Consider a galvanic cell with a zinc electrode immersed in 1.0 M Zn²* and a nickel electrode immersed in 0.38 M Ni²*. Zn2+ + 2e→ Zn e° = -0.76 V Ni2* + 2e→ Ni E° = -0.23 V Calculate the cell potential (Ecell) for this cell. (Hint : Find the cathode and the anode and the standard potential) a. 0.73 V b. 0.44 V c. 0.98 V d. 0.61 V

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Q: A galvanic (voltaic) cell consists of an electrode composed of chromium in a 1.0M chromium(III) ion…

A: To calculate Standard potential , we use formula : E°cell =  E°r ( cathode ) - E°r (anode )

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu2+…

A: Step 1:

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

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.825 M and…

A: Answer = 0.464 V

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Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: We will calculate the standard reduction potential at 25 degree centigrade.

Q: A certain half-reaction has a standard reduction potential Ered = +0.73 V. An engineer proposes…

A: Ecello=1.00 VEcathodeo= +0.73 V

Q: Calculate AG° and K for the following cell reactions. State whether the cell reaction is spontaneous…

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Q: Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.29 M), Cr3+ (2.0 M) || Co 2+ (0.18 M) |…

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A: we have to calculate Ecell

Q: The free energy change for the following reaction at 25 °C, when [Ag*]= 1.16 M and [Cd²+]= 3.49×10-3…

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Q: Consider the battery represented by the following notation. Ni(s) | Ni*"(aq) || Ag*(aq) | Ag(s)…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C , given that [Zn2+]=0.807 M and…

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Q: A cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given :  E°Zn+2/Zn  = -0.76 V  E°Cu+2/Cu = 0.34 V  [CuSO4] = 0.01 M  [ZnSO4] = 0.02 M

Q: ablished using the following cell reaction, Cu(s) + 2Ag+(0.100 M) Cu2+(0.200 M) + 2Ag(s) Each…

A: Given,

Q: The standard reduction potential of Cu(s) is + 0.339 V. What is its standard oxidation potential?…

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Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

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Q: Consider the following galvanic cell. (Hint: Write the balanced reaction.) Cr(s)ICr+(aq, 1.0 M) ||…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² +] = 0.755 M…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.864 M and…

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

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Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

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Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

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Q: Consider a galvanic cell based on the reaction   2 Fe2+ (aq)     +   Cl2 (g)   ------------>2 Fe3+…

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Q: A certain half-reaction has a standard reduction potential E =+0.43 V. An engineer proposes using…

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Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+]=0.753 M and…

A:

Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

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

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Q: The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn^2+(0.20 M)|| H+ (test solution)|…

A: Given, Cell potential = 0.475 V Temperature = 25°C =(25+273)K=298 K

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

A: Given :

Q: The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V.…

A: Ecell = Eocell - 0.0591/n log[product]/[reactant]

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M…

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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.