15. Construct a spontaneous balanced cell reaction and use the value of E° cell to calculate each of thefollowing. (25° C) (1 V= 1J/C)a. the value of E°b. the value of AGºc. the value of KCu+2 (ag)+ 2 e- → Cu (s)E° = + 0.34 VAu +3(ag)+ 3 e- –Au (s)E° = + 1.50 V%3D

Answered: Image /qna-images/answer/51c8482f-552e-4f8c-aac9-68d25eef085a.jpg

Construct a spontaneous balanced cell reaction and use the value of E° cell to calculate each of the following. (25º C) (1 V= 1J/C) b. the value of AGº c. the value of K a. the value of E° Cu+2 (ag) Cu (s) E° = + 0.34 V %3D + 2 e- Au (s) E° = + 1.50 V %3D Au ** (ag) +3 + 3 e- →

Construct a spontaneous balanced cell reaction and use the value of E° cell to calculate each of the following. (25º C) (1 V= 1J/C) b. the value of AGº c. the value of K a. the value of E° Cu+2 (ag) Cu (s) E° = + 0.34 V %3D + 2 e- Au (s) E° = + 1.50 V %3D Au ** (ag) +3 + 3 e- →

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: Determine E° for the half-reaction Fe3 (aq) + e Fe2 (aq). Fe3+(aq) + H2(g) → 2H*(aq) + Fe2+(aq) E° =…

A: E° for the following net cell reaction = +0.77 V Fe3+(aq) + H2(g) ---> 2H+(aq) + Fe2+(aq) E°…

Q: The standard cell potential (E cell) of the reaction below is -0.34 V. The value of AG for the…

A: Relationship between Gibbs free energy (∆G° ) and cell potential ( E° cell ) at standard condition…

Q: A spontaneous electrochemical reaction has which of the following? AG° 1 AG° = 0, ɛ° = 0, K> 1 %3D…

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

Q: Determine E° for the reaction: Mg(s) + Sn**(aq) → Mg²*(aq) + Sn²(aq) Reduction half-reaction: V…

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

Q: 3+(aq) +3 e Al(s) E° = -1.676 V %3D 2+(aq) + 2 e Zn(s) E° = -O.763 V %3D

A: Ecell for the given reaction is

Q: 2. Consider a voltaic cell at 25 degrees in which the following reaction takes place. 3O2(g) +…

A: Given: 3O2(g) + 4NO(g) + 2H2O --> 4NO3-(aq) + 4H+(aq) [NO3-] = 0.750 MPNO = 0.993 atmPO2 = 0.515…

Q: 1. From the table: E° (V) Half-reaction Cr+3 + 3e¯ -→ Cr Fe+2 + 2e¯ → Fe Fe+3 + e¯ → Fe+2 Sn** + 2e¯…

A: If E°cell is positive then reaction is spontaneous. If E°cell is negative then reaction is…

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

Q: 10 Question: Predict whether the following reaction would occur spontaneously at 25°C. i) Sn** (aq)…

A: The Gibbs free energy change is the energy change accompanied by the progress of the reaction. In…

Q: Calculate the standard cell potential for the reaction below. 2. Calculate ΔG°rxn for the reaction…

Q: The standard cell potential (Eᵒcell) of the reaction below is -0.34 V. The value of AG for t kJ/mol.…

A: We can calculate standard Gibbs energy ∆G° by using following equation ∆G°= - n×F×E° Where ∆G° =…

Q: What is AG° for a redox reaction where 6 moles of electrons are transferred and E° =-1.10 V? (F =…

A: Gibb’s free energy- ∆G0=-nFE0cell Where, ∆G0=change in standard Gibb’s free energy n= Number of…

Q: What is E°cell for the following reaction? Is this reaction spontaneous under standard conditions?…

A: Given : Cu+2(aq) + 2e- -----> Cu(s) E° = 0.34 V Sn+4(aq) + 2e- -------> Sn+2(aq) E° =…

Q: None

Q: A redox reaction employed in an electrochemical cell has a negative AGn. Which statement is true? a.…

A: The relation between ∆Grxn0 and Ecell0 is given by, ∆Grxn0=-nFEcell0 The relation between ∆Grxn0 and…

Q: For the galvanic (voltaic) cell Fe(s) + Mn² (aq) Fe²(aq) + Mn(s) (E° = 0.77 V at 25°C), what is [Fe]…

A: The reaction given isFe(s) + Mn²⁺(aq) ⟶ Fe²⁺(aq) + Mn(s) Since Fe is converting to Fe2+ by losing 2…

Q: 1.0 M Zn(NO3h 1.0 M CUSO How would the intensity of light from the bulb change if you were to:…

A: Topic- Redox reaction between Cu(s)/Cu2+ and Zn(s)/Zn2+.

Q: 6. Given the following galvanic cell: The Mn electrode is immersed in 0.40 M Mn²+. The other…

Q: We have the overall reaction for a lead battery, at 25°C the E° = 2.04 V Pb(s) + PbO2(s) + 2H+(aq)…

A: Reaction occurs in Lead Battery Pb (s) + PbO2 (s) + 2H+ (aq) + 2HSO4- (aq) ------>…

Q: In an electrochemical cell, Q = 0.0010 and K = 1.45. What can you conclude about ℰcell and ℰ°cell?…

A: Given: K = 1.45 And Q = 0.0010

Q: What is the E value for the Galvanic cell formed from these two half-reactions? PbO2(s) + 3 H*(aq) +…

Q: Part A The standard emf for the cell using the overall cell reaction below is +2.20 V: 2Als) + 312…

A: The solution of the question is given below:

Q: Consider the voltaic cell with the reaction: What is the E° for this cell? (A) -0.52 V (B) +0.24 V…

A: The objective of the question is to calculate the standard cell potential (E°) for the given voltaic…

Q: Calculate AGO for a voltaic cell with E° = +0.309 V if the overall reaction %3D involves a…

A: Number of electrons transferred n = 3 Emf of cell = Eo = +0.309 V We need to find change in Gibbs…

Q: Consider the cell whose net reaction is shown attached. What will the activity of the Sn (IV) ion be…

Q: 2. Calculate E° for the following voltaic cells: a) 2Nas) + Fe" (aq) → 2Na" b) 3504 (aq) + Fers) +…

A: Electrochemical cell is device which provide potential difference using chemical reaction.

Q: For the following redox reaction: MnO2(s) + NO (g) → Mn2+ (aq) + NO3-(aq) a. Write the cell…

A: Given Reaction : a. Cell Notation for this reaction: NO|NO3 || MnO2 | Mn2+ b. Yes the…

Q: What is AG° for a redox reaction where 6 moles of electrons are transferred and E° =-3.10 V? (F =…

Q: u 2 Calculate the A G° for the following redox reaction: nüz Cu(s) + Zn 2+ (aq) →Cu2+(aq) + Zn(s) E°…

Q: Consider the following standard reduction potentials, Fe2+(aq) + 2 e- → Fe(s) E° = -0.45 V Cl2(s) +…

A: The standard potentials given are, => Fe2+(aq) + 2 e- → Fe(s) E° = -0.45…

Q: What is AG° for a redox reaction where 6 moles of electrons are transferred and E° -4.30 V? (F =…

A: To calculate the Gibbs free energy change (ΔG∘) for a redox reaction,we can use the following…

Q: When E° for a cell is positive, what is true for AG° and K?

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

Q: For the reaction: 2+ 2Ag + Zn - 2Ag + Zn E° = 1.56 V. cell What is the corresponding value of AG°?.…

Q: A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3…

Q: How do I calculate the E° of a cell that contains (below) and how to write the balanced cell…

Q: Using the Nernst Equation, determine if the reaction in question 10 is spontaneous at 20 °C with…

A: For a reaction to be spontaneous, the value of cell potential (Ecell) should be negative. And the…

Q: Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e 2Br (aq) 1.080V Sn2+ *(aq) +…

Q: What is the standard cell voltage at 25.0oC for the reaction below? Hg2+(aq) + 2MnO42-(aq) ↔ Hg(l) +…

A: The given red-ox reaction is Hg2+(aq) + 2MnO42-(aq) ↔ Hg(l) + 2MnO4-(aq), K = 6.44x109 The standard…

Q: In a process of electroplating silver, a current of 15.2 amps (A) was passed through an electrolytic…

A: Since you have posted multiple questions, we are solving the first question. Please post rest of the…

Question

15. Construct a spontaneous balanced cell reaction and use the value of E° cell to calculate each of the
following. (25° C) (1 V= 1J/C)
a. the value of E°
b. the value of AGº
c. the value of K
Cu+2 (ag)
+ 2 e- → Cu (s)
E° = + 0.34 V
Au +3
(ag)
+ 3 e- –
Au (s)
E° = + 1.50 V
%3D

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 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

Calculate AG° for a voltaic cell with E° = +0.309 V if the overall reaction involves a 3- %3D electron transfer. R = 8.314 J/mol-K %3D F = 96,485 J/mol-V %3D
9. For each set of reactants, write a redox equation for the reaction that may occur. Calculate the E° cell values and determine if the reaction is spontaneous. a) Mg(s) + A1" d) Sn(s) + H* b) Hg" + Ag(s) e) H2(g) + Cl½(g) c) CI + 1(s) ) Cu(s) + I
please help
What is AG° for a redox reaction where 6 moles of electrons are transferred and E° =-2.25 V? (F = 96,500 J/(V mol))
14. Determine overall E° cell for the voltaic cell and diagram the cell including the anode, cathode, movement of electrons, and the KNO3 salt bridge: → Ag (s) Eo = +0.80 V 1+ Ag "(aa) e- E° = - 0.74 V !! Cr 3+ (ag) + 3e → Cr (8)
Give Clear Detailed mechanism Solution with explanation needed..don't give Handwritten answer
What is AG° (in kJ/mol) for a redox reaction where two electrons are transferred with E°cell = 0.317 V?
Q10
5 5) Calculate E cell at 313K for the concentration cell described below. Both electrodes are made or Mg. On the left side of the cell there is a solution of 0.10M Mg(NO3)2. On the right side of the cell a saturated solution of MgF2 is prepared by adding 1.00 g of solid of MgF2 to 100.0 mL of pure water. Because Ksp for MgF2 is small (Kp for MgF2=64 x 10"), the concentration of Mg2+ on the right side of the cell is much less than 0.10 M. %3D Mg2+ + 2e → Mg E° = -2.37 V Voltmeter Porous Mg Barrier Mg Saturated MgF2 0.10 M Mg(NO3)2
A voltaic cell utilizes the following reaction and operates at 298 K. 3 Ce4+(aq) + Cr(s) 3 Ce3+(aq) + Cr3+(aq) (a) What is the emf of this cell under standard conditions? ______V (b) What is the emf of this cell when [Ce4+] = 2.0 M, [Ce3+] = 0.012 M, and [Cr3+] = 0.011 M? _______V (c) What is the emf of the cell when [Ce4+] = 0.58 M, [Ce3+] = 0.88 M, and [Cr3+] = 1.2 M? _______V
Find K for the following reaction at at 25°C. E cell = -0.10 V Cd²+ (aq) + Fe(s) Cd(s) + Fe2+ (aq) 4.2 x 10-4 O 1.2 x 10-5 1.2 x 105 4.2 x 1010
c) 45.8 kJ/mol 9. Using the appropriate half-cell reactions, and assuming y. - product of AgCl at 25°C: AgCl(s) Ag'(aq) + Cl(aq) a) 5.21 x 10-13 b) 1.68 x 10-10 1.85 × 10-10 10. Between 0°C and 90°C th d) 50.7 kJ/mol 1, calculate the solubility d) 1.56 × 10-10