Calculated Ecell (V)Calculated E°cell (V)CellsRTEcell = E°cell'InQE cell= E°cathodenFanodeQ is reaction quotientZn(I)(0.1M) || Fe(I)(0.1M)Zn(II)(0.1M) || Pb(II)(0.1M)Zn(II)(0.1M) || Cu(I)(0.05M)Zn(I)(0.1M) || Cu(II)(0.1M)Zn(I)(0.1M) || Cu(I(0.5)Zn(I)(0.1M) || Cu(II)(1.0M)Cu(I)(1.0M) || Cu(II)(0.001M)Zn(I)(0.1M) || Cu(II)(xM) a. Calculate the EMF of cells A through F at standardstates (E°cell) and non-standard states (Ecell) usingNernst equation. Fill in Table-1 with your answers.

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Calculate the EMF of cells A through F at standard states (E°cell) and non-standard states (Ecell) using Nernst equation. Fill in Table-1 with your answers.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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.

Question

Calculated Ecell (V)
Calculated E°cell (V)
Cells
RT
Ecell = E°cell'
InQ
E cell
= E°
cathode
nF
anode
Q is reaction quotient
Zn(I)(0.1M) || Fe(I)(0.1M)
Zn(II)(0.1M) || Pb(II)(0.1M)
Zn(II)(0.1M) || Cu(I)(0.05M)
Zn(I)(0.1M) || Cu(II)(0.1M)
Zn(I)(0.1M) || Cu(I(0.5)
Zn(I)(0.1M) || Cu(II)(1.0M)
Cu(I)(1.0M) || Cu(II)(0.001M)
Zn(I)(0.1M) || Cu(II)(xM)

a. Calculate the EMF of cells A through F at standard
states (E°cell) and non-standard states (Ecell) using
Nernst equation. Fill in Table-1 with your answers.

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Direction: Choose two (2) elements for the galvanic cell in the table below. Afterward, do and answer the following questions: Draw the hypothetical galvanic cell Formulate and balance the half-reactions at the anode and cathode. Calculate the standard cell potential (or voltage) generated during the redox reactions at the anode and cathode; Include the cell diagram/notation Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness.
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A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • The equilibrium constant K at 25.0 °C. me 1. ? • The cell potential under standard conditions E°. 00 2. His results are listed below. Ex Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. 000 Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 2. 10 Ar cell n calculated quantities (Check the box next to any that are wrong.) K 0 E 27 A 2 156. kJ/mol O 2.14 X 10 0.81 V 11 B 2 66. kJ/mol O 3.65 × 10 -0.34 V C 2 -264. kJ/mol 46 1.78 x 10 -1.37 V K So Na G 4. 3.
. Consider a galvanic cell with the anode containing a Zn metal electrode and a 0.10 M Zn(NO3)2solution and the other half-cell containing a Sn metal electrode and a 0.10 M Sn(NO3)2 solution. If themeasured Ecell value is +650 mV and the Zn2+/Zn reduction potential is assumed to be −790 mV, what isthe Sn2+/Sn reduction potential? Show all work.
8:51 AM Mon Dec 5 = S BIOL 286 E B Lecture Pow... Bb Lecture Pow... O ELECTROCHEMISTRY Recognizing consistency among equilibrium constant, free... cell A B A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions º His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. C Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. n 1 AA 1 1 Explanation 142. kJ/mol O calculated quantities (Check the box next to any that are wrong.) AG - 50. kJ/mol O - 46. kJ/mol O Check www-awu.aleks.com K 24 7.54 x 10 O…