Q7. Calculate the equilibrium constant at 25°C for the reaction2Fe (aq) 21 (aq)-2Fe²(aq) +1₂(s)Given the standard reduction potentials:2Fe2e2Fe² E-0.771 VE-0.5355 VB) 9.161₂ +2e21A) 18.3C) 9.10x10 D) 9.54x10 E) 2.9x10²

Answered: Image /qna-images/answer/cc77d638-3096-44e6-a120-2280e2e127fc.jpg

07. Calculate the equilibrium constant at 25 "C for the reaction: 2Fe (aq) +21 (aq)-2Fe²(aq) +12(s) Given the standard reduction potentials: 2Fe +2e2Fe E-0.771 V 1₂ +2e21 A) 18.3 E-0.5355 V B) 9.16 C) 9.10x10 D) 9.54x10' E) 2.9x10¹

07. Calculate the equilibrium constant at 25 "C for the reaction: 2Fe (aq) +21 (aq)-2Fe²(aq) +12(s) Given the standard reduction potentials: 2Fe +2e2Fe E-0.771 V 1₂ +2e21 A) 18.3 E-0.5355 V B) 9.16 C) 9.10x10 D) 9.54x10' E) 2.9x10¹

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: termine E°, AG" , and K for the overall reaction from the balanced half-reactions and their standard…

A: We have to find ∆G, ∆E and K for given reaction And using given reduction potential of half cell

Q: Using data from the Standard Reduction Potentials table, place the following in order of increasing…

Q: standard Gibbs energy (G°) of

Q: Use Equation 5 and the Standard Reduction Potentials table to determine which statement is true.…

A: According to equation 5, the Eocell is given by, => Eocell = Eored (cathode) - Eored (anode)…

Q: Consider the following cell. Cr | Cr³+ (1.00 M) || Ni²+(1.00 M) | Ni = 0.68 V (a) How many…

A: (b) Write the balanced chemical equation for the overall cell reaction and use the ICE table.

Q: 2H*(aq) + Sn(s)–H2(g) + Sn²*(aq) ificant figures during intermediate calculations to avoid round off…

A: The cell reaction is: Sn + 2H+ -----> Sn2+ + H2 We have : E°cell = E°H+/H2 - E°Sn2+/Sn…

Q: Which reaction can take place spontaneously? TABLE: Standard Electrode (Reduction) Potentials at 25…

A: According to the given standard reduction potential, those species with less negative reduction…

Q: half-reaction standard reduction potential 2+ Zn (aq)+2e Zn(s) E=-0.763 V red HNO,(aq)+H (aq)+e…

A: Using concept of galvanic cell we can solve this problem. From given half cell data.

Q: Calculate the maximum amount of work produced by the cell when the partial pressure of O₂ is 0.2050…

Q: (b) Given the overall equation a redox reaction alongside the standard reduction potentials, E |A(s)…

Q: Calculate the Kf of Ag(NH3)2+ from

A: For kf, the reactions arrangement - Ag+aq+e⇔Ags...E∘=0.80 VAgs + 2NH3aq ⇔AgNH32++e-...E∘=-0.37VAdd…

Q: Use the standard reduction potenitalto calculate equilibrium constantsfor the following reaction.…

A: The reactions given are 1) H2 (g) ------> 2 H+ (aq) + 2 e-…

Q: Cr|Cr3+ ||Co2+ |Co Eo is 0.46V. the same cell was prepared in the laboratory at standard conditions.…

Q: If an electrochemical cell will be composed of the Hg electrode and Cr electrode, which one will…

A: The half cell reactions given are, 2 Hg2+(aq) + 2 e– → Hg22+ (aq) E°= 0.92 V Cr3+(aq)…

Q: 5. Consider the following reactions: 3 Ni 2"taq) + 2Cr(OH)3 (s) + 10 OH ¯ (aq) → 3 Ni (s) + 2 CrO4…

Q: 7. Calculate AG° for the following galvanic cell Zn(s) | Zn²*(aq) || Fo2*(aq) IFe(s) given these…

A: The standard electrode potential of a Galvanic cell is given by the formula E° = E°(cathode) -…

Q: half-reaction standard reduction potential Fe?+ (аq) .0 3+ Fe"(aq)+e E°=+0.771 V red…

A: The half reactions along with their standard reduction potential are given as, The half reaction…

Q: 3. How many grams of zinc, Zn (s) are electroplated out of a solution containing Zn²+ (aq) if the…

Q: (a) Write down the overall reaction for the formation of the complex ion [Zn(NH:)-]²*(aq) from its…

Q: Q2 :- You have the following cell: Cd(s) Cd² (aq, a= 1) Cu (aq, a=1) Cu(s) At a temperature of 298…

Q: A cell employs the following half-reactions. Ni(s) Eº2+ = -0.25 V Cr(s) E°3+ = -0.74 V Ni Calculate…

A: Given, Ni2+(aq) + 2e- ----> Ni(s) E°Ni2+ = -0.25 V Cr3+(aq) + 3e- -----> Cr(s) E°Cr3+ = -0.74…

Q: Given the information below. Is the cell spontaneous in the forward or reverse directions? Pt |…

A: Given that, Pt | Pt2+|| Au3+| Au Pt2+(aq) + 2 e– ----> Pt(s) ; E° = 1.20 Au3+(aq) + 3 e–…

Q: Calculate the pK for the oxidation of X by Hplus at 25 degrees C. X(s) + 1 Hplus → X1 plus (aq)+…

Q: A silver metal electrode is immersed into an AgNO3 Solution. A potential value of 0.734 V is…

A: Electrode potential is the electromotive force for the galvanic cell developed from a standard…

Q: Given the following standard reduction potentials: MnO4 (aq) + 8H*(aq) + 5 e - - Mn2*(aq) + 4 H20()…

A: The expression of Nernst equation is shown below: E =E0cell -0.0591n log Q Where; Ecell= cell…

Q: Make Latimer diagrams for Indium and Thallium, using the information in the standard reduction…

A: Latimer diagram summarizes the standard electrode potential data or the redox information of an…

Q: It is requested: a) The direction of the current

A: Galvanic cells: the devices in which chemical energy is converted into electrical energy Redox…

Q: The voltaic cell Ca(o)Ca²+ (aq) || Ni?+(1.0 M)|Ni(s) has a cell potential of 0.300 V at 25°C. What…

A: Given : Ecell = 0.300 V Temperature = 25 oC Concentration of Ni2+, [Ni2+ ] = 1.0 M And Eocell =…

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: We know using the standard reduction potential we can calculate E° cell After calculating the E°cell…

Q: Calculate the potential measured for the following cell at 298 K. Cr(s) | Cr3+(aq) (0.0055 M) ||…

A: Given data: The cell reaction is Cr(s) I Cr3+(aq) (0.0055 M) ∥ Ni2+(aq) (1.27 M) I Ni(s) The…

Q: Given that standard reduction potentials at 298.15 K are E° Ag+ /Ag = +0.800 V and E° Cu?"/Cu =…

A: When Ag foil is soaked into Cu(NO3)2 solution, for Ag to dissolve the reaction involved would be:…

Q: The following standard reduction potentials have been determined for the chemistry of indium:…

A: The objective of the question is to calculate the cell potential, E°, and the equilibrium constant,…

Q: 7. Using the standard reduction potentials given below, answer each question. A2 (aq) + e- = A*(aq)…

A: Reduction is gaining of electrons. Oxidation is lose of electrons. Redox reactions are those where…

Q: Use standard reduction potentials to calculate the equilibrium constant for the reaction: Pb2*(aq) +…

A: The solution is as follows :

Q: What is the standard cell potential for the cell: Al|Al3+ (1M) || Fe2+ (1M) |Fe? E° for Al / Al3+…

Q: The standard reduction potential E° for the reduction of permanganate in acidic solution is +1.51 V.…

A: Given, E° for reduction of permanganate in acidic solution is +1.51 V. We have to calculate the…

Q: Consider the following reduction half-reactions: MnO4 (aq) + 8 H*(aq) + 5 e¯ = Mn²+ (aq) + 4H₂O(1)…

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: Voltage can be calculated as follows

Q: wing reduction equations and their associated standard reduction potentials, E", determine the…

A: Galvanic cell: It is a kind of cell n which electric current s produced due to the redox reactions…

Q: The free energy change for the following reaction at 25 °C, when [Fe²+] = 1.18 M and [Cr³+] =…

A: an electrochemical cell reaction is an example of redox process

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

A: E°cell = E°red cathode - E°red anode here anode is Fe because it has less reduction potential and…

Q: Which of the following substances is the strongest oxidizing agent?

A: Oxidizing agent are substances which reduces itself and oxidizes other species.

Q: Cr3+(aq) + 3e- à Cr(s) -0.763 V Au+(aq) + e- à Au(s)…

A: Given reactions are : Cr3+(aq) + 3e- -------------> Cr(s) E0 = -0.763…

Q: 11. Consider the following reaction and its AG-AGo at 25.00 °C. 2Ag(aq)+Cu(s) 2Ag(s)+Cu*(aq) AG…

A: Given reaction is : 2Ag+ (aq) + Cu (s) ------------> 2Ag (s) + Cu2+ (aq) , ΔG0 = -88660 J/mole…

Q: AlF63-(aq)

A: Al3+ (aq) + 3e- -------> Al(s) ......E°(reduction) = -1.66 V AlF63-(aq) + 3e- ----> Al(s) +…

Question

Q7. Calculate the equilibrium constant at 25°C for the reaction
2Fe (aq) 21 (aq)-2Fe²(aq) +1₂(s)
Given the standard reduction potentials:
2Fe2e2Fe² E-0.771 V
E-0.5355 V
B) 9.16
1₂ +2e21
A) 18.3
C) 9.10x10 D) 9.54x10 E) 2.9x10²

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

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2Cu²+ u²+ (aq) + 21- (aq) → 2Cut (aq) + 12 (8) 2+ Cu²+ (aq) + e → Cut (aq) Ee red I2 (s) +2e → 21¯ (aq) AGO = K for this reaction would be kJ E red - 0.153 V 0.535 V than one.
Plese don't provide handwritten solution
Consider the following cell. Cr | Cr³+ (1.00 M) || Ni²+(1.00 M) | Ni & = 0.68 V (a) How many milligrams of metallic nickel would be plated on the cathode if a current of 0.16 A is drawn for 1.3 hrs? 4.0 2.3e2 mg (b) What is the Cr³+ concentration when the Ni²+ concentration has dropped to 1.0 × 10-4 M? 4.0 33 X M What is the cell potential at this point? 4.0 0.666 X V
The free energy change for the following reaction at 25 °C, when [Cd2*] = 1.17 M and [Cr+] = 8.47x10-3 M, is -207 kJ: 3ca**(1.17 M) + 2Cr(s)3Cd(s) + 2Cr³+(8.47x103 M) AG = -207 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
True or False: The reaction, S₂082- + Ni(OH)2 + 2OH2SO42- + NiO2 + 2H₂O, will occur spontaneously under standard state conditions. Following are the standard reduction potentials that may be useful: NiO2 + 2H₂O +2e=Ni(OH)2 +2OH E = 0.49 V S2082 +2e=2SO4²- True False E° = 2.01 V
Given the standard reduction potentials: Zn2*(aq) + 2e- Zn(s) Ag*(aq) + e + Ag(s) E°=-0.76 V E°= 0.80 V Which species is the best oxidizing agent? Ag(s) O Ag*(aq) O Zn(s) O Zn2*(aq)
3.) Consider the following standard reduction potentials, which statement is correct at standard conditions? Ni?* (aq) + 2 e → Ni (s) E°red = -0.26 V I2 (s) + 2 e -> 2 (aq) E°red = 0.54 V I. Ni²* (aq) is a stronger oxidizing agent than I2 (s), and I is a stronger reducing agent than Ni (s) II. I2 (s) is a stronger oxidizing agent than Ni2", and Ni (s) is a stronger reducing agent than I (aq) III. Ni (s) is a stronger oxidizing agent than I (aq), and Ni2* is a stronger reducing agent than I2 (s) IV. I(aq) is a stronger oxidizing agent than Ni (s), and I2 (s) is a stronger reducing agent than Ni2+ (aq) А. IV В. Ш С. П D. I
Consider the following standard reduction potentials: F2(g) + 2 e - 2 F (aq) E° = +2.87 V Mg2*(aq) + 2 e - Mg(s) E° = -2.37 V Under standard conditions, O Mg(s) is a stronger oxidizing agent than F (aq), and Mg2*(aq) is a stronger reducing agent than F2(g), O F (aq) is a stronger oxidizing agent than Mg(s), and F2(g) is a stronger reducing agent than Mg2*(aq). O F2(g) is a stronger oxidizing agent than Mg-"(aq), and Mg(s) is a stronger reducing agent than F (aq). O Mg2*(aq) is a stronger oxidizing agent than F2(g), and F(aq) is a stronger reducing agent than Mg(s).
1) Calculate the following for the reaction at 298.0 K . The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) A) The standard Gibbs free energy change of the reaction @ 298.0 K B) The equilibrium constant for the reaction C) The standard cell potential 2) Calculate the free energy change and the cell potential for the reaction at 298.0 K if all reactants are at 2.00 M and/or 2.00 atm and all products are at 0.0100 M and/or 0.0100 atm
Given the electrochemical reaction, Mg/ Mg 2(aq) // Zn2(aq) / Zn, E+1.61 V. If the standard reduction potential of Zn²-Zn is -0.76V. What is the standard reduction potential of Mg2+ = Mg? -2.37 V (В 0.85 V -0.85 V 2.37 V
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?
The free energy change for the following reaction at 25 °C, when [Cu2+] = 2.57x10-³ M and [I₂] = 1.10 M, is 88.8 kJ: 2Cu²+(2.57x10-3 M) + 2.001 (aq)—2Cu+ (aq) + 1₂(1.10 M) AG= 88.8 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?