Physical constants that you may need: R = 8.31446 mol K C Faraday's constant F= 96485 mol e Gas constant Determine the pH in the following cell at standard temperature 25° C, using the reduction potential given below. Provide your answer with two significant digits. Pt(s) |H₂(g, 1.0 bar) |H+ (aq, pH =?) ||AgCl(s), Ag(s) |Cl(aq, 1.0 M), Ecell = 0.243 V AgCl(s) + e → Ag(s) + Cl(aq), E° = 0.22 V

Q: 3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of…

A: Given cell reaction: 3Co(s)+2NO3-(aq)+8H+→3Co+2(aq)+2NO(g)+4H2O(l)

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

A: To calculate the electrode potential of the given electrochemical cell solving only the first…

Q: Given the cell notation  M1 | M12+(aq) |  | M2+(aq) | M2, calculate the standard potential of the…

A: The cell given is, => M1 | M12+ (aq) || M2+ | M2 Given : Standard reduction potential of M1 =…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3559 V at 25 °C. Pt(s) | H₂(g, 0.767…

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Q: Given the standard cell potential, E°ce = 1.10 V, for the cell, Zn(s) | Zn(NO,)(aq) || Cu(NO,)(aq) |…

A: Standard cell potential (E°cell) = 1.10 V  Temperature = 25°C.  The reaction :  Zn(s) + Cu2+(aq)…

Q: The standard cell potential for the following galvanic cell is 0.390 V.  What is the cell potential…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: =

A: Given: Sn | Sn2+ (aq) =−0.140 V Pb | Pb2+(aq) =−0.126 V, T= 298 K

Q: Calculate the standard cell potential at 25°C for the following cell reaction from standard free…

A: The question contains more than one question so only the first one is solved here, if the other one…

Q: Your mystery voltaic cell has a standard cell potential of 0.741 V and can be written in cell…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

Q: A Cr(s) | Cr(aq)|| Fe*(aq) | Fe(s) galvanic cell has a standard cell potential of 0.700 V. Calculate…

A: We have find out the ∆G and maximum amount of work done by the cell on the surrounding.

Q: Using these metal ion/metal standard reduction potentials: Cd2+ (aq)|Cd(s): -0.41 V; Zn²+ (aq)…

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Q: Devise a cell in which the following is the reaction and calculate the standard cell potential: 2…

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Q: For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777…

A: Ecell = 0.3657 V PH2 = 0.777 atm The balanced reduction half reactions  2 H+ (aq) + 2 e- ----->…

Q: The standard cell potential (E°) of a voltaic cell constructed using the cell reaction below is 0.76…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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

A: In the electrochemical cell notation, chromium electrode function as anode and mercury function as…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3621 V at 25 °C. Pt(s) | H₂(g, 0.765…

A: Answer: This question is based on Nernst equation which is shown below: Ecell=Ecell0-0.0592nlogQ…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

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Q: The following cell Ag | Ag+(0.10M) || Ag+(1.0M) | Ag is a concentration cell and is capable of…

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Q: For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C.   Pt(s) |…

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Q: For the cell shown, the measured cell potential, Ecell, is –0.3669 V at 25 °C. Pt(s) | H, (g, 0.713…

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Q: 1. Write the electrode reactions and the cell reactions for the following galvanic cells, and…

A: 1)   Cu CuCl2(aq) | Cl2(g), Pt The electrode reactions for this galvanic cell are as follows:   At…

Q: For the cell shown, the measured cell potential, ?cellEcell, is −0.3669 V at 25 °C.   Pt(s) |…

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Q: The measured cell potential, Ecell, is -0.3507 V at 25 °C. Pt(s) | H2(g,0.779 atm) | H+(aq,? M) ||…

A: Answer: A Galvanic cell for hydrogen ions and Cd2+ ion is given us and we have to find out the…

Q: Consider the following galvanic cell at 25°C Pt|Br (aq) (0.25 M), H* (aq) (0.1 M) |Br2 () || O2 (g)…

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Q: For the cell shown, the measured cell potential, Ecell, is -0.3725 V at 25 °C. Pt(s) | H₂(g,0.849…

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Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell.  Given  At Anode  Cu/Cu2+; E°=-0.34 V At…

Q: The following cell with the standard cell notation shown below has an t potential of 0.92 Volts…

A: As per the Nernst equation under standard conditions,   Ecell=Ecell0-0.0591nlog[A2+][B+]2----(1)

Q: For the cell shown, the measured cell potential, Ecell, is -0.3643 V at 25 °C. Pt(s) | H₂ (g,0.895…

A: Cell potential, Ecell= -0.3643 VHalf-cell reactions are also given.

Q: Consider the following cell diagram: Cool Co2+ (aq) (0.015 M) | Fe2+ (1.94 M)| Fes) (aq) What is the…

A: The cell potential will given by Nernst Equation:

Q: Based on the cell notation of an electrochemical cell, Pt(s)| H2 (g. 1 atm) |H+ (aq,0.02M)|| Ag…

A: Interpretation -  Based on the electrochemical cell which is given in the question give the answer…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

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Q: Gibbs energy change, A;G°, is related to cell potential, Eel, by the equation A;G° = -nFEl Part B…

A: The given reaction is as follows: Xs+2Y+(aq) → X2+(aq) + 2Y(s) ∆rG° of the reaction can be…

Q: For the cell shown, the measured cell potential, Ecell, is –0.3525 V at 25 °C. Pt(s) | H,(g, 0.851…

A: The cell given is, Given: Ecell = -0.3525 V Temperature = 25 oC And the half-reactions are,

Q: The measured cell potential, Ecell, for the cell shown is –0.3549 V at 25 °C. Calculate the Ht…

A: Given: E∘cell is -0.3549 V.  H2→2H+aq+  2e-    Eo=0.00 V             Cd2+aq+ 2e-→Cds Eo=-0.403 V…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3537 V at 25 °C. Pt(s) | H₂(g, 0.837…

A: Cell potential, Ecell= -0.3537 VHalf-cell reactions are also given.

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

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Q: For the cell reaction, Zn(s) | Zn2*(aq, 1 M) || Cu2*(aq, 1 M) | Cu(s), the electrode potential of…

A: Cell Notation :  Zn(s) | Zn2+(aq,1M) || cu2+(aq, 1M) | Cu(s)  Electrode potential of cathode = 0.34…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3651 V at 25 °C. Pt(s) | H₂(g, 0.797…

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Q: The cell potential of the following cell is determined using an unspecified concentration of acid.…

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Q: Identify the CORRECT cell notation for the galvanic cell (diagram below) that involves an…

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Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co²+ (aq) = Ti²+…

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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.