Calculate the values of E°, A,G, and K for the following reactions at 30°C: (a) Cu° + Sn* Cu+ + Sn²+ E° 4,G K

Q: Silver can be plated out of a solution containing Ag+ according to the half-reaction:Ag+(aq) +…

A: Given, Mass of silver = 12g I = 3.0A

Q: The equilibrium constant K for the overall reaction that takes place in the cell Pt|Sn2+,…

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Q: How many seconds are required to deposit  0.207 grams of iron metal from a solution that contains…

A: According to Farady's law of electrolysis we can write m =I×t×MF×νwhereI = currentt = timeM = atomic…

Q: For the following redox reaction at 25.0℃, determine the E°cell, ∆G°(kJ/mol) and K value.

A: Pb2+(aq) + 2 e- --> Pb(s) E0 = - 0.126 V.  Co2+(aq) + 2e– ⇌ Co(s). –0.277   So, E° = Eoxid +E…

Q: Calculate E°cell. Mn(s) + Fe2+(s) (aq) ↔ Mn2+ (aq) + Fe (s) a)E°cell =  ?V  b) Calculate E° for…

A: a) Eocell = Eored cathode - Eored anode  Here cathode: Fe2+ (aq) / Fe (s) Therefore, Eored cathode =…

Q: Write down the cell reaction and calculate EMF of the following cell at 25°C. Zn│ Zn 2+ (0.02M) ║…

A: Nernst equation is, E=E0cell-RTnFnQ T= temperature in Kelvin. n = number of electrons involved. F is…

Q: An unknown metal M is reduced by electrolysis from a solution of M(NO3)3. It took 74.1 s for a…

A: Given: Time = 74.1 s Mass = 0.107 g Current = 2.00 A

Q: Pt| H, (g, 1 atm) |H* (aq, ? M) I| Ag* (aq, 1.0 M) | Ag (s) Calculate the pH in the anode. The…

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Q: A cell contains two hydrogen electrodes. The negative electrode is in contact with a solution of…

A: According to the information given in the question, the cell contains two hydrogen electrodes.

Q: For the following redox reaction: Fe2* (aq) + Mg (s) = Mg²* (aq) + Fe(s) a. Identify the oxidation…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: According to the Faraday's electrolysis law -  W = Zit  W is the weight in grams.  Z = E/96500 where…

Q: The value of K, for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br°(aq)…

A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq)       E°=0.070 V The Ksp value 5.4×10-13

Q: 2. A spoon with an area of4.00 cm² is plated with silver from an Ag(CN),¯ solution, using a current…

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Q: The free energy change for the following reaction at 25 °C, when [Cr³+] = 7.70x10-3 M and [Cu2+] =…

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Q: The free energy change for the following reaction at 25 °C, when [Cu²+] = 3.44×10-3 M and [Cu²*] =…

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Q: Calculate E° for the following cells: a) Cl/CIO;//0/H,O b) OH/O2//CIO3/Cr" (basic medium)

A: A galvanic cell is used for the generation of electricity by the use of spontaneous reaction. An…

Q: A galvanic cell is at equilibrium when Ecell is within the range ±(0.05916/n) of E° Ecell is…

A: The correct option has to be chosen.

Q: Consider a galvanic cell that uses the reaction 2 Ag"(aq) + Sn(s) 2 Ag(s) + Sn2*(ac Calculate the…

A: Electrolytic cell that comprises of two half-cells with the same electrodes but have different…

Q: [References) Use the References to access important values if needed for this question. The free…

A: Given cell reaction is : Cu2+(8.37×10-3 M) +Fe2+(aq)→ Cu+(aq)+ Fe3+(1.19 M) ∆G°=71.9 kJ=71.9 ×103 J

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: If at 25°C the standard electrode potential of the Ag/Ag* electrode is 0.799 V, and the equilibrium…

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Q: Calculate the equilibrium constant at 35°C, for the redox reaction between Au (aq) and Br(aq). HINT:…

A: Given reduction half-reactions with E0 values:

Q: The following reaction occurs at 298 K:  Zn (s) + 2 Ag+ (aq) ---> Zn2+ (aq) + 2 Ag (s) i. Sketch a…

A: E°cell= E°cathode- E°anode  G°=-nFE°  G°= RT In K

Q: 2. Calculate the potential of the following two half-cells that are connected by a salt bridge:

A:

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: Recall the half-cell reaction,                     AgCl s  +  e-  →  Ag s  +  Cl- aq…

Q: If the Ecell of the following cell is 0.905 V, what is the pH in the anode compartment? Pt(s) |…

A: The given cell is as given below --- Pt(s) | H2 (1.00 atm) | H+(aq) || Ag+(0.100 M) | Ag(s) The half…

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

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Q: Calculate the ΔGO(in kJ/mol) for the following reaction at 25.0℃. Sn+2(aq)+Mn(s)→Sn(s)+Mn+2(aq)

A: Answer: ∆G° for the following reaction at 25.0°C is -200.527 kJ/mol

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: Current = 5 A Voltage = 4.5 V Time = ? Volume = 215 mL = 0.215 L Molarity = 1.19 M

Q: Calculate the non-standard cell potential (in V) for the following reaction at 612.31 ℃ with the…

A: Mg2+ concentration = [Mg2+] = 1.1×10-2 M Cu2+ concentration = [Cu2+] = 4.40× 10-5 M Temperature (t)…

Q: A solution of a metal ion Mag is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g of…

A: a.

Q: Calculate the non-standard cell potential (in V) for the following reaction at 237.73 °C with the…

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Q: A voltaic cell is constructed with two silver–silver chlorideelectrodes, each of which is based on…

A: Both the compartments have the same half cell reaction,Oxidationanode.Ags+Cl-aq→AgCls+e-…

Q: How many grams of iron metal are plated out when a constant current of 8.50 A is passed through…

A: We have 8.5 A of current, passed for 50 minutes, we have to calculate the mass of iron metal…

Q: Which metals would act as sacrificial anodes (cathodic protection) for iron? Na Mg Zn Sn Pb Despite…

A: A method that is used to control the corrosion of one metal surface by using the cathode of an…

Q: A. Calculate the standard potential of each of the following cell: Cu(s) + Pb2+(aq) → Cu2+(aq) +…

A: The Standard potential of the cell is having the formula, Ecell°=Ecathode°-Eanode° The Standard…

Q: A metallurgist wants to chromium plate his car’s hood ornament. The ornament has a surface area of…

A: Given : surface area = 13.64 in2  And thickness = 0.0040 in

Q: The button case is usually plated from the solution of AgNO3. If a current of 5.60 A is maintained…

A: The given data contains, Current  = 5.60 A Time = 1045 seconds

Q: 1. A solution of a metal ion Mi) is electrolyzed by a current of 5.00 A. After 10.0 minutes, 1.19 g…

A:

Q: Consider a Daniell cell, for which the overall cell reaction is Zn(s) + Cu2+ → Zn2+ + Cu(s). The…

A: Given cell reaction is : Zn (s) + Cu2+ (aq) → Zn2+ (aq) + Cu (s) Standard reaction energy = ΔG0 =…

Q: 1. Which of the following statements accurately describes the Nemst equation shown below? Ecell =…

A: Redox reaction are those in which both oxidation and reduction reaction occurs simultaneously.

Q: Calculate the standard reaction free energy (AGO) for the following unbalanced redox reaction in…

A: Oxidation means loss of electrons and reduction means gain of electrons during redox reaction.

Q: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: Given that,Concentration of Ag+ =0.0115MConcentration of H+ =0.335MPressure of H2 =1.00atm

Q: Consider the battery represented by the following notation. Ni(s) | Ni²*(aq) || Ag*(aq) | Ag(s)…

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Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If…

A: In the given half-cell reaction, the Cr of Cr2O72-(aq) undergoes reduction from +6 oxidation state…

Q: The free energy change for the following reaction at 25 °C, when [Cd2*] = 1.17 M and [Cr+] =…

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Q: Calculate the cell potential for this reaction, in the direction shown, at 298 K. Ni?+ (0.0000310 M)…

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Q: Suppose the following reaction happening at 25°C Sn(s) + CuSO4(aq) <-----¯ Cu(s) + SNSO4(aq)…

A: In an electrochemical cell, the electrical energy is produced from the spontaneous cell reaction at…

Q: The standard cell potentials for following reaction at standard room temperature are E Fe/Fe =…

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Q: Find K for the following reaction at at 25°C. E cell = -0.10 V Cd²+ (aq) + Fe(s) -----> Cd(s) + Fe²+…

A: We have to predict the K for the 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.