When the Hg?+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical cell with the following reaction is 2.129V. What is the Mn²+ concentration? 2+ Hg²*(aq) + Mn(s)→ Hg(1) + Mn²*(aq) 2+ Answer: M

Q: When the Hg2+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Hg2+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

A: The concentration of   Hg2+ is 1.01 M, the observed cell potential( E cell)at 298K for an…

Q: When the Pb2+ concentration is 1.17 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Cu2+ concentration is 1.02 M, the observed cell potential at 298K for an electrochemical…

A: Given: Eo (Cr3+/Cr (s)) = -0.74 V Eo (Cu2+/Cu (s)) = 0.337 VCopper act as a cathode. Chromium acts…

Q: When the Ag+ concentration is 3.64×10-4 M, the observed cell potential at 298K for an…

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Q: When the Pb2+ concentration is 1.35x104 M, the observed cell potential at 298K for an…

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Q: When the Cu²+ concentration is 5.94x10-4 M, the observed cell potential at 298K for an…

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Q: Calculate the potential for the following half-cell: Ag+(0.120M) + 1e- → Ag

A: The expression of Nernst equation is shown below: Ecell =E0cell -0.0591nlog Q Where; Ecell= cell…

Q: When the Pb²+ concentration is 1.68×104 M, the observed cell potential at 298K for an…

A: Introduction: The cells which can convert chemical energy to electrical energy are called…

Q: When the Ag+ concentration is 1.09 M, the observed cell potential at 298K for an electrochemical…

A: The reaction at cathode i.e; reduction. Ag+(aq)+e-→Ag(s)                      E0red=0.7996 V The…

Q: When the Ag+ concentration is 8.96x10-4 M, the observed cell potential at 298K for an…

A: Here we are required to find the concentration of Mn2+.

Q: When the Cu²+ concentration is 1.18 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Pb2+ concentration is 1.41 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag* concentration is 1.04 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag* concentration is 1.42 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Hg2+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag* concentration is 1.25×10-4 M, the observed cell potential at 298K for an…

A: Nernst equation can be used to determine the equilibrium concentration in galvanic cells

Q: When the Ag+ concentration is 4.98×10-4 M, the observed cell potential at 298K for an…

A: Given reaction is ,           3Ag+(aq) + Al(s)----> 3Ag(s) + Al3+(aq) Nernst equation for the…

Q: When the Ag* concentration is 1.23 M, the observed cell potential at 298K for an electrochemical…

A: Given:  Concentration of Ag+ = 1.23 M  Cell potential = 3.264 V

Q: When the Ag* concentration is 1.25×104 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Hg2+ concentration is 8.85×10-4 M, the observed cell potential at 298K for an…

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Q: When the Pb2+ concentration is 1.10 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Cu²+ concentration is 9.81x10-4 M, the observed cell potential at 298K for an…

A: Given, Cu2+(aq) + Mn(s) ---> Cu(s) + Mn2+(aq) Cell potential (Ecell) = 1.428 V [Cu2+] = 9.81 ×…

Q: When the Hg2+ concentration is 1.47 M, the observed cell potential at 298K for an electrochemical…

A: Nernst equation is used to determined the cell potential of reaction. Formula of Nernst equation.…

Q: When the Hg* concentration is 1.36 M, the observed cell potential at 298K for an electrochemical…

A: concentration of Hg2+ = 1.36 M  Ecell = 1.668 V  We have to find concentration of Cr3+

Q: When the Hg2+ concentration is 1.23 M, the observed cell potential at 298K for an electrochemical…

A: Given reaction is : 3Hg2+ (aq) + 2Cr (s) ---------> 3Hg (l) + 2Cr3+ (aq)  Concentration of Hg2+ =…

Q: When the Cu²+ concentration is 1.04 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Pb2+ concentration is 1.13 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Hg2+ concentration is 1.16 M, the observed cell potential at 298K for an electrochemical…

A: The given electrochemical cell is 3Hg2+(aq) + 2Al(s)→3Hg(l) + 2Al3+(aq) Which is can be obtained…

Q: When the Cu2+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag+ concentration is 1.11 M, the observed cell potential at 298K for an electrochemical…

A: We will use nernest Equation

Q: When the Pb2+ concentration is 1.30 M, the observed cell potential at 298K for an electrochemical…

A: The net cell reaction :  Pb2+(aq) + Zn(s) ---> Pb(s) + Zn2+(aq)  The observed cell potential =…

Q: When the Ag+ concentration is 1.29 M, the observed cell potential at 298K for an electrochemical…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: When the Pb2+ concentration is 1.19 M, the observed cell potential at 298K for an electrochemical…

A: Since you have posted multiple questions as per guidelines we can answer one per session . if you…

Q: When the Pb2+ concentration is 5.43×10-4 M, the observed cell potential at 298K for an…

A: The Nernst equation at 298 K is given as :

Q: When the Ag+ concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

A: The given cell is an electrochemical cell.

Q: When the Ag+ concentration is 1.07 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Cu²+ concentration is 1.00 M, the observed cell potential at 298K for an electrochemical…

A: The given reaction is : The half reactions are : At cathode :Cu2+  +  2e-  →  Cu         E°=+0.34 V…

Q: When the Pb2+ concentration is 1.32×104 M, the observed cell potential at 298K for an…

A: In the given cell, lead is undergoing reduction at anode and aluminium is getting oxidized at anode.…

Q: When the Cu2+ concentration is 1.21 M, the observed cell potential at 298K for an electrochemical…

A: We will use nernest Equation to get the answer

Q: When the Ag concentration is 1.31x10 4 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

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Q: A voltaic cell employs the following redox reaction: 2 Fe+ (aq) + 3 Mg (s) → 2 Fe (s)+3 Mg²+ (aq)…

A: Given- [Fe+3]=3.10M  [Mg2+]=1.2×10-3M Ecell=? ->Answer may differ slightly because values of…

Q: When the Hg* concentration is 8.47x10+M, the observed cell potential at 298K for an electrochemical…

A: Formula used :- Ecell = E°cell - (2.303RT÷nF ) log([product]÷[Reactant]) At Room temperature…

Q: When the Cu2+ concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Ag* concentration is 1.33 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Cu2+ concentration is 2.68x10-4 M, the observed cell potential at 298K for an…

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Q: When the Ag+ concentration is 1.68×10-4 M, the observed cell potential at 298K for an…

A: The given reaction : 2Ag+(aq) + Zn(s)→2Ag(s) + Zn2+(aq)

Q: When the Pb2+ concentration is 1.15 M, the observed cell potential at 298K for an electrochemical…

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Q: When the Cu2+ concentration is 1.47 M, the observed cell potential at 298K for an electrochemical…

A: Nernst equation for electro chemical cell at standard condition is as follows, Ecell=…

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.