Ag+(aq) + e = Ag(s) Ag(NH,),+(aq) + e = Ag(s) + 2NH;(aq) E° = 0.80 V E° = 0.37 V

Q: Give the standard line notation for each cell. (a) 2 103 (ад) + 10 Cr2+ (аg) + 10 H* (аq) — 10 Crst…

A:

Q: 9. At 25° C: AG° is 21.3 kJ for the reaction HCO,H(aq) - H*(aq) + HCO2 (aq) Given that R= 8.314…

A:

Q: Use the tabulated electrode potentials to calculate K for the oxidation of iron by H++ (at 25°C):…

A:

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

A:

Q: The standard cell potential for the reaction: A (s) + B2* (aq) = A2* (aq) + B (s) is - 0.371 V. What…

A:

Q: The cell potential for the standard galvanic cell shown above is +1.56V. If AgNO3(aq)|Ag(s) is…

A: Initially, At cathode:   E°AgNO3/Ag=+0.80 V      (reduction)At anode :    E°Zn(NO3)2/Zn=-0.76 V…

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: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

Q: Manganese dioxide (MnO2) for use in dry cell batteries is made by electrolyzing solutions of Mn2*…

A:

Q: Consider the following reaction and its AG° at 25.00 °C. 2 Ag*(aq)+Cu(s) 2 Ag(s) + Cu²+(aq) AG° =…

A: Standard cell potential, E0: The standard cell potential (E°cell) is the potential of the cell under…

Q: How long would it take to deposit 3.75 g of iron from an aqueous solution of iron (III) sulfate by…

A: According to Faraday's First Law of Electrolysis, the chemical deposition due to flow of current…

Q: Brass, an alloy of copper and zinc, can be produced by simultaneously electroplating the two metals…

A:

Q: Write the individual electrode reactions and the overall cell reaction for the following cell: Pt |…

A: The electromotive force of the cell or of the EMF of the cell is the maximum potential difference…

Q: 4. Calculate the Gibbs Free-Energy and the standard Gibbs Free- Energy by the cell in the given cell…

A: Given : [Zn+2]  = 4.0 x 10-3 M  [H2] = 0.010 M  [H+] = 1.0 M  Also,  E°Zn+2/Zn = - 0.76 V  E°H+/H2 =…

Q: 2+ A current of 3.40 A is passed through a solution containing Cu²+ (aq) for 30.0 minutes, with…

A:

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 at 25 ∘C for the reaction X(s)+2Y+(aq)→X2+(aq)+2Y(s) where…

A: Given standard cell potential : X(s)+2Y+(aq)→X2+(aq)+2Y(s) Also, ∆H° = -935 KJ/mol ∆S° = -373 J/K…

Q: The standard cell potential for the reaction Zn + 2 Ag+(aq) → Zn2+(aq) + 2 Ag is 1.56 V. Given that…

A: In the given reaction the Zn is getting oxidized to Zn2+ while the Ag+ is getting reduced to Ag. So…

Q: The standard cell potential of a voltaic cell consdtructed using the cell reaction below is 0.772 V.…

A:

Q: If a standard cell potential is E°cell = +0.85 V at 25 °C, is the redox reaction of thecell…

A: The standard condition for a reaction to be a spontaneous is the standard cell potential is E°cell…

Q: For the standard cell potentials given here, determine the ΔG° for the cell in kJ.(a) 0.000 V, n =…

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

A:

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr, converting some of the H* to…

A: Given: Current (I) = 11.3 A     Volume of solution (L) = 1.25 L    Concentration of HBr = 0.552 M…

Q: What

A: We will use nernest equation.

Q: Calculate the standard Gibbs free energy change for the following cell. 2Li(s) + 2F-(aq) → 2Li* (aq)…

A:

Q: = +0.851Vwhat is the spontaneous reaction between these two half-cells and what is the poten

A: For Spontaneous reaction, E°cell is positive.  Electrode with higher standard reduction potential…

Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

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Q: What mass of each of the following substances can be produced in 1.4 h with a current of 10. A? (a)…

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Q: For the below reaction, AGn at 298 K is -84.1 kJ. Calculate its equilibrium constant, K. 3. Fe2+…

A: The equilibrium constant for a given reaction is defined as the number which is used to express…

Q: 3. For the reaction: Zn(s) + 2Ag (aq)-Zn2(aq) 2Ag(s).. a. Determine the standard cell potential. b.…

A: Standard cell potential: E°cell =E°reduction -E°oxidation Where E°reduction = standard reduction…

Q: Q.4. Calculate the standard Gibbs free energy change, AG°, at 250C for the following reaction.…

A:

Q: If the coefficients of a balanced reaction are all multiplied by 2, the cell potential is also twice…

A: Given that we have to multiply the coefficient of a cell reaction with 2.

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

A: The details solution for this is provided below in attach image. And table is drawn on last page…

Q: (d) The basis of a battery or cell design can be explained by a galvanic cell shown Cu…

A: In the given question we have to tell all mechanism and cell reaction of given cell.

Q: The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2…

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu?* (aq)…

A:

Q: Tell weather the following redox reactions is spontaneous or not. With explanations/solution 3+ C.…

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

Q: What mass of each of the following duced in 1.0 h with a current of 15 A? a. Co from aqueous Co2+ b.…

A: Explained as follows

Q: A constant current is passed through an electrolytic cell containing molten MgCl2 for 18 h. If 4.33…

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Q: A cell has a standard emf of+ 0.134 V at 298 K.

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Q: Enter your answer in the provided box. A constant current is passed through an electrolytic cell…

A:

Q: Consider the following reaction and its AG° at 25.00 ° 2 Ag*(aq) + Cu(s) → 2 Ag(s) + Cu²+(aq) AG° =…

A: Given that: temperature, T = 25 oC ∆G°= -88.66 kJ/mol To find: standard cell potential, Eocell?…

Q: Answer the four questions below related to the spontaneous redox reaction that occurs whenCr(OH)3(s)…

A: The two half-reactions of the given redox reaction are as follows:

Q: A concentration cell consisting of two hydrogen electrodes (P H,- latm), where the cathode is a…

A: Given data: Pressure of H2 = 1 atm  Cell voltage (Ecell) = 0.193 V Temperature = 298 K Formula used:…

Q: f the potential of a galvanic cell is +1.20 V, what is the Gibbs free-energy change when one mole of…

A: Given  potential of a galvanic cell is +1.20 V when one mole of electrons is transferred in the…

Q: Which of the following is not correct ? Electrode potential or cell potential is an intensive…

A: 1) Electrode potential or cell potential is independent of the amount of substance involved. It is…

Q: At 298 K a cell reaction has a standard cell potential of+0.17 V. The equilibrium constant for the…

A: At 298 K a cell reaction has a standard cell potential of +0.17 V. The equilibrium constant for the…

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.