Prelaboratory Assignment: Electrochemistry: Galvanic Cells and the Nernst Equation 1. Use the calculation of E° to determine which of the following reaction is spontaneous under standard conditions: a) AuCl, o0) + 3Fe* c0) - Au, +4CI + 3 Fe" (aq) (aq). (aq) (aq) b) Cu) + 2H* (aq) Cut, +H2g) (aq)

Prelaboratory Assignment: Electrochemistry: Galvanic Cells and the Nernst Equation 1. Use the calculation of E° to determine which of the following reaction is spontaneous under standard conditions: a) AuCl, o0) + 3Fe* c0) - Au, +4CI + 3 Fe" (aq) (aq). (aq) (aq) b) Cu) + 2H* (aq) Cut, +H2g) (aq)

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...

See similar textbooks

Related questions

Q: A student measures Ecell of a concentration cell created by having the saturated solution of AgBr on…

A: According to the guidelines, we will solve the first 3 parts. If you want any other part also…

Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl2(g) -> 2 Ag+(aq) + 2 Cl2-…

A: Nernst equation is used to calculate cell potential or cell voltage as follows

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

Q: Write a balanced chemical equation for the overall cell reaction represented as (a) Ag | Ag+ ║…

A: In a balanced chemical reaction, the number of atoms or ions on each side of a reaction is the same.…

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: Introduction In drinking water, the chloride concentration is typically regulated to ensure it falls…

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

Q: What is the cell potential (EO) for a galvanic cell formed from the following two half-reactions?…

A: Interpretation- We have to determine the cell potential (Eo ) of the galvanic cell from the given…

Q: (a) In which of the voltaic cells does the hydrogen electrode serve as the cathode? 2+ SHE & Sr (aq,…

Q: Calculate Ecell for the following electrochemical cell at 25°C given that the standard cell…

A: Given -> E°cell = 0.460 V Temperature (T) = 25°C = 25 + 273 = 298 K

Q: Identify

A: According to the question, we need to identify the anode and cathode for the following…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* 1.0 M…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: The standard cell potential for the following galvanic cell is 0.390 V. What is the cell potential…

A: Given: Temperature = 325 K Eocell = 0.390 V Concentration of Sc+3 = 0.077 M Concentration of Ti+2 =…

Q: Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is…

A: Given : Table of half reactions and reduction potential. To find: Complete the given table.…

Q: Your mystery voltaic cell has a standard cell potential of 0.741 V and can be written in cell…

A: The importance of Gibbs energy is that it gives information about the spontaneity of the reaction or…

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

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

Q: Calculate the free energy for a spontaneous galvanic cell where the standard half-cell potentials…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: We have to write the half-reactions at the cathode and the anode and then write the overall balanced…

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

Q: Use the appropriate standard reduction potentials below to determine the equilibrium constant at 386…

A: In this question, we want to determine the value of Equilibrium constant. How we can determine, you…

Q: I-(aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. AgI(s) + e-…

A: Standard reduction potential, E°cell = E°c - E°a = -0.15 - 0.15 = -0.30 V Net cell reaction,…

Q: For each of the following cells, write the net ionic equations occurring at the cathode and at the…

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: Predict the standard potential for the galvanic cell. Standard reduction potentials can be found in…

A: Electrochemical cell is a cell in which chemical energy is converted into electrical energy. In this…

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: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

Q: What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2…

A: Given : half cell reaction Tip : cell having higher value of reduction potential will reduced

Q: Consider a voltaic cell whose overall reaction isPb2+(aq) + Zn(s)---->Pb(s) + Zn2+(aq). What is…

A: At 298 K, the emf (ECell) generated by the cell is calculated as shown below in equation (1) where…

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: onsider the following half-cells: (1) AgCl(s) | Ag(s), Cl–(aq) E°red =…

A: The given half cells are: (1) AgCl(s) | Ag(s), Cl–(aq) E°red = +0.22 V…

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: Consider the following galvanic cell at 25°C Pt|Br (aq) (0.25 M), H* (aq) (0.1 M) |Br2 () || O2 (g)…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3725 V at 25 °C. Pt(s) | H₂(g,0.849…

Q: Consider the following half-reactions: Half-reaction E° (V) Br,(1) + 2e → 2Br (aq) |1.080V Co2+…

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: An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a…

A: The standard reduction potential values are: Mg2+(aq) + 2e- ---> Mg(s) ; Eo = - 2.37 V I2(s) +…

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: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Calculate Ecell for the following cell: Pt(s) | H2(g) | H *(aq) || Pb2*(aq) | PBSO4(s) | Pb(s) given…

Q: In a galvanic cell, the cathode consists of a Ag*(1.00 M)|Ag half-cell. The anode is a platinum…

A: Introduction: Galvanic cell is an electrochemical cell in which currents are generated though…

Q: Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | Fe3+(aq, 0.100 M), Fe2+(aq,…

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

Q: Calculate Ecell for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm) | H+(aq,…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3537 V at 25 °C. Pt(s) | H₂(g, 0.837…

A: Cell potential, Ecell= -0.3537 VHalf-cell reactions are also given.

Q: For the cell shown, the measured cell potential, Ecell, is -0.3521 V at 25 °C. Pt(s) | H,(g, 0.785…

Q: Consider the following half-reactions: Half-reaction E° (V) F2(g) + 2e → 2F°(aq) 2.870V 2+ Pb"(aq) +…

Q: Consider the following half-cells: (1) AgCl(s) | Ag(s), Cl–(aq) E°red = +0.22 V…

A: In this question, we will Identify which combination produces Highest voltage. How we can identify…

Q: For the cell shown, the measured cell potential, Ecell, is -0.3651 V at 25 °C. Pt(s) | H₂(g, 0.797…

Question

Name:
Date:
Section:
Prelaboratory Assignment: Electrochemistry: Galvanic Cells and the Nernst
Equation
1. Use the calculation of E° to determine which of the following reaction is spontaneous under
standard conditions:
a) AuCl, (aq)
+ 3FE2+
(aq).
- Au, + 4Cl
+ 3 Fe,
(aq)
(aq)
b) Cu + 2H*,
Cu" (aq)
(aq)
Cu²+,
+ H2
1)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Be sure to answer all parts. (a) Balance the skeleton reaction. Include the states of matter for each substance. (b) Calculate E (c) Determine whether the reaction is spontaneous. A table of standard electrode potentials is given below for reference. Cl₂(g) + Fe2+ (aq) → CI (aq) + Fe³+ (aq) (a) (b) (c) O Strength of oxidizing agent cell V not spontaneous spontaneous Selected Standard Electrode Potentials (298 K) Half-Reaction F2(g) + 2e7 Cl₂(g) + 2e7 MnO₂(s) + 4H+ (aq) + 2e7 NO3(aq) + 4H+ (aq) + 3e¯ Ag+ (aq) + e Fe³+ (aq) + e O₂(g) + 2H₂O() + 4e Cu²+ (aq) + 2e7 2H+ (aq) + 2e7 N₂(g) + 5H+ (aq) + 4e¯ Fe2+ (aq) + 2e7 2+ Zn²+ (aq) + 2e 2H₂O() +2e7 Na+ (aq) + e 2F (aq) 2C1 (aq) 2+ Mn²+ (aq) + 2H₂O(l) NO(g) + 2H₂O(l) Ag(s) Fe²+ (aq) 4OH(aq) Cu(s) H₂(g) N₂Hs+ (aq) Fe(s) Zn(s) H₂(g) + 2OH(aq) Na(s) Strength of reducing agent E half-cell (V) +2.87 +1.36 +1.23 +0.96 +0.80 +0.77 +0.40 +0.34 0.00 -0.23 -0.44 -0.76 -0.83 -2.71
For the cell shown, the measured cell potential, Ecell, is -0.3587 V at 25 °C. Pt(s) | H, (g, 0.839 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2 H* (aq) + 2 e H, (g) E° = 0.00 V Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V Calculate the Ht concentration. [H*] = %3D rIC ho C TV OLER EEDO DCD 24 4/2 DELL PrtScr Insert Home End F8 F9 F10 F11 F12 F4 F5 F6 F7
Consider the following cell. Ag(s)|AgCI(s)|NaCI(aq)|Hg2Cl2(s)|Hg(/)|Pt(s) (a) Write the half-cell reactions. (Include states-of-matter under the given conditions in your answer.) Cathode: chemPad Help Greek - Anode: chemPad O Help X.X"| Greek - (b) The standard emfs of the cell at several temperatures are as follows. T/K 291 298 303 311 E°/mV 43.0 45.4 47.1 50.1 Calculate the values of A,G°, A,Sº, and A,H° for the reaction at 303 K. A,G°: A,S° kJ•mol-1 J-mol -1.к-1 %3D A,H° kJ•mol-1
What is the cell potential of the following electrochemical cell? (Report your answer to 2 significant figures.) Co(s) | Co²+ (aq, 0.31 M || Co²+ (aq, 0.035 M) | Co(s) Co²+/Co(s) = -0.28 V Eºred 1 2 4 7 +/- 5 8 v 3 6 9 0 X с x 100
For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M
Construct a galvanic cell from MnO4- (aq)/MnO2 (s) and H2 O2 (aq)/H2 O (l).a) Write a balanced equation for the cell.b) What is the value of E°cell? standard Ni (s) | Ni2+ (aq) || Ag+ (aq) | Ag (s) is constructed and the standard cell potential is1.03 V.a) Write a balanced reaction for the cell.b) What is ∆G° for the cell?
3. Calculate the standard potentials for each of the cells at 298 K. Is each combination spontaneous as written? (a) Ag (s) | Ag + (aq) || Au *3 (aq) | Au (s) (b) Cu (s) | Cu +2 (aq) || Al *3 (aq) | Al (s)
A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
Calculate values for the galvanic cells described below. (a) Cr³+ (aq) + Cl₂(g) Cr₂O7²-¯(aq) + Cl¯ (aq) (b) Zn(s) + Ag¹(aq) Zn²+ (aq) + Ag(s)
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)
Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation: