4. Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reaction described here. State whether it is spontaneous or nonspontaneous under each set of conditions at 298.15 K. Hg(l)+ S2- (aq, 0.10M) + 2Ag* (aq, 0.25M) –→ 2Ag (s) + HgS (s)

Q: The dichromate ion, Cr2O72-, in acidic solution is a common oxidizing agent for organic compounds.…

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Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

A: Given: The overall cell reaction will be as follows: 2H+(aq) + Zn(s)---------> H2(g) + Zn2+(aq).…

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

A: The cell notation given is,  Pt(s) ∣ H2(g, 1.0 atm) ∣ H+(aq,1.0M) ∣∣  Au3+(aq,? M) ∣ Au (s)

Q: free energy change

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Q: The standard cell potential for the reaction shown here is 0.136 V. Calculate AG° for this reaction.…

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Q: The cell reaction of the “Bunsen cell” is Zn(s) + 2NO3-(aq) + 4H+(aq) Zn+2(aq) + 2H2O(l) + 2NO2(g).…

A: Zn(s) + 2NO3-(aq) + 4H+(aq) --> Zn+2(aq) + 2H2O(l) + 2NO2(g)2NO3- + 4H+(aq)  +2e  -->2NO2 +…

Q: Calculate the cell potential for the galvanic cell in which the reaction   Fe(s)+Au3+(aq)↽−−⇀…

A: Please find your solution below :

Q: A)Give the reason why it is necessary to use hydrogen as a standard to define the standard potential…

A: The solutions are given below -

Q: In the presence of oxygen, the cathode half-reaction writ- ten in the preceding problem is replaced…

A: Anode half reaction for oxidation of Fe to Fe2+ is, Cathode half reaction for reduction of O2 is,…

Q: Use the tabulated electrode potentials to calculate K for the oxidation of zinc by H+ (at 25 ∘C):…

A: The Nernst equation at 298 K is as follows,                                     E = Eo - 0.0592n…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2VO (aq) +…

A: Given, 2VO2+(aq) + 4H+(aq) + Fe(s) --------> 2VO2+(aq) + 2H2O(l) + Fe2+(aq)  [VO2+] = 1.50 M…

Q: (c) Calculate the standard cell potential, E° of the following reaction at equilibrium. Show your…

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Q: Determine the thermodynamic equilibrium constant K for a voltaic cell made of a Zn strip and a Pb…

A: In a voltaic cell made  of Zn/Zn2+ and Pb/Pb2+ , the Pb/Pb2+ electrode will act as cathode because…

Q: The cell potential of the following electrochemical cell depends on the pH of the solution in the…

A: The question is based on the concept of redox reactions reactions.   Reactions in which simultaneous…

Q: Tabulated thermodynamic data can be used to predict the standard potential of a cell even if it…

A: Given: The balanced equation of the reaction is given as, Standard Gibbs energy of the reaction =…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Zn(s)→→→→→→ Hg({) + Zn²+ (aq) The standard…

A: The equation ∆G∘ = -nFE∘Cell can also be used to calculate the potential of half-cell by addition or…

Q: Consider the following reactions. Are they spontaneous in the direction written, under standard…

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Q: 1. Calculate the emf generated, Gibbs Free-Energy and the standard Gibbs Free-Energy by the cell in…

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Q: Calculate the standard cell potential for this reaction. b. 2ClO2(g) + 1l-(aq) --> 2ClO2-(aq) +…

A: The given reaction; 2ClO2(g) + 2l-(aq) --> 2ClO2-(aq) + I2(s) Here ClO2 is getting reduced and I-…

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

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

Q: For the cell represented as Al(s)∣Al3+ (aq)∥Sn2+ (aq), Sn4+ (aq)∣Pt(s), how many electrons are…

A: We would first write reduction half reaction and oxidation half reaction.  From this we can check…

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A: The standard Reduction potential of Zn2+, E◦red.= -0.76 V The standard Reduction potential of X2+,…

Q: An inventor proposes using a SHE (standard hydrogen electrode) in a new battery for smartphones that…

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

A: Given that: Reaction = Zn(s)+Cu2+(aq) ⟶ Cu(s) + Zn2+(aq)     (standard cell potential) E°cell =…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: . The reaction Si(s) + 2 H2(g) ⇌ SiH4(g) is spontaneous at 298 K. The standard enthalpy of reaction…

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Q: Consider the reaction given below at 25 degrees Celsius and answer the questions that follow. (A).…

A: An electrochemical cell undergo both oxidation and reduction process at the same time at respective…

Q: The free energy

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Q: Consider the diagram of galvanic cell, which consists of Ag*(aq)/Ag(s) and Sn²+ (aq)/Sn(s)…

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Q: Given the reaction: Anode: NO3- + 2H + +e- ---> NO2 + H2O Cathode: 2H + 2e- ---> H2 Redox:…

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Q: Calculate the cell potential for the galvanic cell in which the reaction   Al(s)+Au3+(aq)↽−−⇀…

A: Cell potential of a galvanic cell can be calculated using nernst equation

Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) | H2(g,…

A:

Q: The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] =…

A: We know from the relation that ∆G=-nFEcell where ∆G=Free energy change F=Faraday constant Ecell=Cell…

Q: A nonstandard cell is made by replacing the 1.0 M solutions of Cu(NO3)2 and Sn(NO3)2 in the standard…

A: Answer: 1. Let the standard electrode potential 1 M solution of Cu(NO3)2 and Sn(NO3)2 be E0 So,…

Q: The free energy change for the following reaction at 25 °C, when [Cd2+] = 3.67×10-3 M and [Ag+] =…

A: Answer:- This question is answered by using the simple concept of calculation cell potential using…

Q: Consider the following reaction at 298K. 2Fe3+(aq) + 2I-(aq)------>2Fe2+(aq) + I2(s) The standard…

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Q: 33M.  I need to calculate Gibb's free energy and equilibrium constant, K.  Is the reaction…

A: In an electrochemical cell, two electrodes are used. One is an anode and the other is a cathode. The…

Q: consider the following tin-permanganate cell: Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq)…

A: The cell given is Sn(s) | Sn2+ (0.36 M) || MnO4- (aq) (0.050 M), H+(aq) (0.022 M) | MnO2 (s).

Q: The net ionic cell reaction for the 'Bunsen cell ' is Zn(s) +2 NO3-(aq) + 4 H+(aq) → Zn2+(aq) + 2…

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Q: onsider the following reaction at 298K. Fe³+(aq) + Cd(s)→→→→→2Fe²+ (aq) + Cd²+ (aq) he standard…

A: Given,             ∆G°=-226.58kJ 2Fe3+(aq) + Cd(s) →2Fe2+(aq) + Cd2+(aq)∆G°=-nFEocelln= Number of…

Q: For the ΔG° values given here, determine the standard cell potential for the cell.(a) 12 kJ/mol, n =…

A: The standard cell potential(E0cell)is the potential difference between cathode and anode measured at…

Q: Consider the following reactions. Are they spontaneous in the direction written, under standard…

A: Cell with positive EMF represents negative free energy change with accompanies spontaneous change.

Q: The Nernst equation allows us to calculate non-standard state cell potentials. Much like with free…

A: Given data: Concentration of Mg2+=3.00M Concentration of Fe3+ = 1.00×10-3M E0cell = +2.33V

Q: For the reaction: Zn(s) + 2Ag*(aq) → Zn*2(aq) 2Ag(s). a. Determine the standard cell potential. b.…

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Q: Consider the following electrochemical cell notation with a cell potential of 1.22 V. Pt(s) ∣ H2(g,…

A:

Q: Referring to the table of Standard Cell Potentials below, determine the standard cell potential for…

A: E°(cell) = E°(cathode) - E°(anode) Anode: oxidation occurs Cathode: Reduction occurs

Q: In electroplating operation, the cell potential is sometimes 0V. Why is zero potential possible in…

A: Electroplating is the process of coating metal using an electric current. This is mainly for the…

Q: Consider the following galvanic cell: Agls) | Ag"(3,0 x 10“ M) || Fe³"(1.1 × 10³ M), Fe²"(0.040 M) |…

A: The give cell notation is            Ag(s)/Ag+(3.0×10-4 M)   //      Fe3+(1.1×10-3 M), Fe2+(0.040…

Q: Consider the following reaction at 298K. Hg2+ (aq) + Ni(s)→→→→→ Hg(l) + Ni²+ (aq) The standard Gibbs…

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Q: The standard cell potential is a thermodynamic state func-tion. How are E° values treated similarly…

A: The standard cell potential is a thermodynamic state function. Hence similar to other state…