The spontaneity of the following redox reaction with investigated by determining the change in Gibbs free energy at various temperature: Cu(s)+Ag^+(aq)--> Cu^2+(aq)+Ag(s) The data from the experiment is reproduced below: T/K DeltaG/kj 277.1 88.7665 287.1 82.2055 295.4 75.8375 304.9 69.0835 312.4 67.5397 322.5 64.8381 With the use of a spreadsheet program, generate a well-labeled plot of a DeltaG vs T and write down the equation of the trendline.  From the graph, determine the deltaH and deltaS of the redox reaction.  Explain the meaning of the changes in enthalpy and entropy of the reaction.

Q: After plotting the cell potential (Ecell) measured at 298 K on the y-axis versus the natural…

A: Answer: Nernst equation for calculating cell potential is shown below: Ecell=Ecell0-RTnFlnQ   Here:…

Q: Select the correct cell notation for the following reaction, which is setup as a cell with a…

A: Option b should be the correct answer.

Q: A galvanic cell Cr(s)|Cr2+(aq) || Sn2+(aq)|Sn(s) is constructed using a completely immersed Cr…

A: Cr(s) is undergoing oxidation to Cr2+(aq) and Sn2+(aq) undergoing reduction to Sn(s) half-reactions…

Q: Calculate values for the galvanic cells desch (a) Cr³+ (aq) + Cl₂(g) = Cr₂0,2 (aq) + Cl(aq) V (b)…

A:

Q: In electrochemistry, spontaneous redox reactions are used for what purpose?

A: The branch of chemistry that deals with the inter-relationship between the electricity and chemical…

Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) – Zn2-(aq) + Cu(s) the ion concentrations are [Cu2*]…

A: Th Ecell of the cell reaction can be calculated by using Nernst equation as follows -

Q: 4. Calculate the Eºcell and predict whether the following reactions would occur spontaneously in…

A: Oxidation : Loss of electrons with increase in the oxidation state .Reduction : Gain of electrons…

Q: The II, III, and IV oxidation states of Mn are related thermodynamically by these equilibria in acid…

A: Given:Determine the standard electrode potential of the couple.The standard electrode potential…

Q: Calculate the solubility product of AgCl at 25.0 °C, given the following data: AgCits)+eAg(s) +…

A:

Q: Calculate the equilibrium constants of the following reactions at 25 °C from standard potential…

A: Equilibrium is the condition in which forward rate of reaction become equal to backward rate of…

Q: A galvanic cell using Cut/Cu and Zn2+/Zn was set up at 329 K and the non-standard cell potential was…

A:

Q: The free energy change for the following reaction at 25 °C, when [H*] = 8.48x10-3 M and [Fe3+] =…

A: The given chemical reaction is

Q: The standard electrode potential (E°) for Daniel cell is +1.1 V. Calculate the ΔG° for the…

A: Gibbs free energy is the difference between enthalpy and product of entropy.

Q: 18.15 Consider the following half-reactions: MnO, (aq) + 8H*(aq) + 5e¯ - Mn²*(aq) + 4H,O(1) NO, (aq)…

A: The standard reduction potential ( Eo) value for the 1st reaction is 1.512V and for the second…

Q: ) Determine the cell potential, Eo, for an electrochemical cell described by the following cell…

A:

Q: Determine the equilibrium constant at the following reaction at 298 K. 2 Fe3+ + Sn2+ 2 Fe2+ + Sn4+…

A:

Q: Balance the redox reaction in acidic solution: Cu(s) + NO, (aq) »Cu*(aq) + NO,(8) Express your…

A: To balance a redox reaction in acidic medium. to identify species undergoing oxidation and…

Q: Consider these metal ion/metal standard reduction potentials Cd2+(aq)|Cd(s): -0.40 V;…

A: ->The species which has high reduction potential that tends to reduce itself and oxidize other…

Q: Calculate the standard Gibbs free energy change, AG°, at 25 C for the following reaction. E°cu"/cu =…

A:

Q: Given that the standard electrode potentials (E°) of metals are:K+/K = -2.93 V, Ag+/Ag = 0.80…

A: standard electrode potentials (E°) is inversely proportional to reducing power  Higher standard…

Q: Consider the reaction 2Co3+ (aq)+2CI-(aq)-2Co2+(aq)+Cl2(g) EOcell=0.71 V What is the cell potential…

A: Given data: E°cell = 0.71V  [Co3+] = 0.258V [CO2+] = 0.249V  [Cl-1] = 0.523V Pressure of Cl2 =…

Q: 11.)

A: We have given that From representation of the cell reaction  Oxidation half reaction :  Zn(s)…

Q: Consider the following electrochemical cell: Cd(s) | Cd2+ (aq) || Ce4+ (aq), Ce3+ (aq) | Pt(s) Which…

A: Nernst equation gives the relation between cell potential, standard cell potential and the…

Q: Calculate the standard reaction free energy delta G for the following redox reaction. Round to 3…

A:

Q: Calculate K for the following reaction Cu (s) + 2 Ag+ (aq) ⟶ 2 Ag (s) + Cu2+ (aq);…

A:

Q: for the galvanic cell at 298 K Zn(s) + 2In2+(aq) Zn2+(aq) + 2In+(aq) Ecell = 0.36V what is the…

A: Equilibrium constant(Kc) and Ecell are related as Ecell=0.0592nlogKc      at 298KOn rearranging the…

Q: The free energy change for the following reaction at 25 °C, when [Cu2+] = 1.71×10-3 M and [Fe3+] =…

A: First, we need to convert the free energy change (ΔG) from kilojoules to joules because the standard…

Q: cell potential

A:

Q: C-C    , C-N     , C-Cl   what is the: BOND POLAR _________________ BOND LENGTH _________________…

A:

Q: Calculate the cell potential for the following concentration cell at 25 °C.…

A: Here the cell represented consists of a cathode and the anode made up of nickel. In the cell…

Q: Calculate AG° f( in kJ) or the reaction of iron(II) ions with permanganate ions. (F =96500 C) MnO4…

A: MnO4-(aq) + 8H+(aq) + 5e- ---> Mn2+(aq) + 4H2O(l)  ; E° = 1.51 V  Fe3+(aq) + e- ---> Fe2+(aq)…

Q: 16) Using these metal ion/metal standard reduction potentials: Fe2+ (aq) Fe(s) Zn²+ (aq)|Zn(s) -0.44…

A: We know Oxidation occurs at anode and reduction occurs at cathode .  Cell potential is an intensive…

Q: Calculate the Eocell and equilibrium constant for the following reaction at 25oC. Write the answer…

A:

Q: 2b) balanced the following redox reaction in aqueous basic solution  NO3-(aq) +Fe(CN)64-(aq) -->…

A: 2b) balanced the following redox reaction in aqueous basic solution  NO3-(aq) +Fe(CN)64-(aq) -->…

Q: The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.11 M and [H+] =…

A:

Q: 4) Determine cell potential, at 298 K, for the following cell if the copper ion concentration is…

A: The electrochemical cell described involves a redox reaction between copper (Cu) and iron (Fe)…

Q: A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell…

A: Ag+ (aq) + 0.5 H2 (g) ==> H+(aq) + Ag(s)

Q: Zn cation has 0.76 V as it's standard reduction potential.the cell potential is measured for the…

A: 0.0203 mol/L

Q: 20.) Ferric oxide is one of the product of rusting. The reaction for the formation of rust is given…

A: In this question we have to tell the Gibbs energy of the reaction.

Q: In a certain zinc-copper cell, Zn(s) + Cu2"(aq) – Zn²"(aq) + Cu(s) the ion concentrations are [Cu2*]…

A:

Q: Calculate the equilibrium constant K, for the following balanced redox reaction at 25oC.  (R = 8.31…

A: When a reaction is in equilibrium it has the value of Gibbs free energy change of the reaction as…

Q: TABLE OF ELECTRODE POTENTIALS Eº Reduction (EºAg+,Ag = Electrode Reaction in 0.00 V) Reduction Eº…

A: The standard cell potential is calculated using the standard reduction potential of the cathode and…

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

A: The Nernst equation is often used to calculate the cell potential of an electrochemical cell at any…

Q: Calculate the Gibbs free energy (AG°) of the reaction below. Is this reaction spontaneous or…

A: At standard condition Gibbs free Energy explain maximum work done by a thermodynamical system .

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.