CALCULATE THE CELL POTENTIAL ,THE EQUILIBRIUM CONSTANT AND THE FREE ENERGY CHANG FOR Ba(s) +Mn^-2(aq,1M) II-->Ba^2+(aq,1M)+Mn(s) given the E^o values as Ba^2+(aq)+2e^-   -->Ba(s)  E^o=-2.90 V Mn^-2(aq)+2e^-   -->Mn(s)  E^o=+0.80 V

Q: What is the cell potential of the following voltaic cell at 25°C?…

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Q: Consider the following cell: Fe|Fe³+ ||H+, H₂|Pt If the cell is run backwards by subjecting it to a…

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

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A: A numerical problem based on Nernst equation, which is to be accomplished.

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

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Q: andard potentials given in the appendices s for the following reactions: Cu(s) +2Ag*(aq) Cu2*…

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Q: What is the proper cell notation for the reaction: Cu + 2Fe^3+ = Cu^2+ + 2Fe^2+ * O Cu(s) | Cu*+2…

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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: Cd\Cď²* (aq) (0.100M) || Ag* (aq)(0.25M)|Ag(s)

A: A numerical problem based on electrochemistry, which is to be accomplished.

Q: A Zn-Ag Galvanic cell has an Ecell value of 1.536 V. The cell diagram is as blow. Calculate the…

A: This is a simple question of electrochemistry for the application of Nernst equation.

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: Consider the reaction corresponding to a voltaic cell and its standard cell potential.…

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Q: Calculate the non-standard cell potential (in V) for the following reaction at 33.56 ℃ with the…

A: The cell reaction taking place is given as, => Pb2+ (aq) + Li (s) ------> Pb (s) + Li+ (aq)…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 178.7℃ with the…

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Q: What is the cell reaction for the galvanic cell Al(s) | Al3+(aq) || Br-(aq) | Br2(g) | Pt?   Numbers…

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Q: A galvanic cell is constructed using two half-cells in standard state: Al|Al3+ and Ni|Ni+2 Al3+(aq)…

A: To find out the standard cell potential, first check out which species are oxidized and reduced.…

Q: What is the cell potential for the (non-standard) cell at 298.15 K represented by:Pt(s) | Sn2+(aq)…

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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 cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

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Q: What is the relationship between the standard cell potentials, E°, for the followng two galvanic…

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Q: Consider the following cell reaction: Mn(s) + 2 H*(? M) →Mn²+(1.00 M) + H₂(g)(1.00 atm) If the cell…

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Q: Consider the following cell notation and use a Table of Standard Electrode Potentials (Appendix Le…

A: Ecell can be calculated using nernest equation. To calculate Ecell , we would first write a complete…

Q: voltaic cell employs the redox reaction: Au(s) + 3 Na+(aq) → 3 Na(s) + Au3+(aq)    E°cell = -4.21 V…

A: The solution is as follows:

Q: A) Write half-reactions and overall cell reaction for the following cell: Zn(s)| Zn?* (aq) ||…

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Q: Write a balanced net ionic equation for the overall reaction represented by the following cell…

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Q: How can I find the standard cell potential with the delta G being -100 kJ/mol and the redox reaction…

A: We have given that ∆G°= - 100 kJ/mole And the reaction is                                  2Ag+(aq)…

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: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Mno, (s) +…

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

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: Which of the following cells is most likely to be an example of a galvanic cell?   Zn(s) | Zn2+ ||…

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Q: A Cr+ (aq) solution is electrolyzed using a current of 7.30 A. What mass of Cr(s) is plated out…

A: a) Given: Current passed = 7.30 A. And time passed = 2.90 day = 2.90 × 24 × 60 × 60 = 250560 s…

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

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Q: Calculate the cell potential of tho following cell at 25°C. Cr(s) | C" (1.0 X 10° M) || Ni²* (1.5 M)…

A: Given data,[Cr3+]=1.0×10-3M[Ni2+]=1.5MTemperature=25oC

Q: Cr(s) | Cr^3+(aq) || VO2+(aq), H+(aq), VO^2+(aq) | Pt(s)   Calculate the equilibrium constant…

A: Anode or oxidation half-cell reaction

Q: Calculate the standard cell potential for the following galvanic cell. La(s) La (aq)|Br (1), Br…

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Q: For the galvanic cell  2Ag+ + Cr  →  2Ag + Cr2+,  which equation allows you to correctly calculate…

A: E°cell = 2.5122 V

Q: Calculate the non-standard cell potential (in V) for the following reaction at 160.73 ℃ with the…

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Q: Calculate the equilibrium constant for 2+ Ca(s) + Mn²+ (aq) (1M) → Ca²+ (aq) (1M) + Mn(s) Calculate…

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Q: What is the standard potential of an unknown M²+/M electrode if the following cell is constructed:…

A: Given, the cell notation: Pb|Pb2+||M2+|M The emf of the cell = 2.99 V The standard potential of lead…

Q: In the given electrochemical cell, what is the cathode half-reaction? Zn(s) | Zn2+(aq) || Fe3+(aq),…

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Q: Fe³+ (aq) | Fe(s) || Cl(aq) | Cl₂(g) | Pt 3+ Cl₂(g) | Cl(aq) | Pt || Fe(s)| Fe³+ (aq) 3+ Fe(s) |…

A: Lose of electrons is called Oxidation Gain of electrons is called Reduction

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.