Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00385 M TIC1, and 0.0431 M TICI at 25 °C. T1³+ (aq) + 2 e TI* (aq) Ept Ept 1.2803 || Incorrect Determine the potential of a platinum electrode when placed in a mixture of 0.0173 M potassium permanganate (KMnO4) and 0.0876 M manganese chloride (MnC1₂) at pH 3.72 and 25 °C. MnO4 (aq) + 5e + 8 H* (aq) = Mn²+ (aq) + 4H₂O(1) E° = 1.25 V Incorrect E° = 1.51 V V

Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00385 M TIC1, and 0.0431 M TICI at 25 °C. T1³+ (aq) + 2 e TI* (aq) Ept Ept 1.2803 || Incorrect Determine the potential of a platinum electrode when placed in a mixture of 0.0173 M potassium permanganate (KMnO4) and 0.0876 M manganese chloride (MnC1₂) at pH 3.72 and 25 °C. MnO4 (aq) + 5e + 8 H* (aq) = Mn²+ (aq) + 4H₂O(1) E° = 1.25 V Incorrect E° = 1.51 V V

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter18: Introduction To Electrochemistry

Section: Chapter Questions

Problem 18.2QAP

See similar textbooks

Related questions

Q: A cell is constructed according to the cell diagram below. If the measured potential is 1.00 V, what…

A: Here we are required to find the pH of the dichromate cell.

Q: A galvanic cell is constructed in which the overall reaction is: Br2(1) + H2(9) → 2Brag) + 2H+…

Q: Consider the following galvanic cell: Ag(s) | Ag*(3.0 × 10“M) || Fe³*(1.1 × 10³ M), Fe²"(0.040 M) |…

A: Given,

Q: Calculate the unknown concentration of Ag+ if the potential of the following concentration cell is…

A: The unknown concentration is calculated below. Given Ecell = 300 mV = 300*10-3 V

Q: The following cell has a potential of 0.10 V at 25oC. Ni(s) | Ni2+(aq) (1.0 M) || H+ (? M) | H2(g)…

A: Ni(s) + 2 H+(aq) ⇔ Ni+2(aq) + H2 (g) Ecello = 0.23…

Q: The standard reduction potential of the permanganate ion, MnO4-, to Mn2+ is 1.51 volt, when it takes…

A: Redox potential is a measure of the tendency of a chemical species to get reduced, by accepting…

Q: A student is given two beakers in the laboratory. One beaker contains a solution that is 0.14 M in…

A: Given: [Mn3+ ] = 0.14 M [Mn2+ ] = 0.46 M [Sn2+ ] = 0.28 M And [Sn4+ ] = 0.056 M

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.0 M NISO4 solution…

A: A question based on electrochemical cell that is to be accomplished.

Q: Which of the following would give you the highest standard cell potential if used as the cathode in…

A: Ni electrode AnodeStandard Reduction PotentialNiaq2++2e-→NisE°=0.26 voltE°cell=E°cathode-E°anode.…

Q: Calculate the standard cell potential for the following galvanic cell. La(s) La (aq)|Br (1), Br…

Q: If at 25°C the standard electrode potential of the Ag/Ag' electrode is U.799 V, and the equilibrium…

A: Fe+3 + Ag ------> Fe+2 + Ag+ EoAg|Ag+= 0.799 V K = 0.531 V

Q: The standard electrode potential (E°) for Daniell cell is + 1.1 V. Calculate the AG° for the…

A: The conversion of chemical energy into electrical energy is carried out by using an electrochemical…

Q: The cell potential for Ag, AgCl | HCl (0.35M) || NaIO3 (0.70 M), HCl (0.010 M), I2 (0.25 M) | Pt…

A: At Cathode: Reduction- Half reaction IO3− + 6H+ + 5e− ------> ½I2(s) + 3H2O(l) Eo = +1.195…

Q: The cell potential of the cell is 0.60V measured at 30degC. The half-reaction of the cell is Cr|Cr⁺³…

A: Since you have asked a question with multiple sub-parts, as per our company guidelines we are…

Q: If the potential for the following electrochemical cell is determined to be -0.525V SCE || Ag(CN)2…

A: Formation constant Kf = 5.25 × 1017Explanation:

Q: 3. Calculate the standard potentials for each of the cells at 298 K. Is each combination spontaneous…

A: The standard electrode potential is equal to the difference between the standard electrode potential…

Q: For the following electrochemical cell: Mn(s)|Mn2+(aq)(.215M)||Cr3+(aq)(.113M),…

A: Provided concentration of Mn2+=0.215M Provided concentration of Cr3+=0.113M Provided concentration…

Question

Determine the potential of a platinum electrode (vs. SHE) when placed in a mixture of 0.00385 M TIC1, and 0.0431 M TICI
at 25 °C.
T1³+ (aq) + 2 e Tl* (aq)
Ept
Ept
1.2803
Incorrect
||
Determine the potential of a platinum electrode when placed in a mixture of 0.0173 M potassium permanganate (KMnO4) and
0.0876 M manganese chloride (MnCl₂) at pH 3.72 and 25 °C.
E° = 1.25 V
2+
MnO4 (aq) + 5e + 8 H¹ (aq) = Mn²+ (aq) + 4H₂O(1)
Incorrect
V
E° = 1.51 V
V

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: Write the Nernst equations

VIEW

Step 2: Find the potential under the given conditions

VIEW

Step 3: Find the potential under the given conditions

VIEW

Solution

VIEW

Step by step

Solved in 4 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

Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which I(aq) is in contact with I2(s) and an electrode in which a chromium strip dips into a solution of Cr3(aq)?
The cell potential of the following cell at 25C is 0.480 V. ZnZn2+(1M)H+(testsolution)H2(1atm)Pt What is the pH of the test solution?
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
From the standard potentials Tl++eTl(s)E0=0.336V TlCl(s)+eTl(s)+ClE0=0.557V calculate the solubility product constant for TlCl.
What is the cell potential of the following cell at 25C? Ni(s)Ni2+(1.0M)Sn2(1.5104M)Sn(s)
Galvanic cells harness spontaneous oxidationreduction reactions to produce work by producing a current. They do so by controlling the flow of electrons from the species oxidized to the species reduced. How is a galvanic cell designed? What is in the cathode compartment? The anode compartment? What purpose do electrodes serve? Which way do electrons always flow in the wire connecting the two electrodes in a galvanic cell? Why is it necessary to use a salt bridge or a porous disk in a galvanic cell? Which way do cations flow in the salt bridge? Which way do the anions flow? What is a cell potential and what is a volt?
From the standard potentials Ag2SeO4(s)+2e2Ag(s)+SeO42-E0=0.355V Ag++2eAg(s)E0=0.799V calculate the solubility product constant for Ag2SeO4.
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)
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
The table below lists the cell potentials for the 10 possible galvanic cells assembled from the metals A. B. C. D. and E. and their respective 1.00 M 2+ ions in solution. Using the data in the table, establish a standard reduction potential table similar to Table 17-1 in the text. Assign a reduction potential of 0.00 V to the half-reaction that falls in the middle of the series. You should get two different tables. Explain why, and discuss what you could do to determine which table is correct. A(s)in A2+(aq) B(s)in B2+(aq) C(s)in V2+(aq) D(s)in D2+(aq) E(s)in E2+(aq) 0.28V 0.81V 0.13V 1.00V D(s)in D2+(aq) 0.72V 0.19V 1.13V C(s)in V2+(aq) 0.41V 0.94V B(s)in B2+(aq) 0.53V

SEE MORE QUESTIONS

Recommended textbooks for you

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN: