In an electrochemical cell, Q = 4.0 and K = 0.07. What can you conclude about Ecell and E°cell?

Q: Given the reaction: Hg2+  + Cd   ⇔  Cd2+  + Hg

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Q: Which of the following relationships are true if a cell has a large positive standard cell potential…

A: Equilibrium constant greater than1 indicates that reaction poceed in forward direction

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: 1. Find ΔG in J for: X5+(aq) + 5e- → X(s) E = -0.56 V 2.  2Al(s) + 6H+(aq) → 2Al3+(aq) + 3H2(g)…

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Q: Calculate the voltages of the following voltaic cells under the conditions specified: a) Cd…

A: (a) The given cell reaction is : Cd2+(0.020 M)+Zn(s) →Zn2+(0.50 M) +Cd(s)

Q: Given a voltaic cell and the reaction attached takes place, find: ΔG°? What is Q under the…

A: As per the given data we have2NO3-(aq)+3H2(g)--->2NO(g)+2OH-(aq)+2H2OE0=+0.688VThe standard…

Q: What is the ΔG° in kJ for the following cell? X(s) + Y3+(aq) ↔ Y(s) + X3+(aq)      E°cell = -0.078…

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Q: If a redox reaction is non-spontaneous under standard conditions, what is true about the reaction's…

A: If Eo(redox reaction) is negative (Eo(redox reaction) < 0), the reaction will be non-spontaneous.…

Q: In an electrochemical cell, Q = 4560 and K = 345. What can you conclude about Ecell and E°cell?…

A: Given that the reaction quotient, Q, is 4560 and the equilibrium constant, K, is 345.

Q: What is the maximum amount of work that is possible for an electrochemical cell where E = 1.34 V and…

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Q: A solution is prepared by dissolving 22.7 g of Al2(S04)3 in water. What current would be needed to…

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Q: Determine ΔG° for a cell that utilizes the following reaction: Cl2(g) + 2Br–(aq) → 2Cl–(aq) +…

A: Formula used ∆G = -nFE° E°cell

Q: Determine the value of Ecell (25°C) for the following voltaic cell: GSW (s)  ∣  GSW3+(aq, 0.115 M)…

A: The given cell is a concentration cell and for the concentration cell, as electrodes and ions are…

Q: Using the Nernst Equation, Calculate Ecell for the following electrochemical cell under the stated…

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Q: Determine the equilibrium constant, K, for the voltaic cell composed of the following 2 half…

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Q: What is the maximum amount of work that is possible for an electrochemical cell where E = 1.09 V and…

A: The maximum amount of work that can be produced by an electrochemical cell (Wmax) is equal to the…

Q: n the electrochemical cell represented by the reaction: Sn(s) + 2Ag*(aq)→ Sn²*(aq) + 2Ag(s) which…

A: Oxidation involves loss of electrons and Reduction involves gain of electrons. Half reaction which…

Q: Determine E° for a galvanic (voltaic) cell if AG° = -6.3 kJ/mol and n = 3. (F = 96,500 J/(V•mol))…

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Q: The free energy change for the following reaction at 25 °C, when Sn2+ = 0.00776 M, is -133 kJ: Sn²+…

A: Spontaneous reaction : It is the reaction which favours the product reaction that is it supports the…

Q: Calculate the voltage generated by a hydrogen-concentration cell utilizing the following…

A: The cell reaction given is  H2 (2 atm) + 2 H+ (0.1 M) → H2 (0.5 atm) + 2 H+ (0.5M) In the above cell…

Q: Consider the following voltaic cell at 298K. Select only the statements that are TRUE. Mg (s) I Mg2+…

A: In the cell, LHE is the anode where oxidation takes place and the right hand electrode is the…

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential for the…

A: For the given reactions, F- is undergoing oxidation (increase in the oxidation state from -1 to 0)…

Q: 1. Find ΔG in J for: X5+(aq) + 5e- → X(s) E = -0.56 V   2.    2Al(s) + 6H+(aq) → 2Al3+(aq) + 3H2(g)…

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Q: Consider the following voltaic cell at 298K. Select ONLY the conditions in which Ecell > E cell- Mg…

A: Electrode having higher reduction potential undergoes reduction while that with lower reduction…

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.