If an alkaline battery produces a cell potential of 1.64 V, what is the value of ΔGcell? The half-reactions in alkaline batteries are:ZnO(s)+H2​O(l)+2e−Zn(s)+2OH−(aq)   ΔGcell =     kJ

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: Sketch the voltaic cell represented by this notation. You must include labels for the anode,…

A: We have to sketch the voltaic cell represented by this notation. You must include labels for the…

Q: Use the standard free energies of formation in Appendix B to calculate the standard cell potential…

A: As per the standard table standard free energy of formation is :  ∆G°f (H2) = 0 KJ/mol  ∆G°f (O2) =…

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

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Q: What is the maximum amount of electrical work that can be done when 50.5 grams of PbO2 is converted…

A: The rxn for the lead acid battery is given as   and we have to calculate the energy in terms of kJ…

Q: Calculate the standard cell potential at 25°C for the following cell reaction from standard free…

A: The question contains more than one question so only the first one is solved here, if the other one…

Q: Calculate the standard Gibbs free energy change, AG°, in kJ for the following reaction occurring in…

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Q: A constant current flows for 3.75 h through an electrolytic cell containing aqueous AgNO3(aq).…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: Under standard conditions, the ΔGo of the reactants for a given redox reaction is measured to be…

A: Since the relationship between the Eocell and the ΔGo is given by  ΔGocell = -nFEocell  where n =…

Q: An electrochemical cell Bi(s) | Bi2S3(s) | Bi2S3(aq) | Bi(s) the standard potential is 0.96 V at 25…

A: we  have to calculate the equilibrium constant for the cell

Q: Calculate the non-standard cell potential (in V) for the following reaction at 190.51 ℃ with the…

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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: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn"…

A: The reaction given is Hence in the above reaction, Sn2+ is being reduced to Sn and Ba is being…

Q: Calculate ΔGo based on the equation from the following line notation.   IO4-1(aq) + 2H+1(aq) + 2e-1…

A: Given data: Eo of IO4- half-cell = 1.60 V Formula used:

Q: Use the following two half-reactions to write balanced net ionic equations for one spontaneous…

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Q: A voltaic cell was build upon the following redox reaction: 4 Ag (s) + O2 (g) + 4 H+ (aq) →4 Ag (s)…

A: if ∆G° is negative the reaction is spontaneous. if ∆G° is positive the reaction is non spontaneous.

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: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: In the given question->[Sn2+] = 0.0670 M[Co3+] = 0.0365 M[Sn4+] = 0.00661 M [Co2+] = 0.00991MThe…

Q: The standard EMF for the cell using the overall cell reaction below is +0.57 V: 2AI (s) + 312 (s)…

A: Answer:Relation between standard Gibbs free energy change and standard cell potential will be used…

Q: Electrode Potentials and Voltaic Cells For each of the following; Write the overall cell reaction/…

A: In a cell reaction a redox reaction occur .Both oxidation and reduction occur at the same  time

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

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Q: Consider the following galvanic cell:     E° (V) Sn4+  +  2 e−   →   Sn2+ 0.139 Ag+  +  e−   →…

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Q: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

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Q: What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell…

A: Note: None of the above given reaction is giving correct answer, but by assuming these two reaction…

Q: Calculate the standard Gibbs free energy change, AGº, in kJ for the following reaction occurring in…

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Q: For the cell represented as Al(s)∣Al3+ (aq)∥Sn2+ (aq), Sn4+ (aq)∣Pt(s), how many electrons are…

A: We would first write reduction half reaction and oxidation half reaction.  From this we can check…

Q: When lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

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Q: Explain the following relationships: Delta G and w, cell potential and w, cell potential and Delta…

A: The equations for the relationship between Delta G and w, cell potential and w, cell potential and…

Q: What is the cell potential (in V) for the reaction below with the given concentrations at 33.0 oC?…

A: Given concentrations:[H+] = 0.152 M[NO3- ] = 0.470 M[Fe3+ ] = 0.885 M[NO] = 0.623 MFirst, let's…

Q: The free energy

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Q: The standard voltage, Eº, for the reaction of Zn(s) and Cl₂(g) is 2.12 V. What is the standard Gibbs…

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Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

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Q: Given the balanced electrochemical reaction below (M and N represent generic metals), what is the…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

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Q: Consider the voltaic cell with a standard cell potential of 0.150 V. What is the cell potential of…

A: Given, Cd(s)|Cd2+(1.00 × 10-4 M)|| Ni2+(0.100)|Ni(s) R = 8.314 J/mol-K F= 96,485 J/mol-V Temperature…

Q: onsider the following balanced equation for a redox reaction in an electrochemi ell: 3 Cd (s) + 2…

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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: The free energy change for the following reaction at 25 °C, when [H*] = 3.34x103 M and [Hg2*] = 1.15…

A: Given :

Q: Metallic magnesium can be made by the electrolysis of molten MgCl2. (a) What mass of Mg is formed…

A: Given chemical reaction is :  MgCl2 (s)  ---------->  Mg(s)  +  Cl2 (g)  It is a thermal…

Q: alculate the standard potential, ?∘, for this reaction from its Δ⁢G° value.…

A: Standard Reduction Potential - It is the difference between the reduction potential of cathode and…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Sn (s) is oxidized…

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Q: Use half-reaction potentials to predict whether the following reaction are spontaneous or…

A: Given: T=298.15K2H2​S(g)​+O2(g)​→2H2​O(l)​+2S(s)​Step 1: Write the half-reaction. Include the H2O,…

Q: The standard EMF for the cell using the overall cell reaction below is +0.65 V: 2AI (s) + 312 (s)…

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Q: 35. Calculate the equilibrium constant at 25 °C using standard cell potential data, Sn(s) + CuSO4…

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Q: Explain the following relationships: Delta G and w, cell potential and w, cell potential and Delta…

A: The cell which consists of the same type of electrodes and the same type of solutions just varying…

Q: A certain metal M forms a soluble sulfate salt M₂(SO4)3. Suppose the left half cell of a galvanic…

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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.