Standard Reduction Potentials at 25 °C Half-reaction Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e-Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Au+ 2Au + Au³+

Standard Reduction Potentials at 25 °C Half-reaction Eº(volts) Au³+ + 2e Au+ 1.290 Aut+eAu 1.680 Au³+ + 3e-Au 1.420 In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction: 3Au+ 2Au + Au³+

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: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The given redox reaction is 4Br-(aq) + N2(g) + 4H2O(l) → 2Br2(l) + N2H4(aq) + 4OH-(aq) Calculate the…

Q: termine E°, AG" , and K for the overall reaction from the balanced half-reactions and their standard…

A: We have to find ∆G, ∆E and K for given reaction And using given reduction potential of half cell

Q: Using data from the Standard Reduction Potentials table, place the following in order of increasing…

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

A: The two half reactions of galvanic cell are given as,

Q: Consider the standard reduction potentials listed below and identify the substance that will act as…

A: For checking strongest oxidising agent we first of all check which species have highest reduction…

Q: Using the standard reduction potential, Calculate the standard emf for each of the following…

A: Given; 2Al3+(aq) + 3Ca(s) ➝ 2Al(s) + 3Ca2+(aq) Standard emf for the following reaction (E°cell) = ?…

Q: Given the following 2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq) E°cell = 0.73 V and…

A: Given reaction: 2AgCl(s) +X(s) → 2Ag(s) + 2Cl-(aq) + X2+(aq) E°cell = 0.73 V AgCl(s) → Ag(s)…

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

Q: Use the table of standard reduction potentials to select a reducing agent that converts NI2+ to Ni…

Q: Gold exists in two common positive oxidation states, +1and +3. The standard reduction potentials for…

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

Q: At 25 oC, if the potential of a Zn–H + cell is 0.55 V at 25oC when [Zn2+] = 1.0 M and PH2 = 1.0 atm,…

A: Given Temperature = 25°C = (25 + 273.15)K = 298.15 KGiven Cell Zn-HCell reaction Zn(s) + 2H+…

Q: Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations…

A: Here we are required to find the cell potential of the given two electrochemical reaction

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: A redox reaction is an electron transfer process where oxidation and reduction reactions occur…

Q: Calculate the maximum amount of work (per mole reaction) that can be obtained from the following…

A: a. Given, a galvanic cell is constructed between Au3+ and Cu2+. Au3++3e-→Au E°=1.50VCu2++e-→Cu+…

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

Q: A certain half-reaction has a standard reduction potential E=-1.33 V. An engineer proposes using…

A: Answer: For an electrical cell its cell potential will always be: E°cell=E°cathode-E°anode Given…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Detail

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni²*] = 6.00 × 10-² M and an Ag*/Ag hal cell…

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 cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given : E°Zn+2/Zn = -0.76 V E°Cu+2/Cu = 0.34 V [CuSO4] = 0.01 M [ZnSO4] = 0.02 M

Q: Based only on the half-reactions in table below, determine what spontaneous reaction will occur if…

Q: Consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Cr3+(aq)…

A: Given data of equations : Cr3+(aq) + 3e- → Cr(s) E° = -0.74 V Cd2+(aq) + 2e- → Cd(s) E° =…

Q: What is the standard electrode potential for a galvanic cell constructed in the appropriate way from…

A: The standard reduction potential of a species define its ability to gain electrons and get reduced.…

Q: The corrosion of iron is an electrochemical process that involves the standard reduction potentials…

A: given data are- Fe(s) ⟶ Fe2+(aq) + 2e-Eo = -0.44 V O2(g) + 4H+(aq) + 4e- ⟶ 2H2O(l) Eo = 1.23 V…

Q: Which is the best oxidizing agent in the following set? You may use the table of standard cell…

A: Oxidizing agent

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

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Eored MnO2 / Mn2+ = 1.23 V Eored Cl2 / Cl- = 1.36 V

Q: Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction…

Q: A certain half-reaction has a standard reduction potential E -0.37 v. An engineer proposes using…

A: At the anode, oxidation takes place and at the cathode, reduction takes place in a galvanic cell. In…

Q: The cell notation for the Galvanic cell is A(s)/A2+//B2(s)/B- The Standard Reduction…

Q: Standard Reduction Potentials (Volts) at 25 °C Cl2 (g) + 2 e- 2 Cl- (aq) 1.360 O2(g) + 4 H3O+(aq) +…

A: The process of electrolysis is a combination of oxidation and reduction. When any element releases…

Q: A silver metal electrode is immersed into an AgNO3 Solution. A potential value of 0.734 V is…

A: Electrode potential is the electromotive force for the galvanic cell developed from a standard…

Q: All of our standard reduction potentials are supposed to be at "standard acidic conditions, which…

Q: Use standard reduction potentials to find the equilibrium constant for the following reaction at 25…

A: Standard reduction potential is defined as the tendency of a chemical species to be reduced and this…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The standard free energy change is also known as Gibb's free energy change. It is denoted by symbol…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Answer:During a cell reaction, oxidation always occurs at anode and reduction always occurs at…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: The reaction given is In the above reaction we can see that Mn in MnO2 is initially in 4+…

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

A: equilibrium reaction is Sn+2(aq) + 2 Fe+3(aq) <--> Sn+4(aq) + 2 Fe+2(aq) (1)…

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: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

A: Answer: Relation between standard cell potential and standard Gibbs free energy change is shown…

Q: E°(V). -1.66 3+ + 3e¯→ Al(s) +0.07 gBr(s) + e¯→ Ag(s) + Br¯ 4+ + 2e → Sn 2+ +0.14 ° 3+ + e¯→ Fe2+…

A: Loss of electrons is oxidation. Gain of electron is reduction. Species undergo oxidation is…

Q: The standard reduction potentials of the Fe2*/Fe and Al3*/Al couples are -0.44 V and - 1.66 V,…

Q: Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free…

Q: On the diagram below sketch the regions where colour has developed and what colour each region is…

A: Sacrificial anodes protect metals from corrosion, it works by oxidizing more quickly than the metal.…

Question

**Standard Reduction Potentials at 25°C**

| Half-reaction | E° (volts) |
|--------------------------------|------------|
| Au³⁺ + 2e⁻ → Au⁺ | 1.290 |
| Au⁺ + e⁻ → Au | 1.680 |
| Au³⁺ + 3e⁻ → Au | 1.420 |

In a disproportionation reaction, the same species is oxidized and reduced. Use the data given above to analyze the disproportionation reaction:

\[ 3\text{Au}^+ \rightleftharpoons 2\text{Au} + \text{Au}^{3+} \]

Will Au⁺ disproportionate in aqueous solution? [ ]

To justify your answer, what is the standard cell voltage for the disproportionation reaction? [ ] 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: Disproportionation reaction

VIEW

Step 2: Calculating the value of Ecell

VIEW

Step 3: Disproportion of Au+

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 9 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

Given the electrochemical reaction, Mg/ Mg 2+ (aq) // Zn2+ (aq) / Zn, E = +1.61 V. If the standard reduction potential of Zn²+ = Zn is - 0.76V. What is the standard reduction potential of Mg2+ = Mg? A) 2.37 V B 0.85 V Ⓒ-0.85 V D) -2.37 V
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 = V
Use the following half-reactions to calculate the E0cell for the reaction and classify if the redox is spontaneous or nonspontaneous Au+(aq)+e-→Au(s) E0=1.69V N2O(g)+2H+(aq)+2e-→N2(g) +H2O(l) E0=1.77V Cr3+(aq)+3e-→Cr(s) E0= -0.74V Half-Reactions E0cell Spontaneity ( Spontaneous or Nonspontaneous) N2(g)+H2O(l)+2Au+(aq)→N2O(g)+2H+(aq)+2Au(s) _ _ 3N2O(g)+6H+(aq)+2Cr(s)→3N2(g)+3H2O(l)+2Cr3+(aq) _ _ 3Au+(aq)+Cr(s)→Cr3+(aq)+3Au(s) _ _
Given the following standard reduction potentials, calculate the solubility product constant (Ksp) for lead sulfate, PbSO4. PbSO4 (s) + 2 e-→→→→ Pb (s) + SO42- (aq) E° = - 0.36 v Pb+2 + 2 e-→→→→Pb (s) E° = - 0.13 v
Determine the cell potential for the following reaction: Hg2+ + 21→ Hg + 12 Given the following standard reduction potentials: Hg2+ + 2 e-→ Hg 2 + 2 e-→21- +0.854 V +0.536 V 0.318 V -0.318 V O-1.39 V O 1.39 V
Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Ch (g) + 2 e–→ 2 CI (aq) 1.360 02(g) + 4 H30*(aq) + 4 e→ 6 H20(1) 1.229 2 H20(1) + 2 e – H2(g) + 2 OH(aq) -0.828 |-0.403 Ca2* (aq) + 2 e" - → Cd (s) A 0.124 M neutral aqueous CdCl, solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: 6H,0 | 4H,0* + 4e Half-reaction at cathode: Cd2+ 2e Cd (b) What is the expected decomposition potential? 2.123 V +
Using the following standard reduction potentials: Ag+ (aq) + e- ⇌ Ag (s) E o = +0.80 V Pb2+ (aq) + 2e - ⇌ Pb (s) Eo = -0.13 V i. i. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place.II. Describe the process involved in electroplating a silver coin.
Given the standard reduction potential, E°, which of the following half-reactions contain the strongest reducing agent. A) Au3*(aq) + 3e → Au(s); E° = + 1.42 V B) Cu2*(aq) + 2e → Cu(s); E° = + 0.34 V c) Co2*(aq) + 2e- - Co(s); E° = - 0.28 V D) Cr2*(aq) + 2e· → Cr(s); E° = - 0.91 V
Given the following standard reduction potentials, E°red, which species has the greatest tendency to be oxidized? S (s) + 2 H+ + 2e− → H2S (g) E°red = +0.144 V O2 (g) + 4 H+ + 4e− → 2 H2O (l) E°red = +1.229 V Sn2+ (aq) + 2e− → Sn (s) E°red = −0.137 V HERE ARE THE OPTIONS: O2 (g) S (s) Sn (s) H2S (g)
Given the half-reactions and their respective standard reduction potentials 1. Cu³+ + 2 e- + Cu+ E; = +1.28 V Cu²+ + e E; = +0.15 V E; = = +0.52 V 2. + Cu+ 3. Cu²+ + 2 e- → Cu(s) = +0.34 V 4. Cu* + e- Cu(s) E calculate the standard reduction potential for the reduction half-reaction of Cu(III) to Cu(II). Cu³+ + e Cu2+ E° = V
Nitesh
Consider the following electrochemical cell in which X is an unknown metal: Pt | Cl-(1 M) | Cl2( 1 atm) || X3+(1 M) | X(s) If the standard cell emf is minus3.26 V, what is the standard reduction potential at 25oC for X3+ + 3e- → X(s) -3.26 V 3.26 V 1.36 V 1.90 V -1.90 V