Answered: For the electrochemical cell 2 Al(s) +…

For the electrochemical cell 2 Al(s) + 3 Mn2 (aq)→ 2 Al (aq) + 3 Mn(s) (E° = 0.48 V, [A3] = 1.0 M), what is the value of E when [ Mn2'] = 0.060 M? Assume T is 298 K %D %3D

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: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A: An electrochemical cell is a cell that converts chemical energy into electrical energy. There are…

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

A: A student constructs a galvanic cell.

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

Q: Consider a spontaneous concentration cell based on the following half-reactions (where "a" stands…

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

Q: When the Cu²+ concentration is 9.20×10-4 M, the observed cell potential at 298K for an…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

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

A: The objective of the question is to write the balanced equation for the overall reaction in acidic…

Q: What is K for the reaction Zn(s) + Cu²*(aq) ® Zn²*(aq) + Cu(s), given E°cell is 1.1 V at 25 °C for…

Q: For the electrochemical cell 2 Au³⁺(aq) + 3 Zn(s) → 3 Zn²⁺(aq) + 2 Au(s) (E° = +2.260 V, [Zn²⁺] =…

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

Q: When the Ag concentration is 1.49 M, the observed cell potential at 298 K for an electrochemical…

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

A: Use Nernst equation to calculate the emf of the cell: Ecell = Eocell - 0.0592n log Q where,…

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A: Given, 2Al(s) + 3Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M),…

Q: Use measured cell potential to calculate concentration. When [ Hg2+ ] = 1.46 M, the observed cell…

A: Given, Hg2+(aq) +Mn(s)→Hg(l) +Mn2+(aq) [Hg2+]=1.46MEcell=2.150 V

Q: The free energy change for the following reaction at 25 °C, when [Zn²+] = 4.75×10³ M and [Ni2*] =…

A: Answer: These questions are based on relationship between Gibbs free energy change and cell…

Q: What is the cell notatio of the reactions: Fe3+(aq) + 3e- → Fe(s) Eo=-0.036 V and…

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

A: Given, AgCl s + e- → Ag s + Cl- aq E°red = 0.2223 V…

Q: For the galvanic (voltaic) cell Cd²"(aq) + Fe(s) → Cd(s) + Fe²"(aq) (E° = 0.0400 V), what is the…

A: we have given the reaction as follow Cd2+ + Fe → Cd + Fe2+…

Q: What is the maximum amount of work that can be done by an electrochemical cell where E° = 2.23 V and…

Q: When [Hg2+1 = 1.47 M, the observed cell potential at 298 K for an electrochemical cell with the…

Q: For the electrochemical cell described, what is the value of E when [Sn²⁺] = 0.25 M? Assume T is 298…

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

A: The objective of this question is to calculate the standard free energy for the reaction in the…

Q: What is the potential (in V) of the following electrochemical cell? Al(s) | Al³"(0.0100 M) ||…

Q: The redox reaction for the electrochemical cell at 25°C was given below: I2(s) + Ag(s) → 21aq) +…

Q: Determine the cell potential for an electrochemical cell (not standard condition, E) based on…

A: GIVEN: Reactions: To Solve: Cell potential for an electrochemical cell=?

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

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

A: The given question can be easily solved with the prior knowledge of the Nerst Equation. It relates…

Q: Imagine an electrochemical cell established from the following half cells, linked by a KCI salt…

A: We have given that 1. a Fe electrode in 2.0M FeCl2 2. a Ni electrode in 2.0M Ni(NO3)3 Ni2+ +…

Q: Determine E° for the reaction AI(s) + 3 Ag*(aq) → 3 Ag(s) + Al³*(aq). Standard Reduction E° (V)…

Q: For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the…

A: The reaction given is Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) Hence in the above reaction, Cd2+ is…

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

A: Answer: Galvanic cell is a type of cell that converts chemical energy into electrical energy via…

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

A: The solution is as follows :

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

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

A: The balanced chemical equation is given as:- 3Cl2(g) + 2Fe(s) → 6Cl- + 2Fe3+ Cl2(g) + 2e- →…

Q: Calculate the Ecell value at 298 K for the cell based on the reaction: Cu(s) +2Ag*(aq) Cu²+ (aq)…

A: Nernst equation :- The relationship between cell potential and concentration of electrolytes is…

Q: 0.115 V, what is the value of the standard free energy (in kJ) for this reaction?

Q: If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2…

A: The Nernst equation is given as :

Q: For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0…

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V…

A: The cell's feasibility as well as potential are estimated using Nernst equation which derives the…

Q: For the galvanic (voltaic) cell Cu(s) + Mn²⁺(aq) ⟶ Cu²⁺(aq) + Mn(s) (E° = 0.60 V at 25°C), what is E…

Q: For the electrochemical cell 2 AI(s) + 3 Mn²*(aq) → 2 Al*(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0…

A: Nernst equation for the given reaction is : Ecell = E°cell -…

Question

100%

For the electrochemical cell 2 Al(s) + 3 Mn² (aq)→ 2
Al (aq) + 3 Mn(s) (E° = 0.48 V, [AI3] = 1.0 M), what is
the value of E when [ Mn2] = 0.060 M? Assume T is
| v
298 K
1
3
4
C
7
8
9.
+/-
x 100
59°F Cloudy A ODA a 40 10:54 AM
AL
H.
Alt
Alt
el

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

A electrochemical cell is made by considering the following unbalanced redox reaction: Pb2+(aq) + Fe(s) → Fe3+(aq) + Pb(s) The cell voltage, Ecell, at 298 K, when [Pb2+] = 0.25 M and [Fe3+] = 0.15 M, is nonspontaneous? Is the reaction spontaneous or
A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCl(s) + e → Ag(s) + Cl(aq) Eºred = 0.2223 V And a copper electrode with 0.500 M Cu²+ as the second half cell Cu²+ (aq) + 2 e → Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0595 V. Write the balanced equation for the overall reaction in acidic solution.
Decide whether or not each metal dissolves in 1 mol L-1 HIO3(aq). Standard Electrode Potentials at 25 °C Reduction Half-Reaction E° (V) Au3+ (aq) +3e → Au(s) 1.50 IO3 (aq)+6H+(aq) + 5e7 →12 (s) + 3H2O(1) 1.20 Ni²+(aq) + 2e → Ni(s) -0.23
For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M), what is the value of E when [ Mn²⁺] = 0.089 M? Assume T is 298 K
For the electrochemical cell 2 Al(s) + 3 Mn²⁺(aq) ⟶ 2 Al³⁺(aq) + 3 Mn(s) (E° = 0.48 V, [Al³⁺] = 1.0 M), what is the value of E when [ Mn²⁺] = 0.018 M? Assume T is 298 K
A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e¯ → Ag(s) + Cl¯(aq) E°red = 0.2223 V And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0903 V. What is the standard cell potential for this cell in V?
Calculate E and G for the following electrochemical cell at 25°C, Pt | H₂(g) (1.0 atm) | H+ (0.010 M) || Agt (0.020 M) | Ag if E°(H+) = +0.000 v and E°(Ag +) = 0.799 V.
For the galvanic (voltaic) cell Cd²⁺(aq) + Fe(s) ⟶ Cd(s) + Fe²⁺(aq) (E° = 0.0400 V), what is the ratio [Fe²⁺]/[Cd²⁺] when E = 0.001 V? Assume T is 298 K
At 298 K, what is E (in V) for the electrochemical cell below when [Cd2+] = 4.500 M and [Cu2+] = 0.009 M ? Cd(s) | Cd2+(aq) || Cu2+(aq) | Cu(s) Cu2+ (aq) + 2e– → Cu(s) 0.34 Cd2+ (aq) + 2e– → Cd(s) –0.40
Consider the following electrochemical cell at 298 K where the source of Cu2+ (aq) is the sparingly soluble salt CuX. Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s) Zn2* + 2e = Zn E° = -0.76 V Cu2+ + 2e = Cu E° = 0.34 V If the potential created from this cell = 1.03 V, what is Ksp for CuX? O 1.9x10-9 3.8x10 12 4.6x10 6 2.0x10 7
For the electrochemical cell 2 Al(s) + 3 Mn2*(aq) – 2 Al**(aq) + 3 Mn(s) (E° = 0.48 V, [AI3*] = 1.0 M), what is the value of E when [ Mn2*] = 0.091 M? Assume T is 298 K %3D
For the electrochemical cell 2 Al(s) + 3 Mn²+ (aq) → 2 Al³+ (aq) + 3 Mn(s) (E° = 0.48 V, [A1³] = 1.0 M), what is the value of E when [Mn²+] = 0.026 M? Assume T is 298 K