Ni2+ +2e− →Ni    −0.25V Zn2+ +2e− → Zn   −0.76V Zn(s)+Ni2+(aq)⇌Zn2+(aq)+Ni(s) This reaction runs a battery. Assume this battery initially contains standard conditions, [Ni2+] and [Zn2+]=1.00M. What will be the voltage of this battery after it runs for a while and 92.8% of [Ni2+] gets used up.

Q: 2Cu²+ (aq) + Mg (s) →→→ 2Cu+ (aq) + Mg²+ (aq) Determine the equilibrium constant (K) of this…

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Q: Calculate e values for the galvanic cells based on the following overall reactions. Assume that all…

A: Given reactions are : (a). Cr3+ (aq) + Cl2 (g) <--------------> Cr2O72- (aq) + Cl- (aq)   (b).…

Q: Consider the following cell: Cu(s) | CuCl2(0.025 M) || FeCl2(0.055 M) | Fe(s) a) Using the standard…

A: According to our policy, we should solve one question  ( If any subpart is present then the first…

Q: 1. Consider the following voltaic cell: Zn (s) | Zn²+ (aq) | Br (aq) | Br2 (1)| Pt (s) a. Write a…

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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: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction:  2X(s) +  3Y2+(aq)  →2X3+  + 3Y(s) As the charges are equal on both sides.…

Q: The standard cell potential for the reaction shown here is 0.136 V. Calculate AG° for this reaction.…

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Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

A: The equilibrium constant K is defined as the ratio of the concentrations of the products to the…

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

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Q: The standard reduction potentials for zinc and silver are     Ag (aq) + e -> Ag (s)   Eo = +0.80 V…

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Q: Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the…

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Q: What is the cell notation for the following redox reaction? Sn2+(aq) + Cu2+(aq)→ Sn4+(aq) + Cu(s)…

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

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Q: Consider the cell Zn | Zn²+ || Cu²+ | Cu . What is the overall reaction? Zn(s) + Cu²+ + 2e → Zn²+…

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Q: For the reaction 2Co 3+ (aq)+2Cl − (aq)→2Co 2+ (aq)+Cl 2 (g). E ∘ =0.483 V what is the cell…

A: Given information: Standard cell potential of the cell = 0.483 V Temperature = 25 ℃ Concentration of…

Q: Starting with a cell described below: Al | Al3+ (1.00 M) || Pb2+ (1.00 M) | Pb What is the cell…

A: In this question we have to calculate the cell potential of following happen in enough time to…

Q: For the electrochemical cell Ni(s) | Ni 2+(1 M) || H +(1 M) | H 2(1 atm) | Pt(s), which one of the…

A: Well, cell reaction of Ni(s) | Ni 2+(1 M) || H +(1 M) | H 2(1 atm) | Pt(s) Anode- Ni(s)→Ni2+(aq)+2e…

Q: Consider the following cell: Cu(s) | CuCl2(0.025 M) || FeCl2(0.055 M) | Fe(s)

A: Given:  Concentration of CuCl2 = 0.025 M  Concentration of FeCl2 = 0.055 M

Q: A student does an experiment to determine the molar solubility of lead(II) iodide. She constructs a…

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Q: The equilibrium constant, K, was found to be 2.5 x108 at 25°C for the following reaction, 2X(s) +…

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Q: Calculate the standard cell potential for the reaction using the following 2 half reactions.  Na^+…

A: From the given two half cell reactions we can write the whole reaction as given below: 2Na (s) +…

Q: Calculate the standard potential for the following reactions: Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+…

A: Given that  Mg (s) + Cu2+ (aq) → Cu (s) + Mg2+ (aq) Cu2+ (aq) + 2 e- → Cu (s)    0.34 V…

Q: Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the…

A: Given: Electrochemical cell: Co(s)|Co2(+aq,0.0155M)||Ag+(aq,1.50M)|Ag(s) To find: Eocell and Ecell.

Q: The standard cell potential E0 for the cell reaction:     Zn + Cu2+       à      Zn2+  + Cu   is…

A: Given :-  Zn + Cu2+ → Zn2+ + Cu  E°cell = 1.100 V  [Zn2+] = 0.01 M  [Cu2+] = 1.0 M  To calculate :-…

Q: Consider the following redox reaction: Sn2+  +  Sr(s)  -->  Sn(s)  +  Sr2+ What is the cell…

A: Given, concentrations of Sn2+ and Sr2+ are 3.5M & 0.05M respectively at temperature 10°C. The…

Q: Consider the reaction corresponding to a voltaic cell and its standard cell potential. Zn (s) + Cu²+…

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Q: Under standard conditions, the cell potential for a voltaic cell composed of zinc and copper is 1.10…

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Q: For the following cell reaction, the standard cell potential is 1.34 V. To determine the cell…

A: The answer is n = 10. See solution below: Half cell reactions: Oxidation: 5 H2SO3 + 5 H20 => 5…

Q: The following cell notation contains two half-reactions. Pt | Fe2+ (aq), Fe3+ (aq) || Sn4+ (aq),…

A:

Q: 0.0592 V E cell -log(K) Calculate the equilibrium constant for the following reaction at 25°C:…

A: E°cell = (0.0592 V / n ) × log(K) 2Ag(s) + Fe2+(aq) <---> 2Ag+(aq) + Fe(s)  K = ?

Q: A voltaic cell is set up with a copper electrode in 1.0 mol/L CuSO4 (aq) and a lead electrode in 1.0…

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Q: Sn(s) | Sn²* (aq) || Cu²*(aq) | Cu(s) has a standard cell potential of 0.48 V. Cu2+(aq) + 2e – Cu(s)…

A: The given cell notation is:  Sn(s) | Sn2+(aq) || Cu2+(aq) | Cu(s)  Cu2+(aq) + 2e-   ---> Cu(s) ;…

Q: 3. Al(s) + NO3(aq) + 4H+ (aq) 3+ → A1³+ (aq) + NO(g) + 2 H₂O(l) 2+ 3 43 Pb²+ (aq) + 2 Cr(s) - 3…

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Q: Consider the following working voltaic cell with a positive voltage: Cu(s) | Cu²+ (aq) || Ag* (aq)|…

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Q: Construct a complete galvanic cell/voltanic cell set up. Label it and show the flow of electrons and…

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Q: Consider the voltaic cell: Sr(s)|Sr²+ (1.0 M)||H* (1.0 M)|H₂ (1 atm)|Pt(s) Which of the following…

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Q: A silver wire coated with AgCl is sensitive to the presence of chloride ion because of the half-cell…

A: Concentration of CuSO4 solution = 1 (M) Measured cell potential = 0.0518 V

Q: Eº Ni²+ + 2e → Ni Zn²+ +2e → Zn - 0.76V Zn(s) + Ni²+ (aq) Zn²+ (aq) + Ni(s) This reaction runs a…

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Q: Calculate the standard cell potential and describe the reaction as spontaneous or non-…

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Q: What is the cell reaction for the following voltaic cell? Al(s) | Al3+(aq) || Cl2(g) | Cl–(aq) |…

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Q: Fe(s) | Fe2+(aq) (0.325 M) || Ag+(aq) (0.150 M) | Ag(s) Calculate E°cell. In which direction do the…

A: Given -> Fe(s)/Fe2+(aq)(0.325M)//Ag+(aq)(0.150M)/Ag(s)

Q: Hi! I am having trouble with this. I used the nernst equation and got concentration = 0.5467 but am…

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Q: Write the Nernst equation for the cell Pt(s) U H2(g, 1.0 X 1026 bar) U H1(aq, 0.50 M) i Ag1(aq, 1.0…

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Q: Consider the voltaic Cell shown below. Voltaic Cell V Voltmeter Salt Ag (s)-> bridge Cd (s) Ag+ (aq)…

A: 1) 2.82 V2) Ag3) CdExplanation:

Q: Consider the voltaic cell:     Ni(s)|Ni2+ (1.0 M)||H+ (1.0 M)|H2 (1 atm)|Pt(s)   Which of the…

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Q: Consider the following cell reaction: Zn(s) + 2 H+(? M) —>Zn²+ (1.00 M) + H2(g)(1.00 atm) If the…

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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.