Refer to the following standard reduction half-cell potentials at 25° C: Ni?+ (aq) + 2e VO2 (aq) + 2H*(aq) + → Ni(s) → VO² (aq) + H2O(1) E° = -0.23 V e E° = 0.99 V Part A An electrochemical cell is based on these two half-reactions: Ni(s) → Ni²+ (aq, 2.5M) +2e Reduction: VO2 *(aq, 0.031M) + 2H*(aq, 1.1M) + e → VO²*(aq, 2.5M) + H2O(1) Oxidation: Calculate the cell potential. Express your answer to two decimal places and include the appropriate units.

Refer to the following standard reduction half-cell potentials at 25° C: Ni?+ (aq) + 2e VO2 (aq) + 2H(aq) + → Ni(s) → VO² (aq) + H2O(1) E° = -0.23 V e E° = 0.99 V Part A An electrochemical cell is based on these two half-reactions: Ni(s) → Ni²+ (aq, 2.5M) +2e Reduction: VO2 (aq, 0.031M) + 2H(aq, 1.1M) + e → VO²(aq, 2.5M) + H2O(1) Oxidation: Calculate the cell potential. Express your answer to two decimal places and include the appropriate units.

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: Consider these two entries from a fictional table of standard reduction potentials. X³+ + 3 e y³+ +…

Q: Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced…

A: The given two half-reactions are:NO3−+4H++3e−→NO+2H2O Eredo=0.96VCu2++e−→Cu+…

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential (Eᵒcell)…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e- →…

A: We have two half cell reaction: X3+ + 3e- ----> X(s) E°= -1.61 V Y3+ + 3e- ---->…

Q: Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced…

Q: Consider the following standard reduction potentials Ag+(aq) + e-→Ag(s)…

Q: Given the following half-reactions and half-cell potentials, write the balanced overall…

Q: Standard reduction potentials at 25°C NO3(aq)+4H+(aq) +3e¯→ NO(g) +2H2O(1) Na+ (aq)+eNa(s)…

A: Step 1: An electrochemical cell is an apparatus that is used to generate electricity from a…

Q: Mg2"(aq) + 2 e Mg(s) E° = -2.38 V Cu2*(ag) + 2 e Cu(s) E° = +0.34 V O-2.04 V O +2.72 V O+2.04 V…

A: Given : Mg2+ (aq) + 2e- ==> Mg(s) E° = -2.38 V Cu2+ (aq) + 2e- ==> Cu (s) E° =…

Q: Using the following standard reduction potentials, Fe3+(aq) + e- → Fe2+(aq) E° = +0.77 V Cu2+(aq) +…

A: The standard cell potential (Eocell) for the cell is determined using the following equation…

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

Q: half-reaction standard reduction potential Br,()+2e 2 Br (aq) E =+1.065 V red MnO (aq)+8H (aq)+5e Mn…

A: The half cell for which the value E°red is higher, will be preferred as the cathode. Here, MnO4-…

Q: Calculate the potential (emf) of a working galvanic cell that is based on these two half cells and…

A: Answer -

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

Q: In the following electrochemical cell, which is the half reaction at the cathode? 2 Ag + ( aq) + Ni…

A: 2 Ag + ( aq) + Ni ( s) → 2 Ag ( s) + Ni 2+ ( aq) Standard Reduction Potentials Ni 2+ ( aq) + 2 e -…

Q: A certain half-reaction has a standard reduction potential Ed=-0.06 V. An engineer proposes using…

Q: the standard half cell potentials to calculate the standard cell potential (E°cell ) for the…

A: -> 2Fe2+(aq) + Ni2+(aq) -----> 2Fe3+(aq) + Ni(s) Equation for reduction of Fe3+ is written…

Q: A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that…

A: The galvanic cell consists of two half-cell ; at one half cell oxidation reaction occurs and at the…

Q: You are shown a voltaic cell in which the cathode is Cu and the anode is an unknown metal, X. You…

A: Given Anode (oxidation half cell) X(s) -------> X2+ + 2e- E°ox = ? Cathode (reduction half…

Q: Find

A: We will calculate reduction potential

Q: n a Voltaic cell composed of CuôCu(NO3)2 and AgôAgNO3 half-cells, if the concentration of the…

A: We have given that [Ag+] = 1.0 x 10–5 M and [Cu2+] = 1.0 M Therefore from electrochemical series of…

Q: Calculate the standard state cell potential for the reaction below given the standard reduction…

A: To solve this problem we need to write the oxidation half and reduction half reaction and According…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e → X(s)…

Q: A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown:…

Q: calculate the standard cell potential (E°cell )

Q: Consider the following two half-reactions and their standard reduction potentials for a voltaic ce…

A: Electrode for which the value of reduction potential is higher has higher chances of being reduced.…

Q: Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard…

A: Given: Half-cell reactions: Cu+2 (aq) + e- → Cu+ (aq) Eo = +0.15 V V+2 (aq) + 2e- → V (s)…

Q: A galvanic cell is based on the following half-reactions (both written as reductions) at 25 °C: VO₂+…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

Q: Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Given the standard reduction potentials, which combination in the answer choices below would produce…

A: Given data:Which combination produces the lowest cell voltage?Standard reduction potential is the…

Q: Standard tables of reduction potentials assume standard conditions, but many electrochemical cells…

A: Using nernst equation, we will calculate cell potential at given concentrations.

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

A: Use Nernst equation, to get the cell potential:

Q: The two half cells that make up a battery are shown below with their reduction potentials Br2(aq) +…

A: ->The species which has large reduction potential that tends to reduce and oxidize other species.…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Refer to the following standard reduction half-cell potentials at 25° C:
Ni?+ (aq) + 2e
+ Ni(s)
- VO²+ (aq) + H2O(1)
E° = -0.23 V
VO, + (aq) + 2H*(aq)
E° = 0.99 V
e
Part A
An electrochemical cell is based on these two half-reactions:
Ni(s) → Ni²+ (aq, 2.5M) + 2e
Reduction: VO, *(aq, 0.031M) + 2H*(aq, 1.1M) +e → VO²+ (aq, 2.5M) + H2O(1)
Oxidation:
Calculate the cell potential.
Express your answer to two decimal places and include the appropriate units.

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 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 E°cell for the cell for the reaction 2 Ga(s) + 3 Sn4+(aq) → 3 Sn2+(aq) +2 Ga3+(aq).The standard reduction potentials are as follows: Ga3+(aq) + 3 e− → Ga(s) E° = –0.55 V Sn4+(aq) + 2 e− → Sn2+(aq) E° = 0.15V
Use the standard reduction potentials given below to predict if a reaction will occur between Ag(s) and F2 (g), when the two are brought in contact via standard half-cells in a voltaic cell. F2 (g)+2e7 →2F (aq) E red Agt (ag)+e → Ag(s) E red + = If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - 2.870 V 0.799 V +
Consider the following two half-reactions and their standard reduction potentials for a voltaic cell. N2O(g)+2H+ (aq)+2e-N2(g)+H2O(l) E° = 1.766 V MnO-4(aq)+4H+ (aq)+3e-MnO2(s)+2H2O(l) E° = 1.673 V 3N2O(g)+2MnO2(s)+H2O(l)3N2(g)+2MnO- 4(aq)+2H+(aq) Calculate the value of AG for the reaction above.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e - 2 Br (aq) =+1.065 V ʼred MnO,(aq)+2 H,O(1)+3e MnO,(s)+4 ОН (аq) E=+0.59 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.
Use the standard reduction potentials given below to predict if a reaction will occur between Zn(s) and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. | Cl2(g) + 2e¯¯ →2C1¯¯ (aq) E Zn2+ = 1.360 V red (aq) + 2e → Zn(s) E = = -0.763 V red If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + +
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction |HNO₂(aq)+H*(aq)+e¯ - →>> NO(g) + H2O(l) Fe3+(aq)+e → Fe (aq) Fe2+(aq) Answer the following questions about this cell. standard reduction potential +0 Ε = +1.00 V 0 red Ered = +0.771 V
Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag^+(aq)+e^-→Ag(s) What mass of silver plates onto the cathode when a current of 7.9 A flows through the cell for 73 min ?
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
This galvanic cell uses the reaction: Cu(s) + 2 Ag*(aq) → 2 Ag(s) + Cu2+(aq). f a C oxidation half cell reduction half cell Identify the composition of electrodes and the direction of electron flow. O a is Ag, c is Cu and electrons flow from c to a O a is Ag, c is Cu and electrons flow from a to c O a is Cu, c is Ag and electrons flow from c to a. O a is Cu, c is Ag and electrons flow from a to c. an
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V