Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this cable. 2 Au³ + (aq) + 3 Cr(s) ⇒ 2 Au(s) + 3 Cr²+(aq) AGⓇ = kJ/mol

Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this cable. 2 Au³ + (aq) + 3 Cr(s) ⇒ 2 Au(s) + 3 Cr²+(aq) AGⓇ = kJ/mol

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 61QAP

See similar textbooks

Related questions

Q: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

Q: Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard…

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

A: Interpretation - To calculate the standard cell potential for the given reaction by using their…

Q: Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard…

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question. A…

Q: Use the following standard reduction potentials to determine which species is the strongest…

A: Given, the standard reduction potentials: Fe2+(aq) + 2 e– → Fe(s); E° = –0.41 V Pt2+(aq) + 2 e– →…

Q: The nickel-cadmium battery cell has a standard potential of +1.20 V. The cell reaction is 2…

A: The solution is as follows :

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

A: The relationship between the potential of an electrochemical cell and ΔG° is given as- The overall…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2 +] = 0.887 M…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.831 M…

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

A: Given,

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

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr2+]=0.876 M and…

A: Cr(s)+Fe+2 (aq )<==> Cr+2 (aq)+Fe(s) [Cr+2] = 0.876 M [Fe+2] = 0.0120 M

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Cr²+] = 0.768 M…

A: Given data : Cr(s) + Fe2+ (aq) ==> Cr2+(aq) + Fe(s) From table : E(Fe2+/Fe) = -0.44 V…

Q: The electrochemical cell Cu|Cu 2+||Al 3+|Al has a potential of –1.997 V under standard conditions.…

Q: Use the following standard reduction potentials to determine which species is the strongest reducing…

A: ->The species which has highest reduction potential that will get reduce itself and oxidize…

Q: John set up a galvanic cell. The balanced redox reaction equation is Mg(s) + 2 Ag+ (aq) →Mg2+(aq) +…

A: emf of cell can be calculate by Nernst equation Ecell = Eocell - (0.0591/n ) log Q ----(1)…

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

Q: 33M. I need to calculate Gibb's free energy and equilibrium constant, K. Is the reaction…

A: In an electrochemical cell, two electrodes are used. One is an anode and the other is a cathode. The…

Q: What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal…

A: The chemical reaction : Cu(s) + 2Ag+(aq) ⇌ Cu2+(aq) + 2Ag(s) The equilibrium constant at 25°C = ?

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, . The reaction that occurs…

A: Give that: the reaction of anode is: 2Cl- (aq) →Cl2 (g) + 2e- Mass of Cl2 produced, w =182 g, time…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M…

Q: What is the equilibrium constant for the following reaction at 25 °C? Round your answer to 1 decimal…

A: Temperature = 25°C = 298 K As per standard data: E°Ag+/Ag = +0.80 V E°Cu+2/Cu = +0.34 V R = Gas…

Q: Given the cell reaction, Zn(s) + Cut2(a the cathode in the cell is: Cu(s) Cu +2 OPt (aq) Zn(s) +2…

A: The objective of the question is to calculate the standard cell potential, Eº, for the given…

Q: Use the following standard reduction potentials to determine which species is the strongest…

A: Oxidizing agent oxidizes other substance and reduced itself. Strongest oxidizing agent has the half…

Q: Calculate the standard free-energy change for the reaction at 25 °C. Refer to the list of standard…

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

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

A: The given cell reaction is 2Au3+(aq) + 3Ni(s) → 2Au(s) + 3Ni2+(aq) ... (A) Temperature = 25 °C =…

Q: The standard free energy change for a reaction can be calculated using the equation ΔG∘′=−nFΔE∘′…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Mg? +] = 0.788 M…

A: Temperature = 298.15 K [ Mg+2 ] = 0.788 M [ Fe+2 ] = 0.0200 M ECell = ?

Q: Use standard reduction potentials to calculate the standard free energy change in kJ for the…

A: Reaction: 2H+ (aq)+Hg(l) → H2(g) + Hg2+(aq)Half cell reactions:2H+(aq) + 2e−→ H2(g)…

Q: A quantity of electricity equal to 9.263 × 104 C passes through a galvanic cell that has an Ni(s)…

A: Given data Electricity passed=9.263x104 C Standard value of the Faraday constant is 96500 C/mole…

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

Calculate the standard free-energy change for this reaction at 25 °C. A list of standard reduction potentials can be found in this
able.
3
2 Au³ +(aq) + 3 Cr(s) — 2 Au(s) + 3 Cr² + (aq)
AG =
kJ/mol

Expert Solution

Step 1

Step by step

Solved in 2 steps with 2 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

1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 seconds
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?
Order the following oxidizing agents by increasing strength under standard-state conditions: Mg2+(aq), Hg2+(aq), Pb2+(aq).
A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?
An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?
For the reaction Cu2+(aq) + Zn(s) → Cu(s) + Zn2+ (aq), why can’t you generate electric current by placing a piece of copper metal and a piece of zinc metal in a solution containing CuCl2(aq) and ZnCl2(aq)?
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Given the following two standard reduction potentials, solve for the standard reduction potential of the half-reaction M3++eM2+ (Hint: You must use the extensive property G to determine the standard reduction potential.)
Consider the following cell reaction at 25C. 2Cr(s)+3Fe2+(aq)2Cr3+(aq)+3Fe(s) Calculate the standard cell potential of this cell from the standard electrode potentials, and from this obtain G for the cell reaction. Use data in Appendix C to calculate H; note that Cr(H2O)63+(aq) equals Cr3+(aq). Use these values of H and G to obtain S for the cell reaction.
Consider the following cell running under standard conditions: Fe(s)Fe2+(aq)Al3+(aq)Al(s) a Is this a voltaic cell? b Which species is being reduced during the chemical reaction? c Which species is the oxidizing agent? d What happens to the concentration of Fe3+(aq) as the reaction proceeds? e How does the mass of Al(s) change as the reaction proceeds?
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
Consider the following galvanic cell: Calculate the concentrations of Ag+(aq) and Ni2+(aq) once the cell is dead.