A cell employs the following half-reactions. Ni(s) Eº2+ = -0.25 V Cr(s) E°3+ = -0.74 V Ni Calculate the potential if [Ni2+] = 1.0 x 104 and [Cr³+] = 2.0 x 10-³ M. Ni²+ (aq) + 2 e Cr³+ (aq) + 3 e

A cell employs the following half-reactions. Ni(s) Eº2+ = -0.25 V Cr(s) E°3+ = -0.74 V Ni Calculate the potential if [Ni2+] = 1.0 x 104 and [Cr³+] = 2.0 x 10-³ M. Ni²+ (aq) + 2 e Cr³+ (aq) + 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: The reaction is 2 SmCl3(aq) + 6 LiCl(aq) + 6 e- → 2 Sm(s) + 6 Li+(aq) + 6 Cl-(aq) Calculate the…

A: Answer: The free energy change for the given reaction is0 J/moland the cell potential is-1.35 Vat…

Q: Given the two following half reactions, Cr3+(aq) + 3e- → Cr(s) E˚ = -0.76 V Hg22+(aq) +…

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

Q: Calculate the value of the cell potential, E cell for the following reaction: 2 Au(s) + 3 Ca2+(aq)-…

Q: rom a table of Standard Reduction Potentials: Fe2+(aq) + 2 e- → Fe(s) E = -0.447 V…

A: Standard electrode potential is the measurement of the potential for the equilibrium and the…

Q: 6) A galvanic cell is composed of these two half-cells, with the standard reduction potentials…

A: It is based on the concept of electrochemistry. Here we are required to find the standard Gibbs…

Q: Avoltaic cell is constructed using this reaction Ni(s) + 2 H+ → Ni2+ + H2(g) The cell potential at…

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

Q: [References] A particular voltaic cell operates on the reaction Zn(s) + Cl2 (g) → Zn²+ (ag) + 2CI…

A: The solution is as follows :

Q: What is the cell potential given the balanced redox reaction? 2+ Mg6) + Cu?+ → Cu(s) + Mg“ (aq) (aq)…

A: The answer to the following questions is-

Q: Calculate ΔG for the following cell reaction: 3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s) where…

A: Concept: For a cell reaction: The overall cell potential can be calculated by using the equation…

Q: Given the following standard reduction potentials: Mg+2 = Mg(s) + 2e- E = (-) 2.37 V 2e- + I2(s) =…

A: Dear student the first equuation for Mg given is wrong as Mg2+ ion can never give Mg and 2 e- .

Q: Calculate the standard free energy, ∆G, for the electrochemical cell below. Is it a galvanic or…

A: Given that : Temperature = 298 K The oxidation half-reaction is : Pb(s) → Pb2+ Adding 2 electrons…

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

Q: The standard reduction potentials for Mg2+/Mg (E'= -2.37 V) and Fe2*/Fe (E'= -0.44 V). When a piece…

A: Concept- By the help of nernst equation, this problem can be solved. Ecell=Eocell− 0.0592/n log10Q…

Q: The free energy change for the following reaction at 25 °C, when [Cd²+] = 2.15×10-³ M and [Ni2+] =…

A: It is given that standard Gibb's free energy, ∆G = 45.0 KJ

Q: Consider the following standard reduction potentials: Fe3+ (aq) + e MnO4 (aq) + 8 H*(aq) + 5e → Mn2+…

A: In this question, we will see the strongest oxidizing agent. You can see below.

Q: A chemist designs a galvanic cell from the following two half-reactions NO3 (aq) + 4H+ (aq) + 3e →…

Q: The free energy change for the following reaction at 25 °C, when [Pb²+] = 1.20 M and Zn²+ ] =…

A: Recall the given reaction, Pb2+ 1.20 M + Zn s → Pb s + Zn2+…

Q: Co2+(aq) + 2e- --> Co(s) Eo=-0.28 V Cd2+(aq) + 2e- --> Eo= -0.33 V What is the standard free…

Q: The following half reactions are used for a galvanic cell: Zn2+(aq)+2e-→Zn(s)E°=-0.76V…

A: Nerst Equation:Where,E is the cell potential under non-standard conditions.E∘ is the standard cell…

Q: When [Cu2+] = 1.24 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: The overall cell reaction : Cu2+(aq) + Zn(s) ---> Cu(s) + Zn2+(aq) The observed cell potential…

Q: Which of the following statements is true concerning the electrochemical cell depicted below? M…

A: According to the representation of the given electrochemical cell the complete red-ox reaction is:…

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

A: Given that : A student constructs an electrochemical cell with a half-cell composed of a nickel…

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

A: Given Reactions: O2 (g)+ 4 H+ +4 e- ------> 2H2O Eored= +1.23 V…

Q: standard cell potential f

Q: Determine the cell potential for the following reaction: Hg2+ + 21- Hg + 12 Given the following…

Q: The free energy change for the following reaction at 25 °C, when [Ni²+] = 1.15 M and [Cd²+] =…

A: Given,

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) = Ti²(aq)…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

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

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

A cell employs the following half-reactions.
Ni(s) Eº2+ = -0.25 V
Cr(s) E°3+ = -0.74 V
Ni
Calculate the potential if [Ni2+] = 1.0 x 104 and [Cr³+] = 2.0 x 10-³ M.
Ni²+ (aq) + 2 e
Cr³+ (aq) + 3 e

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps

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

Galvanic cell has 2 half reactions O2(g) + 4H+(aq) + 4e- → 2H2O(l) E0red = +1.23 V Cr3+(aq) + 3e- → Cr(s) E0red = -0.74 V Write a balanced equation that describes the cell, ensuring that E0cell > 0 V and Calculate E0cell
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your Ov answer to 2 significant digits.
Plese don't provide handwritten solution
Consider the following standard reduction potentials in acid solution: Co2+ + 2e– ----> Co (s) E° = –0.28 V MnO4– + 8H+ + 5e– ---> Mn2+ + 4H2O E° = +1.51 V The strongest reducing agent listed above is:
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M and [Fe2+] = 0.0170 M. Use the standard reduction potentials in this table. Cr(s) + Fe²+(aq) Cr² (aq) + Fe(s) E = x10 TOOLS V
Given the following electrochemical cell, calculate the potential for the cell in which the concentration of Ag+ is 0.0765 M, the pH of the H* cell is 2.700, and the pressure for H₂ is held constant at 1 atm. The temperature is held constant at 55°C. Ag Ag+ H+ Standard reduction potentials: 2H+ +2e¯ → H₂ Eº = 0 V Ag+ le - H₂(g) → Ag Eº=0.800 V
A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo = 0.34 V. If the cell contains 0.00178 M concentrations of HCl and CuSO4, what potential does it produce?
Determine E cell at 298 K when [Ni2+] = 0.33 M and [Ag+] = 0.51 M. Ni2+(aq) + 2e- -> Ni(s) Eredo =-0.257V Ag+(aq) + e- -> Ag(s) Eredo =+0.7996V
Which of the following reactions occurs at the anode of an electrochemical cell composed of Zn│Zn2+(aq) and Fe│Fe2+(aq) half-cells? Their reduction potentials are as follows: Zn2+ + 2e– --> Zn; Eo = -0.763 V Fe2+ + 2e– --> Fe; Eo = -0.447 V (A) Zn2+ + 2e– --> Cr; (B) Zn --> Zn2+ + 2e–; (C) Fe --> Fe2+ + 2e–; (D) Fe2+ + 2e– --> Fe;
Which of the following pairings is CORRECT? Obronze - compound gravel - homogeneous mixture Osolid iodine - atom Obromine gas - molecule white wine - heterogeneous mixture