1. Given the electrochemical reaction shown, what is the standard free energy of change if E* = +1.61 V? Mg/ Mg 2+ (aq) // Zn²+ (aq) / Zn

Q: A solution of nickel(II) ion (Ni2+) is electrolyzed using a current of 15.0 A (amperes) for 25.0…

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Q: Calculate the equilibrium constant for the following reaction carried out in 1 M perchloric acid:…

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Q: Given the following standard reduction potentials: Fe³+ (aq) + e Fe²+(aq), E°= +0.77V - O₂(g)+ 4 H…

A: The electrode which is having a higher reduction potential gets reduced at the cathode while the…

Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

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Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

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Q: Consider the following standard reduction potentials:   Fe3+(aq) + e- → Fe2+( aq)…

A: Electrode reduction potential of all the species are there in a series which is known as…

Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

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Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

A: Concept- By the help of nernst equation, this problem can be solved. Ecell=Eocell− 0.0592/n log10Q…

Q: A steady current of 10 A maintained for 1 hr deposits 12.2 g of zinc at the cathode. What is the…

A: Given,  I = 10 A.  t = 1 hr.  m = 12.2 gm.

Q: Complete and balance the following redox reaction in basic solution     IO3- (aq) + S2- (aq) --> IO-…

A: A redox reaction is that reaction in which there is simultaneous oxidation and reduction. The…

Q: Cr3+(aq) + 3e– -> Cr(s); E° = –0.74 V Ag+(aq) + e– -> Ag(s); E° = 0.80 V What is the cell…

A: We will use nernest Equation

Q: Consider the following reduction half-reactions and the corresponding standard reduction potentials,…

A: Given that : We have to rank following the reducing agents in terms of increasing strength, i.e.…

Q: The following galvanic cell has 8° = +1.887 V at 25°C: Co(s) | Co2+ (aq) || Ce4+ (aq), Ce3+ (aq) |…

A: The solution is as follows:

Q: (a) Calculate the standard reduction potential Eºcell (b) the equilibrium constant K (at 25°C) for…

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Q: Given the electrochemical reaction shown, what is the standard free energy change AG° if E° = +1.61…

A: ∆G° = - n F Eo n= The elctrons transfered from anode to cathode in the cell = 2. F = 96500 columbs.…

Q: The potential in an electrochemical cell, E, is related to the Gibb's free energy change (ΔG) for…

A: The objective of this question is to calculate the standard Gibbs free energy change (ΔG0) for the…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.807 M and…

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Q: Complete and balance the following redox reaction in acidic solution:  AlO2- (aq) + PO33- (aq) -->…

A: Answer - Redox reaction - An oxidation-reduction (redox) reaction is a type of chemical reaction…

Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

Q: If the potential of a Zn–H2 cell (like that in Figure ) is 0.45 V at 25 °C when [Zn2+] = 1.0 M and…

A: The concentration of H+ in the cathode compartment is to be calculated.

Q: Use the following standard reduction potentials to determine which species is the strongest reducing…

A: ->The species which has highest reduction potential that will get reduce itself and oxidize…

Q: Consider the following standard reduction potentials: Mg2+(aq) + 2e– Mg(s); E° = –1.48 V V2+(aq) +…

A: For a reaction to be spontaneous the EMF potential is to be a positive value. The standard reduction…

Q: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction: Given that current passed is…

Q: An antique automobile bumper is to be chrome plated. The bumper, which is dipped into a dichromate…

A: Current passed = 21.4 A Mass of chromium to be deposited = 1.72 x 102 g Time required is to be…

Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG =…

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Q: Use standard reduction potentials to calculate the standard free energy change in kj for the…

A: We have to calculate the standard Gibbs free energy change and the equilibrium constant value.…

Q: 7. Please answer the following questions. (a) Given the following reduction potentials Cd (OH)2 (s)…

A: The objective of the question is to calculate the standard emf of the nickel-cadmium (nicad)…

Q: The following half-reaction °E = -2,07 V. AlF63-(aq) + 3e-  Al(s) + 6F-(aq) Use the data in the…

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Q: Mn(k) | Mn²+(0.2 M) || H+ (pH= ?) | H2 (g, 1.5 atm) | The cell potential of the Pt(k) Cell was found…

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Q: Using the standard reduction potentials, determine which of the following reactions are spontaneous…

A: Feasibility of redox reactions are expressed using their cell potentials which in turn computed…

Q: A particular galvanic cell has a standard cell potential of Eocell = 0.62 V. If the Eo of the…

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Q: Given the following information: • Electrochemical cell: Niº | Ni2+ || Ag+ | Agº • Half-cell…

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Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: Reaction: 2H+ (aq)+Hg(l) → H2​(g) + Hg2+(aq)Half cell reactions:2H+(aq) + 2e−→ H2​(g)…

Q: Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- →…

A: The half reactions are  1) Mt3+ (aq) + 3 e- → Mt (s)                                Eo = 1.09 V 2)…

Q: When a ruthenium chloride solution was electrolyzed for 500. s with a 120 mA current, 31.0 mg of…

A: According to Faraday first law , in electrolysis process weight of deposition of substance is…

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.