Macmillan LearningA coulometer's sensitivity is limited by its minimum current being delivered for its minimum time. Consider a coulometer thatcan deliver 3.8 mA for 0.18 s.How many moles of electrons can this coulometer deliver in 0.18 s via a current of 3.8 mA?moles of electrons:mol e¯Consider a 0.014 M solution of a two-electron reducing agent. How many milliliters of this solution would it take to deliver thesame number of moles of electrons as calculated in the first part of the question?volume:mL

For question 1st To determine the number of moles of electrons delivered by the coulometer in 0.18…

Answered: Macmillan Learning A coulometer's…

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...

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complete solution no need explanation Determine the molar mass (amu) of Metal (M) if it took 2.61 minutes for a current of 1.72 A to plate 0.0595 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
3. What mass of lead is deposited on the cathode during the electrolysis of lead (II) sulphate solution if 3 amps flows for 17 minutes? Electrode equation: Pb²* + 2e* → Pb RAM Pb= 64 1 Faraday= 96 500 C 4. How long will it take to deposit 1.5 g of aluminium on the cathode during the electrolysis of aluminium sulphate solution using a current of 4A? Electrode equation: Al3+ (aq) 3+e→ Fe (s) RAM Al= 27 1 Faraday= 96 500 C 5. What mass of magnesium is deposited on the cathode during the electrolysis of magnesium chloride solution if 17 amps flows for 2 days and 3 minutes? Electrode equation: Mg²+ + 2e → Mg RAM Mg= 24 Quantitative Electrolysis Handout Grade 10 1 Faraday= 96 500 C 6. How long will it take to deposit 17 g of sodium on the cathode during the electrolysis of sodium nitrate solution using a current of 2A? Electrode equation: Na* (aq) +e* → Na (s) RAM Na= 23 1 Faraday= 96 500 C
I need to determine the reduction potentials of all other half-lifes using reduction potential of Zn^2+ (0.10)/Zn half-reaction. I included the data for one of the half-lives I need to find. The known reduction potential for Zn^2+/Zn is -0.79 The cathode is Cu and the anode is Fe The potential (V) for this half cell is 0.767 and it is the potential for the Ecell. The concentration of Cu(NO3)2 is 0.10M and the concentration of Fe(NO)3 is 0.10M In the Cu/Zn pairing the supposed reduction potential of Cu was 0.212. The instructions said to use this value to determine reduction potential of Fe
please solve
3. write a report on the use of zinc as a “sacrificial anode” to minimise the corrosion of iron and steel such as on ships. Use the standard electrode potentials given in question 2 above to predict the cell emf and overall equation for the reaction that would occur in standard conditions between zinc and iron. With ocean-going ships, however, what is the solution in which the two metals are immersed? Is this solution always at an exact concentration of 1 mol dm-3? And in what ways does this real-life situation differ from the standard condition of 25oC / 298K Picture of question 2 is also given
please help me on this one, thank you
Kindly show all your work for the following question:
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg2+ (0.17 M) || Mg2+ (0.85 M) | Mg(s) V
Question 6 ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.91 minutes for a current of 1.2 A to plate 0.063 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
3
4. Name EXPERIMENT 12 ELECTROCHEMISTRY: GALVANIC CELLS Electrodes Use the table of standard reduction potentials from your textbook to complete the following table. The zinc-copper Daniell cell is given as an example. Cu Cu Zn Zn Zn Cu Zn Mg Cu Mg Conc. of Each Cation 1.0 M Zn²+ 0.5 M Cu²+ 1.0 M Zn²+ 0.1 M Cu²+ Date 1.0 M Zn²+ Zn²+ + 2e-Zn (ag) Half-Reactions A. Determine the E for the Standard Zn-Cu Galvanic Cell Zn²+ (aq) 1.0 M Cu²+ Cu²+ +2e-Cu Cathode B. Determine the E* for the Cu-Zn Cell at Non-standard Concentrations 1.0 M Zn²+ Anode + 2e → Zn Instructor Cu²+2e-Cu Zn²+ + 2e → Zn (aq) Report Sheet Cathode or Anode? Anode E E (table) (calcd) -0.76 V +0.34 V -0.76V Cathode 0.34 v anode 0.76v Cathode 0.34 v Cu²+ + 2e - Cul C. Determine the E for Zn-Mg and Cu-Mg Galvanic Cells Zn(aq) +2e Zn (s) cathode -0.76 1.0 M Mg²+Mga+2e Mg(s) anode -2.38 +1.10 V 1.10 V 1.0 M Cu²+ +Ze Cu(s) Cathode 40.34 v 2+ +2e 1.0 M Mg²+ M Mg(s) anode -2.38v "You must use the Nernst equation to calculate this…
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg*(0.37 M) || Mg*(0.77 M) | Mg(s) V

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