Determine AG (in kJ/mol) for a galvanic electrochemical cell at 38.01°C composed of a platinum electrode in a mixture of 0.0325 M Au3+ and 1.902 M Au+ coupled to a platinum electrode in a mixture of 1.784 M Au and 0.578 M Au+. 3+ Au3+(aq) + 2e- = Au+(aq) E° = 1.401 V

Determine AG (in kJ/mol) for a galvanic electrochemical cell at 38.01°C composed of a platinum electrode in a mixture of 0.0325 M Au3+ and 1.902 M Au+ coupled to a platinum electrode in a mixture of 1.784 M Au and 0.578 M Au+. 3+ Au3+(aq) + 2e- = Au+(aq) E° = 1.401 V

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 103QAP: An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from...

See similar textbooks

Related questions

Q: (c) Calculate the standard cell potential, E° of the following reaction at equilibrium. Show your…

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

A: For each reaction cell potential, gibbs free energy, redox reactions and line representation of…

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

Q: Calculate the cell voltage under these conditions around your hands to three significant digits…

A: The two half cell reactionsand their standard reduction potentials are given below.MnO 4 - (aq) + 8H…

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: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

Q: Calculate the potential of the following cells: a. a galvanic cell consisting of lead electrode…

Q: A galvanic cell using Cut/Cu and Zn2+/Zn was set up at 329 K and the non-standard cell potential was…

Q: Consider the following electrochemical cell in which the volume of solution in each half-cell is 100…

A: The Nernst equation is shown below: Ecell = electrode potential at any condition E0cell = standard…

Q: In the electroplating of nickel from a solution containing Ni2+ ions what weight of nickel-metal…

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: In the electrolysis of water, how long will it take to produce 145.0L of Hz at 1.0 atm and 273…

A: we know volume occupied by hydrogen gas = (weight of hydrogen gas /mol. mass of hydrogen) *22.4 l…

Q: In a galvanic cell, the cathode consists of a Ag*(1.00 M)| Ag half-cell. The anode is a platinum…

A: Given: Concentration of benzoic acid = 0.10 M Concentration of benzoate ion = 0.050 M Measured cell…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq)…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

A: The standard electrode potential for the given cell is calculated as shown below. The standard…

Q: Consider the following reaction and its AG° at 25.00 °C. Fe2+ (aq)+Zn(s) → Fe(s) + Zn²*(aq) AG° =…

Q: Given the schematic representation Cd | Cd2+ (1 M) || Ag+ (1 M) | Ag, write the overall cell…

A: A voltaic cell is an example of electrochemical cell. It uses a chemical reaction to produce…

Q: Electrolysis of an NaCl solution with a current of 2.00 A for a period of 200 s produced 59.6 mL of…

Q: A galvanic cell consists of a lead anode immersed in a 1.00 M solution of Pb(NO3)2 and a platinum…

Q: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction:…

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Faraday's law states that the amount of chemical change that is produced by passing a current to an…

Q: Given the following unbalanced½ reactions and their respective reduction cell potentials: Ni0,(s) →…

A: Given that, the unbalanced half-cell reaction and their respective reduction potential values:…

Q: The galvanic cell Zn(s) | Zn2+(aq) | | Ni2+(aq)| Ni(s) is constructed using a completely immersed…

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

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

A: Given-> [MnO4-] = 3.06 M [H+] = 1.02 M [Mn2+] = 4.19 M [Pb2+] = 2.07M

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

A: The given reaction is

Q: Calculate the cell potential for the galvanic cell in which the reaction Cd(s)+Cu2+(aq) ⁢->…

Q: For the following galvanic cell: Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) A. Of the two half reactions…

A: Since you have posted question with multiple subparts as per guidelines we can answer only three per…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag+| = 1.0…

A: Since Ag+(aq) has a higher reduction potential, Ag+(aq) will undergo reduction to Ag(s) and act as…

Q: For the reduction of MnO,¯ to Mn²* in aqueous acid, ɛ° = 1.51 v. For the reduction of I, to 21- in…

A: Answer:- This question is answered by using the simple concept of electrochemistry which involves…

Q: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution : Nernst equation is used to calculate the potential of the cell at non-standard…

Q: The formation of Br2 from Br- was done by electrolyzing 1.0 M KBr solution between two Pt…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq) +…

A: Oxidation is lose of electrons. Reduction is gaining of electrons. Galvanic cell is an…

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

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

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

A: The given redox reaction is, 3 Cu2+(aq) + 2 Al (s) ----> 3…

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

Q: Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs…

A: In order to figure the cell potential of any reaction in an electrochemical cell, first derive…

Q: A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt…

A: Given: Standard half-cell reduction potentials:Fe2+(aq) + 2e- -----> Fe(s) E o = -0.45…

Q: The anode compartment of a galvanic cell consists of a Zn anode immersed in 0.05M ZnCl2 The cathode…

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Given, m = 9.38g I= 23.2A

Q: An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 3.00 A passing…

A: Given Current (I) = 3A Given mass = 1.572g Time = 25min = 1500s Molecular weight = 101.07g

Q: A galvanic cell is constructed with one compartment that contains a mercury electrode immersed in a…

A: Here we have to determine the standard electrode potential of mercury electrode from the following…

Q: Consider the following reaction and its AG at 25.00 °C. Fe2+(aq) + Zn(s) – Fe(s) + Zn?+(aq) AG' =…

Q: Consider a simple galvanic cell consisting of two beakers connected by a salt bridge. One beaker…

A: Interpretation - To write the half cell reaction that occurs at each electrode To check here which…

Q: The standard reduction potential (Eo) for the conversion of Cr2O72- to Cr3+ at 25 degree C in an…

A: A Redox reaction leads to oxidation and reduction processes simultaneously. Oxidation and reduction…

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

Q: 4. An electrolysis cell that deposits gold (from Au*(aq) operates for 15 minutes at a current of…

Concept explainers

Polymers

Polymers are naturally occurring or synthetically produced large molecules or compounds which are made up of series of repeating units called monomers. They are joined together by chemical bonds. The term polymer is coined from Greek roots meaning 'many parts' and are found almost everywhere from the plastics bags to the rubber of our tires to our DNA strands.

Question

Give answer all questions with explanation and answer no

Chemistry
Determine AG (in kJ/mol) for a galvanic electrochemical cell at 38.01°C composed
of a platinum electrode in a mixture of 0.0325 M Au3+ and 1.902 M Au+
to a platinum electrode in a mixture of 1.784 M Au3+ and 0.578 M Au+.
coupled
Au3+(ag) + 2e- =
Au+(aq) E° = 1.401 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

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

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-.
How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of Ni2+ with a current of 4.00 A?
An alloy made up of tin and copper is prepared by simultaneously electroplating the two metals from a solution containing Sn(NO3)2 and Cu(NO3)2.If 20.0% of the total current is used to plate tin, while 80.0% is used to plate copper, what is the percent composition of the alloy?
At what pH does Ecell = 0.00 V for the reduction of dichromate by iodide ion in acid solution, assuming standard-state concentrations of all species except H+ ion?
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.
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
Assume the following electrochemical cell simulates the galvanic cell formed by copper and zinc in seawater at pH 7.90 and 25 C. Zn | Zn(OH)2(s) | OH(aq) || Cu(OH)2(s) | Cu(s) a. Write a balanced equation for the reaction that occurs at the cathode. b. Write a balanced equation for the reaction that occurs at the anode. c. Write a balanced chemical equation for the overall reaction. d. Determine the potential (in volts) of the cell.
An electrochemical cell consists of a silver metal electrode immersed in a solution with [Ag+] = 1.00 M separated by a porous disk from a compartment with a copper metal electrode immersed in a solution of 10.00 M NH3 that also contains 2.4 103 M Cu(NH3)42+. The equilibrium between Cu2+ and NH3 is: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 and the two cell half-reactions are: Assuming Ag+ is reduced, what is the cell potential at 25C?
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.