The cell potential of the cell is 0.60V measured at 300C. The half-reaction of the cell is Cr|Cr⁺³ and  Ni⁺²|Ni and the [Ni⁺²] is 2.40M. Determine the following: (a) complete cell notation, overall cell reaction and  the standard cell potential; (b) the concentration of chromium ion; (c) the free energy (remember the  free energy is related to standard cell potential); and The standard reduction potential for chromium and ion are -0.74V and -0.24V respectively

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A: Nernst equation is used to  calculate cell potential or  cell voltage as follows

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Q: The following galvanic cell is constructed at 273 K. Each aqueous phase reactant and product has a…

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Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s)   +    2 H+(aq)     ⇔    Ni+2(aq)   +     H2 (g)    Ecello = 0.23…

Q: Use the Nernst Eq. Ecell = Eocell - (RT/nF) lnQ to calculate the cell potential when [Mn2+] = 0.010…

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Q: Write a balanced equation for the following cell shorthand notation. (Assume that Pt is an inert…

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Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

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Q: 19.69 Calculate the standard cell potential of the following cell at 25°C.…

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Q: Consider the cell diagram for an electrochemical cell: Pt | Ti2+(aq), Ti3+(aq) || Br2(g), Br-(aq) |…

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Q: Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s)…

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Q: (a) The standard reduction potential for X/X and Y/Y at 285 K are 0.52 V and 0.37 V respectively.…

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Q: he cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized to H*…

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Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag     ℰ° = +0.80 V…

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Q: dit: Calculate the cell potential for the following galvanic cell at 25°C: Al(s)| AI3+ (0.0632 M)||…

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Q: What is E at 25 °C for the reaction described by Mg(s) | Mg²⁺ (1.60 M) || Pb²⁺ (0.850 M) | Pb(s)?…

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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.