Please answer the question in the attachment. 23. For the battery below, and given that Cu | Cu2+(1 M) (E° =0.24V j and H2 | H*(1 M) (E° =0.00V),identify the anode and the cathode.+H2Cu2+, 1 MH*Write your answer concisely:

Anode is the one where oxidation takes place and hydrogen is the electrode where reduction takes…

Answered: battery below, and given that identify…

Science

Chemistry

battery below, and given that identify the anode and the cathode. and H2 +H2 Cu²", 1 M H* Write your answer concisely:

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter22: An Introduction To Electroanalytical Chemistry

Section: Chapter Questions

Problem 22.17QAP

See similar textbooks

Related questions

Q: Understanding Concepts 10. For each of the following cells, write the equations for the reactions…

A: We have to calculate the standard cell potential as follows in step 2:

Q: In a concentration cell, is the more concentrated electrolyte solution in the cathode or the anode…

A: Concentration cells are the cells with E0cell zero i.e the cathode and anode of the electrochemical…

Q: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

A: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

Q: Considering the given, Ni2 ++ 2e- → Ni EO = - 0.25 V Ag ++e- + Ag E0 = +0.799 V which is the result…

A: Electrochemical cell is a type of cell which converts chemical energy to electrical energy. The…

Q: (a) Draw the schematic diagram of the Galvanic cell made from the above with appropriate sign…

A: Redox reaction is that type of reaction where oxidation and reduction take place simultaneously.…

Q: Lead storage batteries are rated by ampere hours, that is, the number of amperes they can deliver in…

A: a) we have to show 1Ah = 3600 C. Charge in coulombs = current in ampere x time in seconds. 1Ah =…

Q: current of 15.0 A is passed through a solution of CrCl2 for 45 min. (a) How many grams Cr is…

A: When current is passed through an aqueous solution of CrCl2 , it gets electrolyzed resulting in the…

Q: FORK TO BE PLATED Ag BATTERY - AGNO,(aq) Answer the following questions based on the above diagram :…

A: The above process is example of electroplating.

Q: A 1.00 g of metal sample took 31.05 minutes to be consumed in the anode to recharge a battery using…

A: According to Faraday's first law of electrolysis, the mass of a substance deposited on the electrode…

Q: A voltaic cell consists of a strip of cadmium metal in asolution of Cd(NO3)2 in one beaker, and in…

A: The value of E˚cell is calculated as shown below: Here, E cell is the standard potential of the…

Q: Is it efficient and practical to operate a battery under these conditions of concentration (10 M…

A: Cell potential of a cell can be calculated as : E∘cell = E∘red - E∘oxi Nernst equation can be use to…

Q: Write the net cell equation for the electrochemical cell. Phases are optional De ot include the…

A: The emf of cell is calculated using formula as follows:- Ecell = Eocell-0.0592nlogproductreactant…

Q: 9. A standard state galvanic cell is constructed from the following half-cells at 298 K. Zn(s)…

Q: coulombs

Q: Label the diagram according to the components and processes of an alkaline battery. Drag the…

A: In the electrochemical cell, the chemical energy is converted into electrical energy. The addition…

Q: (a) Draw a diagram, (b) show balanced half-reactions, and (c) write the standard cell notation (line…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.39 minutes for a current…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: 4. Consider a voltaic cell con sisting of a magnesium electrode in contact with 1.0 M Mg(NO3)2 anda…

A: In the voltaic cell, the redox reactions take place that is, oxidation reaction occurring at one…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

Q: Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the…

A: The standard cell potential, E°cell and the corresponding standard Gibbs free energy change, ΔG°rxn…

Q: Question 8 Caleulate the potential of the fullowing cell at 25 C: CAILAI" Co.01M)||2, l0.0085M)|2.)

A: Given, Al|Al3+(0.01M) ||Zn2+(0.0085M)|Zn Cell potential (Ecell) = ?

Q: The specifications for a lead storage battery include delivery of steady 1.5 A of current for 15 h.…

Q: 37. Sketch the galvanic cells based on the following overall reac- tions. Show the direction of…

Q: in 1886, moissan was the first to prepare f2 by electrolysis of f^- ion. he electrolyzed kf…

A: At cathode : K+ + e- →KK + HF → KF + H 2H →H2 At anode:F- → F+e-2F →F2

Q: A current of 3.16 A is passed through a Cr(NO,), solution for 1.20 h. How much chromium is plated…

A: From given data Current C = 3.16 A Time t = 1.20 hr= 4800 seconds Formula used…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.12 minutes for a current…

A: Given: Time = 1.12 minutes = 1.12×60 sec Correct = 1.22 A Mass of the metal M = 0.0896 g

Q: Shown below is an electrochemical cell with anode a and cathode c. Both tl anode and the cathode are…

A: According to the question, we have an electrochemical cell with anode a and cathode c. Both the…

Q: Based upon the standard electrode potential below, which half reaction is more likely to undergo…

A: For any reaction to be a spontaneous reaction, the value of Eo should be +ve. The reactions given…

Q: 1. What effect would increasing the amperage in your electrolysis cell by a factor of 4 have on the…

A: Amount of substance deposited on electrode is directly proportional to amount of charge supplied.…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.57 minutes for a current…

A: Using the formula for mass deposition to solve this.

Q: estion 8 Copper is electroplated from a CuSO4 solution. A constant current of 4.57 A is applied by…

A: Given:: Mass of Cu = 1.198 g molar mass of Cu = 63.546 g mol-1 Current = 4.57 A Time (t) in minute =…

Q: HTERACTIVE EXAMPLE Electroplating How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with…

A: Given : Mass of Ni = 1.0 g Current (I) = 119.9 A Molar mass of Nickel = 58.7 gm/mol

Q: If 15.0 A of current is applied, how long would it take to produce 48 g of Cr(s)? ___ hr

Q: A gas is observed at the cathode and the pH also went up when a solution of KBr is electrolyzed.…

A: Given: At the cathode, gas is being formed. And the pH of the solution increased when a solution of…

Q: Write the two half reactions, a net reaction and calculate the net E° for the spontaneous reaction…

Q: 5. a. What products form at which electrode during electrolysis of aqueous solution of the following…

Q: How many grams of nickel would be electroplated by passing a constant current of 13.84 A through a…

Q: Consider the voltaic cell: Fe(s) Cr(s) Salt bridge containing KNO,(aq) -1 M Fe+ 1M Cr a. Determine…

A: Since you have asked multiple questions, we will solve the first 3 question for you. If you want any…

Q: A battery relies on the oxidation of magnesium and the reduction of Cu+. The initial concentrations…

A: When the battery goes dead its potential is zero and 2 moles of electrons would already been…

Q: In a voltaic cell, one compartment/electrode is a Ag*(0.600 M) | Ag(s) half-cell, the other is a…

A: Answer: In the Voltaic cell through the redox reaction chemical energy gets converted into…

Q: How many millimoles of O₂ (g) is produced in the anode if water is electrolyzed for 125 seconds…

A: Given : Time (t) = 125 seconds Current (I) = 5.25 A Faraday's constant, F = 96485 units

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current…

Q: What is the direction of electron flow with respect to the an-ode and the cathode in a battery?…

A: Oxidation is the process where an element goes through a process of losing electrons and this turns…

Q: A. Electrolysis of Water Complete the following table. Show your computations Lead and Battery…

Q: 4. An aqueous solution of KBr is electrolyzed . a. Write the half-reaction that occurs at the anode.…

A: a). Half life reaction that occurs at anode = 2Br⁻ (l) ⇒Br₂ (g) + 2e⁻ b). Half life reaction that…

Q: A current of 0.0100 A is passed through a solution of rhodium sulfate, causing reduction of the…

Q: Complete the following, providing written work for each part in order to receive credit: (a) Use…

Concept explainers

Vitamins and Coenzymes

A class of organic compounds needed in the human body for normal activities is known as vitamins. They are characterized into two parts depending upon their solubility in water. They can act as coenzymes, cofactors, or prosthetic groups for enzymes.

Question

Please answer the question in the attachment.

23. For the battery below, and given that Cu | Cu2+(1 M) (E° =0.24V j and H2 | H*(1 M) (E° =0.00V),
identify the anode and the cathode.
+H2
Cu2+, 1 M
H*
Write your answer concisely:

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 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

A metallurgist wants to gold-plate an object with a surface area of 17.21 in2. The gold plating must be 0.00200 in. thick (assume uniform thickness). (a) How many grams of gold (d=10.5g/cm3) are required? (b) How many minutes will it take to plate the object from a solution of AuCN using a current of 7.00 A? Assume 100% efficiency.
Calculate the minimum difference in standard electrode potentials needed to lower the concentration of the metal M1 to 2.00 10-4 M ¡n a solution that is 1.00 10-1 M in the less-reducible metal M2 where (a) M2 is univalent and M1 is divalent. (b) M2 and M1 are both divalent, (c) M2 is trivalent and M1 is univalent, (d) M2is divalent and M1 is univalent, (e) M2 is divalent and M1 ¡s trivalent.
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-.
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 following cell was found to have a potential of —0.492 V: Ag|AgCl(sat’d)||HA(0.200 M),NaA(0.300 M)|H2(1.00 atm),Pt Calculate the dissociation constant of HA, neglecting the junction potential.
You have a concentration cell with Cu electrodes and [Cu2+] = 1.00 M (right side) and 1.0 104M (left side). a. Calculate the potential for this cell at 25C. b. The Cu2+ ion reacts with NH3 to form Cu(NH3)2+ by the following equation: Cu2+(aq)+4NH3(aq)Cu(NH3)42+(aq)K=1.01013 Calculate the new cell potential after enough NH3 is added to the left cell compartment such that at equilibrium [NH3] = 2.0 M.
In biological systems, acetate ion is converted to ethyl alcohol in a two-step process: CH3COO(aq)+3H+(aq)+2eCH3CHO(aq)+H2OE=0.581V CH3CHO(aq)+2H+(aq)+2eC2H5OH(aq)E=0.197V (E°' is the standard reduction voltage at 25°C and pH of 7.00.) (a) Calculate G°' for each step and for the overall conversion. (b) Calculate E°' for the overall conversion.
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?
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