How long does it take to paint a plate with an area 25 cm2 with a layer of Copper is 0.1 mm thick, using a constant current of 0.5 Amp? Note that the density of copper is equal to 8.96 g cm-3 Solution: Applying Faraday's first law: w=Q×e/a×F

How long does it take to paint a plate with an area 25 cm2 with a layer of Copper is 0.1 mm thick, using a constant current of 0.5 Amp? Note that the density of copper is equal to 8.96 g cm-3 Solution: Applying Faraday's first law: w=Q×e/a×F

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 120AE

See similar textbooks

Related questions

Q: 6b. How long does it take to deposit a coating of gold 1.00 picometers thick on a disk-shaped…

Q: Use the tabulated electrode potentials to calculate ΔG° for the reaction:I2(s) + 2…

A: Oxidation half cell: 2Br- (aq) → Br2 (l) + 2e- Eₒ oxid. = -1.09V … (1) Reduction half cell: I2(s) +…

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: A thin circular-disk earring 4.00 cm in diameter is plated with a coating of gold 0.25 mm thick from…

Q: Calculate the cell potential for a cell at 38oC with a Cu2+ concentration of 0.017 M and a Zn2+…

Q: A)Give the reason why it is necessary to use hydrogen as a standard to define the standard potential…

A: The solutions are given below -

Q: Consider the galvanic cell constructed with the following materials Zn electrode Zn(NO3)2(aq), Fe…

A: An electrochemical cell that converts the energy of spontaneous redox chemical reactions to…

Q: Use the tabulated electrode potentials to calculate K for the oxidation of zinc by H+ (at 25 ∘C):…

A: The Nernst equation at 298 K is as follows, E = Eo - 0.0592n…

Q: Two identical spoons were electroplated with Ag or Cd through the use of the electrolytic cells…

A: Amount of metal deposit on spoons depends on the amount of current passed.

Q: Which of the following expressions is correct for the maximum mass of copper, in grams, that could…

A: Given values -> Time = 16hour = 16 × 60×60 seconds =16×3600 seconds…

Q: Gold can be plated out one atom in thickness and look like solid gold. If a necklace has a surface…

A: The oxidation state of gold in the solution given is +3 i.e Au3+. Hence the solution will have Au3+…

Q: 5. (a) A galvanic cell consisting of a Cd electrode dipping into a 1.0 M CdCl2 solution and a Pt…

A: Here, we have to determine the standard cell potential of the following cell in which Cd metal…

Q: Consider the cell Pt(s)/ H2(g, 1 bar)/NaOH (aq, 0.01m), NaCl (aq, 0.01125m)/ AgCl(s) / Ag(s) 2H₂O +…

A: Recall the cell representation, Pt s / H2 g, 1 bar / NaOH aq, 0.01 m,…

Q: using carbon electrodes anode and cathode. i) Calculate the volume of gas evolved at anode (at…

A: We will calculate volume of gas at STP

Q: Using a constant current of 7.8 A, a metal object is to be gold-plated by an electrolytic procedure…

Q: Calculate the cell potential for a cell at 39oC with a Cu2+ concentration of 0.02 M and a Zn2+…

A: Nernst equation gives the cell potential of a electrochemical cell at non-standard condition.

Q: (i) Pt(s) + 2 NH3(aq) + 2 CI ( (aq) cis-[PtCl₂(NH3)2](aq) + 2 e¯ E° = 0.274 V The likely cathodic…

Q: How much time (in hr) must a constant current of 50.0 A be passed through an electrolytic cell…

A: Given : Current = 50.0 A Moles of Cu formed = 5.00 mol And the ions of Cu present in the solution is…

Q: If you started at standard conditions with a battery of Cu*/Cu° and Ag*/Ag®, calculate what the…

A: In an electrochemical cell, reduction takes place at the cathode and oxidation takes place at the…

Q: Why is it not possible to measure single electrode potential?

A: Potential difference in the electro-chemical cell is generated due to the redox reaction occurring…

Q: Consider the following galvanic cell: E° (V) Sn4+ + 2 e− → Sn2+ 0.139 Ag+ + e− →…

Q: What mass (in grams) of nickel (AW = 58.69) could be electroplated from a solution of nickel(II)…

A: Given that: Current(I) = 0.25A = 0.25C/s Time = 10 hours = 10h×3600s/h = 36000s

Q: Given that the standard electrode potentials (E°) of metals are:K+/K = -2.93 V, Ag+/Ag = 0.80…

A: standard electrode potentials (E°) is inversely proportional to reducing power Higher standard…

Q: Use the Nernst equation to calculate the cell potential, Ecell, for a galvanic cell consisting of…

A: Electrons flow from anode to cathode in a galvanic cell. In order to prevent the build-up of…

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A: The expression of Nernst equation is shown below: Ecell = E0cell -0.0591nlog Q Where; Ecell= cell…

Q: What is the standard emf of a galvanic cell made of a Pb electrode in a 1.0 M Pb(NO3)2 solution…

Q: An inventor proposes using a SHE (standard hydrogen electrode) in a new battery for smartphones that…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

Q: Calculate the cell potential for a cell at 29oC with a Cu2+ concentration of 0.017 M and a Zn2+…

A: This question is solved by nernest 's equation.

Q: How long does it take to deposit a coating of gold 1.00 μm thick on a disk-shaped medallion 4.00 cm…

Q: You would like to produce a gold-plated coin by plating gold onto a penny 1.90 cm in diameter. How…

A: Given : diameter of coin = 1.9 cm => radius of coin, r = 1.9 / 2 = 0.95 cm and thickness of gold…

Q: What the standard potential of an electrode of a cell containing the Sn²⁺/Sn and Br₂/Br⁻¹ couples?

A: The standard reduction potential of Sn2+ is -0.14 V. The standard reduction potential of Br2 is…

Q: 20. Due to COVID-19 coupled with erratic power supply from ZESCO, you decide to play around with…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: What would the potential of a standard hydrogen electrode (S.H.E.) be under the following…

A: Given, Molar concentration of H+ = [H+] = 0.12 M Pressure of H2 = PH2 = 2.2 atm Temperature = T =…

Q: Oxygen Supply in Submarines Nuclear submarines can stay under water nearly indefinitely because they…

A: The electrolysis of water produces oxygen. Since the O is in 2- oxidation state in water initially…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The discharging reaction if lead storage battery is given as:Pb (s) + PbO2 (s) + 2SO42- (aq) + 4H+→…

Q: Which of the following expressions is correct for the maximum mass of copper that could be plated…

Q: Calculate the value of the EMF of galvanic cells and write the electrode reactions occurring in…

A: a) Zn/Zn2+(0.001)∥Cd2+(0.1)/Cd Anode : Zn = Zn2+ + 2e-…

Q: Calculate the cell potential for a cell at 29oC with a Cu2+ concentration of 0.01 M and a Zn2+…

Q: A voltaic cell consists of a Cr/Cr2+ half-cell and a Sn/Sn2+ half-cell, with [Sn2+] = 0.20M and…

A: Given: [Sn2+] = 0.20 M [Cr2+] =1.60 M Known: ECr2+|Cro=-0.913 VESn2+|Sno=-0.14 V

Q: Saquon builds a galvanic cell using a zinc electrode immersed in an aqueous Zn(NO3)2 solution and a…

A: The anode , oxidation takes place. So to check which species is produced at anode , we first check…

Q: A galvanic (voltaic) cell consists of an inert platinum electrode in a solution containing 1.0 M…

A: Given : electrode 1 => 1.0 M titanium(III) ion and 1.0 M titanium(II) ion and electrode 2 =>…

Q: Consider the reaction corresponding to a voltaic cell and its standard cell potential.…

A: Reaction: Zn(s) + Cu2+(aq) -------> Cu(s) + Zn2+(aq) E°cell = 1.1032 Cell potential,Ecell = ?…

Q: Calculate the cell potential for a cell at 43oC with a Cu2+ concentration of 0.012 M and a Zn2+…

Q: How long would it take a current of 1 ampere to reduce completely 80 cm3 of 0.10 M Fe2(SO4)3 to…

A: We can solve this problem by using the faraday law of electrolysis W= (E×i×t)/96500 W= mass of a…

Q: Use the tabulated electrode potentials to calculate K for the oxidation of zinc by H+ (at 25 ∘C):…

A: The considered cell reaction is, Zn s + 2H+(aq) →Zn2+(aq) + H2 g

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: Calculate the theoretical cell potential of the following cells. If the cell is short-circuited,…

Q: A spontaneous galvanic cell consists of a Pb electrode in a 1.0 M Pb(NO3)2 solution and a Cd…

A: In galvanic cell greater the value of standard reduction potential greater is the tendency to get…

Question

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps with 4 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

It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Cu2+(aq)+Ni(s)Cu(s)+Ni2+(aq) (b) 2Ag(s)+Cl2(g)2AgCl(s) (c) Cl2(g)+2I(aq)2Cl(aq)+I2(s)
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)?
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.