Use cell potential to calculate an equilibrium constant.Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:Cu2*(aq) + Hg(l)–→ Cu(s) + Hg²*(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off errorwhen taking the antilogarithm.Equilibrium constant:

Answered: Image /qna-images/answer/457d35e0-bd83-4101-bc37-d8bc966df818.jpg

Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: 2+ Cu²*(aq) + Hg()→ Cu(s) + Hg²*(aq)

Use cell potential to calculate an equilibrium constant. Calculate the cell potential and the equilibrium constant for the following reaction at 298 K: 2+ Cu²(aq) + Hg()→ Cu(s) + Hg²(aq)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...

See similar textbooks

Related questions

Q: Given the standard reduction potentials for an element A, at 25 °C: А2"(аg) + е > A (ag) E1° = 1.09…

A: Standard cell potential is an intensive property which does not depend on amount or mass of the…

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

A: Cu(s) ∣ Cu2+(aq, 0.0032 M) ∣∣ Cu2+(aq, 4.48 M) ∣ Cu(s)We need to calculate the cell potential for…

Q: Calculate the equilibrium constants from the following reactions at 25 C. You must first calculate…

Q: The equilibrium constant, K, was found to be 3.8 x108 at 25°C for the following reaction, 2X(s) +…

A: For the given reaction: 2X(s) + 3Y2+(aq) →2X3+ + 3Y(s) As the charges are equal on both sides.…

Q: Calculate the standard cell potential, Ecell°, for the reaction shown. Use these standard reduction…

A: The standard cell potentials are= For the Cu+| Cu half cell = 0.521 V For the Ag+ |Ag half cell =…

Q: Write the cell reaction and electrode half-reactions and calculate the standard emf of the following…

A: The objective of the question is to write the cell reaction and electrode half-cell reactions and…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: Note: Since you have posted a question with multiple subparts, we will solve the first three…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr** (ag)+…

A: The given reaction is, 2Cr3+aq+3Cas→2Crs+3Ca2+aq The half cell reactions and their standard…

Q: Consider an electrochemical cell based on the following cell diagram: Pt | Pu3+(aq), Pu4+(aq) ||…

Q: Calculate the equilibrium constants of the following reactions at 25°C from standard potential data…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: NOTE: “Since you have posted a question with multiple sub-parts, we will solve first three subparts…

Q: The following redox reaction was performed under non-standard conditions. Zn(s) + Cu2+(aq) →…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: Calculate the standard cell potential, E, for the equation cell Cr(s) + F, (g) – Cr*(aq) + 2F (aq)…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Zn (s) is oxidized…

A: electrochemical cell is a device which generates electrical energy from chemical emery , in…

Q: Fe(s) Fe²+ (aq) || MnO4 (aq), Mn²+ (aq)| Pt(s) | Write the half reactions: Oxidation: Reduction: Net…

A: Given in following question a cell reaction Fe(s)/Fe+2(aq)//Mno4-(aq),MN+2 /pt thus cell…

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

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr (aq)…

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2 E0= -2.87…

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a) E=+0.61V B) E=+0.16V

Q: Using values from the table of standard reduction poten- tials, calculate the cell potentials of the…

A: The reduction potential of the cell is calculated by using the electrode potential of the cathode…

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

A: The electrochemical cell consists of two half-cell reactions where there is oxidation and reductions…

Q: Calculate the standard cell potential, ?∘cell, for the equation Zn(s)+F2(g)⟶Zn2+(aq)+2F−(aq) Use…

Q: Calculate the standard cell potential, Ee, for the equation Sn(s) + F,(g) → Sn²+(aq) + 2F¯(aq) Use…

A: Standard reduction potential can be obtained using its respective table. We know more negative…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: a.)

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr** (aq) +…

A: Given reaction is , 2Cr3+(aq) + 3Ca(s)----> 2 Cr(s) +3 Ca2+(aq) Nernst equation for the…

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

Q: half-reactions

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

A: Cus|Cu+2aq,0.0032M∥Cu+2aq,4.48M|Cus∗The oxidation reaction is; Cu→ Cu+2+2e-∗The reduction…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2+ Sn²+…

Q: 2. Using values from the table of standard reduction potentials, calculate the cell potentials of…

A: (a) Ga (s) I Ga+3 (aq) II Ag+(aq) I Ag (s) Ga (s) -->Ga+3(aq) + 3e- is oxidation. E0 reduction…

Q: . Using values from the table of standard reduction potentials, calculate the cell potentials of the…

A: The cell potential can be calculated as follows: E0cell = E0cathode – E0anode.

Q: Using values from the table of standard reduction potentials, calculate the cell potential (in V) of…

A: An electrochemical cell is a cell which is used to concert chemical energy to electrical energy Two…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2vo (aq)+4H…

A: There are two half cell reactions in an electrochemical cell which occur in the oxidation half cell…

Q: standard reduction potential, standard oxidation potential, and standard cell potential. Explain…

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

Q: Calculate the cell potential for the following reactions and predict whether the reaction will take…

A: Zn + 2 Ag+ (aq) ------> Zn2+ + 2Ag At anode ( oxidation) Zn -----> Zn+2 + 2 e- Eoxd =…

Q: Consider the reaction below: 2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a.…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr** (aq)+…

A: The cell reaction taking place is given as, => 2 Cr3+ (aq) + 3 Ca (s) -------> 2 Cr (s) + 3…

Q: A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a…

A: The given equation is, The anode reaction of given cell is, The cathode reaction of given cell is,…

Q: Calculate the standard cell potential, Ecell for the reaction shown. Use these standard reduction…

A: STANDARD CELL POTENTIAL: A cell has both cathode and anode. A positively charge electrode is known…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: Cell notation is a way to represent an electrochemical cell with anode and cathodes.

Q: The standard cell potential for the aqueous reduction of Pb4+ to Pb2+ ions by the corresponding…

A: The equilibrium constant of a reaction can be related with the standard cell potential as follows:…

Q: Calculate the standard cell potential (E°cell) of the cell: Cos)|Co2* || Au3* |Au(s) Half-reactions…

A: Given-> Co(s)/Co2+(aq)//Au3+(aq)/Au(s)

Q: Consider the following reaction and its AG° at 25.00 °C. 2 Ag*(aq)+Cu(s) → 2 Ag(s) + Cu2+(aq) AG° =…

A: ∆G = -88.66 KJ/mol = -88660 J/mol Temperature (T) = 25°C = 25+273 = 298 K R = 8.314 J/mol.K Keq =…

Q: a galvanic cell is constructed from a standard hydrogen electrode and from another hydrogen…

A: A numerical problem about galvanic cell constructed using two Hydrogen electrodes.

Q: Calculate the standard cell potential, and note whether the reaction is spontaneous under standard…

A: We have given that cell : Cu(s)│Cu2+(aq)║Au3+(aq)│Au(s) To know whether the reaction is…

Q: A voltaic cell employs the following redox reaction: 2 Fe+ (aq) + 3 Mg (s) → 2 Fe (s) +3 Mg²+ (aq)…

A: Given values [Fe^3+]=2.00M. ,. [Mg^2+]=1.6×10^-3M Nernst equation --> Ecell = E°cell -…

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

A: The cell reaction taking place is given as, => 3 Cu2+ (aq) + 2 Al (s) -------> 3 Cu (s) + 2…

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

Question

Use cell potential to calculate an equilibrium constant.
Calculate the cell potential and the equilibrium constant for the following reaction at 298 K:
Cu2*(aq) + Hg(l)–→ Cu(s) + Hg²*(aq)
Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error
when taking the antilogarithm.
Equilibrium constant:

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 3

VIEW

Step by step

Solved in 3 steps with 3 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

At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
A galvanic cell is based on the following half-reactions: In this cell, the copper compartment contains a copper electrode and [Cu2+] = 1.00 M, and the vanadium compartment contains a vanadium electrode and V2+ at an unknown concentration. The compartment containing the vanadium (1.00 L of solution) was titrated with 0.0800 M H2EDTA2, resulting in the reaction H2EDTA2(aq)+V2+(aq)VEDTA2(aq)+2H+(aq)K=? The potential of the cell was monitored to determine the stoichiometric point for the process, which occurred at a volume of 500.0 mL H2EDTA2 solution added. At the stoichiometric point, was observed to be 1 .98 V. The solution was buffered at a pH of 10.00. a. Calculate before the titration was carried out. b. Calculate the value of the equilibrium constant, K, for the titration reaction. c. Calculate at the halfway point in the titration.
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
The standard potential of the cell reaction Ag+(aq)+Eu2+(aq)Ag(s)+Eu3+(aq) is E = +1.23 V. Use the tabulated standard potential of the silver half-reaction to find the standard reduction potential for the europium half-reaction.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)