When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.806 V. What is the Mg2+ concentration in this cell? Cu²+ (aq) + Mg(s) →→→ Cu(s) + Mg²+ (aq)

When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the reaction shown below is 2.806 V. What is the Mg2+ concentration in this cell? Cu²+ (aq) + Mg(s) →→→ Cu(s) + Mg²+ (aq)

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

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

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

A: we have to calculate the cell potential

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

A: Thank you,Please rate my response.

Q: A galvanic cell is prepared using aluminum and nickel follows the cell notation Al(s) | AI3+(aq) ||…

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

Q: An electrochemical cell is constructed using a copper cell as the anode and the bromate/bromide cell…

A: The balanced redox reaction involved:3 Cu(s) + BrO3–(aq) + 6 H+(aq) → 3 Cu2+(aq) + Br–(aq) + 3…

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

A: [Co2+]=0.00190 M[Au3+]=0.896 MT=25oC=25+273=298K

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: Consider these two entries from a fictional table of standard reduction potentials.…

A: We have to calculate the standard potential of cell.

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: Write the cell notation for an electrochemical cell consisting of an anode where H2 (g) is oxidized…

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

A: Given potentials are reduction potentials. X E°= -1.65 V Y E° = 0.38 V Standard cell…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: In this question, we want to determine the standard reduction potential of the cell. You can see…

Q: Fe (s) + 2H+ (aq) → Fe²+ (aq) + H₂(g) Express your answer in volts to two decimal places. E cell =…

A: We have to calculate the standard cell potentials of the redox couples.

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

A: STEP 1: To calculate the cell voltage of the galvanic cell under the given conditions, we will use…

Q: Consider these two entries from a fictional table of standard reduction potentials.…

A: Concepts The question is based on calculating the overall standard cell potential, for the given…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg² +] = 0.755 M…

A: Given,

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: 1)A voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The…

A: We know that for any voltaic cell, the cell potential is given by : E = Eo - (RT/nF) ln Q Where Q=…

Q: Alkaline dry-cell batteries have a voltage of 1.50 V under standard conditions. Given this standard…

A: Chemically, a typical alkaline dry cell battery has a zinc anode and a manganese dioxide cathode.…

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

Q: A galvanic cell has the overall reaction: 2Cu+(aq) + Pb(s) → 2Cu(s) + Pb2+(aq) Which is the half…

Q: Mg(s) + Fe²+ (aq) →→ Mg²+ (aq) + Fe(s) The galvanic cell described above has a standard cell…

A: Given that the galvanic cell reaction is Mg(s) + Fe+2 (aq) ----------> Mg+2 (aq) + Fe (s)

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

Q: When the Cu²+ concentration is 1.37 M, the observed cell potential at 298 K for an electrochemical…

A: Given -> [Cu2+] = 1.37 M Ecell = 1.616 V Cu2+(aq) + 2e- --------> Cu(s) E°cell = 0.337 V…

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: When the Hg2+ concentration is 8.04x10-4 M, the observed cell potential at 298K for an…

A: According to given questionfirst standard cell potential calculationsecond concentration calculation…

Q: Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following…

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

When [Cu²+] = 1.49 M, the observed cell potential at 298 K for an
electrochemical cell with the reaction shown below is 2.806 V. What is the
Mg2+ concentration in this cell?
2+
Cu²+ (aq) + Mg(s)→→ Cu(s) + Mg²+ (aq)
[Mg2+1 = 8.11x10^-5 X mol/L

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

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

The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V. If [Au³+] = 0.50 M, what is the concentration of Cu2+? (R = 8.314 J/K mol, F = 96,500 C.mol-¹) 3Cu + 2Au3+→ 3℃u²+ + 2Au O 1.61 M O1.37 M O 258 M O 5.16 M
3) The standard potential for the following galvanic cell is +0.90 V: 3 Cu2+ (aq) + 2 Ga(s) ⇒ 3 Cu(s) + 2 Ga³+ (aq) Given that the standard reduction potential for the Cu2+/Cu half-cell is +0.34 V, what is the standard reduction potential for the Ga3+/Ga half-cell?
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Al(s) ∣ Al3+(aq), 0.115 M|| Al3+(aq), 3.89 M)∣Al(s)
A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a cell potential of 0.763 V. Calculate the maximum electrical work generated when 17.0 g of zinc metal is consumed. Maximum electrical work-
Consider a galvanic electrochemical cell constructed using Cr/Cr³⁺ and Zn/Zn²⁺ at 25 °C. The following half-reactions are provided for each metal: Cr³⁺(aq) + 3 e⁻ → Cr(s) E°red = -0.744 V Zn²⁺(aq) + 2 e⁻ → Zn(s) E°red = -0.763 V Given that the standard cell potential is 0.019 V and the overall equation is 2 Cr³⁺ (aq) + 3 Zn (s) → 2 Cr (s) + 3 Zn²⁺ (aq), what is the cell potential for this cell at 25 °C when [Zn²⁺] = 0.0323 M and [Cr³⁺] = 0.1736 M?
Calculate the equilbrium constant, K, for the reaction
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?
4)A galvanic cell is constructed that uses the following half-cell reactions: Cu+(aq) + e−→ Cu(s) I2(s) + 2e−→ 2I−(aq) a)Determine the cell potential for the spontaneous reaction under standard conditions. b)If the cell in part a is operated at 298 K with [Cu+] = 2.5 M and [I−] = 3.5 M, calculate the cell potential. Is the reaction spontaneous under these conditions? Explain. c)If [Cu+] was equal to 1.4 M, at what concentration of I− would the cell have zero potential?