided by reactant concentration to the…

Q: What mass of each of the following substances can be produced in 1.2 h with a current of 11 A? (a)…

A: Current = 11 ATime = 1.2 h

Q: Calculate the cell potential for the galvanic cell in which the reaction   Al(s)+Au3+(aq)↽−−⇀…

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Q: What is the balanced chemical equation for this galvanic cell reaction? Cr(s) | Cr3*(aq), 1M || CI-…

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Q: (b) Fe(s) | Fe²*(aq) || Ce³+ (aq), Ce**(aq) | Pt

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Q: Cr(s) | Cr^3+(aq) || VO2+(aq), H+(aq), VO^2+(aq) | Pt(s)   Calculate the equilibrium constant…

A: Anode or oxidation half-cell reaction

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.