Using the standard recuction potentials  Au3+ + 3e- = Au   +1.41 volt Ca2+ + 2e-= Ca    -2.74 volt Calculate the value of Ecell in volt for the cell reaction: 2Au+ 3Ca2+ = 2Au3+ +3Ca

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: Consider the following galvanic cell: Ag(s) | Ag*(3.0 x 1o“ M) || Fe3*(1.1 × 10-³ M), Fe2*(0.040 M)…

A: We are given a galvanic cell and we have to answer questions based on that.

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

A: Given-> 2H+(aq) + 2e- ------> H2(g) E°= 0.00 V Cd2+(aq) + 2e- -------> Cd(s)  E°= -0.403 V…

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

A:

Q: Calculate the initial cell voltage ξ0 and the concentrations of Ag+ and Cu2+ when the cell voltage…

A:

Q: Consider the electrolysis reactions cathode anode H₂O(1) whose standard reduction potentials can be…

A: According to the reaction,The reaction at the cathode can be written as,The reaction at the anode…

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

A: First we need to determine the straight line equation used for this plot.  Then by comparing with…

Q: A galvanic cell is constructed of two half cells Zn2+*(aq)/Zn(s) and H2(g)/H*(aq) separated by a…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: For the reaction 3Cu(s) + 2Au3+(aq)  3Cu2+(aq) + 2Au(s), Eocell = 1.16 V. Calculate the cell…

A:

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: A concentration cell consists of two half-cells with identical electrodes but different ion…

A: In a concentration cell, the electricity is generated due to the potential difference created by the…

Q: he measured cell potential, ?cellEcell, for the cell shown is −0.3605−0.3605 V at 25 ∘C25 ∘C.…

A:

Q: For the cell shown, the measured cell potential, Ecell, is -0.3509 V at 25 °C. Pt(s) | H₂(g. 0.773…

A:

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

A: Consider the following balanced redox reaction:  Sn (s) + MnO2(s) + 4 H+(aq)→ Sn2+(aq)+ Mn2+(aq)+2…

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 2 (s) + 2 Br (aq) --> 21…

A: To find :  E°cell = ? Formulae used :  ∆G° = -nFE°cell  ∆G° = - RT lnK  Thus,  -nFE°cell = - RT lnK…

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: Given the schematic representation Cd | Cd2+ (1 M) || Ag+ (1 M) | Ag,  write the overall cell…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: Consider the half reactions shown below with their associated standard reduction potentials at 25 ∘C…

A: First of all we have to calculate the cell potential of the overall reaction.

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

A:

Q: Given the reaction    4 Al(s) + 3O2(g) ===>  2Al2O3(s), write the half reactions and calculate…

A: The reaction given is, => 4 Al (s) + 3 O2 (g) --------> 2 Al2O3 (s)

Q: The following standard electrode potentials have been measured at a temperature of 298 K. Ag+ + e− →…

A: In a cell, there are two components, one is an anode and the other is a cathode. The oxidation…

Q: (0.43 M) as the anode and the half-cell Sn2+(x M) | Sn(s) as the cathode; the measured cell voltage…

A:

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: What is the immediate cell potential (immediate emf) when [Fe 2+]0= 0.459 M react with [Cd2+]0= 1.00…

A: Introduction At 25oC, the cell potential or emf can be calculated by applying the following…

Q: Use the Nernst equation to calculate the cell potential,  Ecell, for a galvanic cell consisting of…

A:

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: 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: The cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

A: The cell potential is calculated by Nernst equation . E = E° - (0.0591/n) log Qc E = cell potential…

Q: Fe (s) + O2(g) + 2H2O (l) → Fe3+ + 4OH- Balance the  simple redox reaction, If the standard change…

A: Oxidation is the loss of electrons and reduction is the gain of electrons.

Q: For a standard voltaic cell comprised of a Zn2+|Zn electrode and a Fe2+|Fe electrode, what is the…

A: Cell potential of given cell can be calculated as:

Q: Calculate the standard cell potential, Ecell, for this reaction at 298 K. 12 (s) + 2 Br (aq) --> 21…

A: Equilibrium constant (Kc) = 1.1 × 10-18  Temperature (T) = 298 k  Standard cell potential (E°) = ? •…

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Given: Cr3+(aq)  →  Cr2+(aq)       E°(Cr3+/Cr2+) = −0.40 V IO−(aq)  →  I2(aq)            E°(…

Q: Determine the standard cell potential, E° cell, for a galvanic cell that employs the half-reactions…

A: Given: Reduction potential of MnO4-/Mn2+ half reaction is 1.506 V. Reduction potential of…

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

A:

Q: Consider the concentration cell shown below. Calculate the cell potential at 25°C when the…

A: (a)

Q: Calculate the cell potential in volts for following cell. Eo = +1.93 V Mg|Mg2+, 1.00 x 10-3 M||Fe2+…

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Q: An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M FeSO4 solution and…

A: In the field of science, An electrochemical cell is a source of…

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: How to balance equations?

A: We need to balance the equation: Al4C3 (s)  + H2O (l)  -------- > Al(OH)3 (s) + CH4 (g)

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: Given the standard potentials EΘ (Cu2+,Cu) = +0.340 V andEΘ (Cu+,Cu) = +0.522 V, calculate EΘ…

A: The relationship between the change in free energy (∆G0) and the electrode potential (E0) in the…

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: Calculate the standard cell potential, ?∘cell,Ecell∘, for the equation…

A: Since the cell potentials for the half reactions are as Sn(s)  -----> Sn2+ (aq) + 2 e-…

Q: Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Standard…

A: The process of breaking the electrolyte by applying an electric charge to its constituent ions is…

Q: 0.068 M and Zn2+ ion concentration = 0.194 M. Report your answer with 3 decimal places.   Zn(s) +…

A:

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: At 25 °C, a titration of 15.00 mL of a 0.0560 M AgNO3 solution with a 0.0280 M Nal solution is…

A:

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.