Answered: Copper can be electroplated at the…

Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu2*(ag) + 2 e - Cu(s) How much time would it take for 325 mg of copper to be plated at a current of 5.6 A?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 18.86QE: How long would it take to electroplate a metal surface with 0.500 g nickel metal from a solution of...

See similar textbooks

Related questions

Q: Calculate the cell potential for the following reaction that takes place in an electrochemical cell…

A: Cu(s) ∣ Cu2+(aq, 0.0032 M) ∣∣ Cu2+(aq, 4.48 M) ∣ Cu(s)We need to calculate the cell potential for…

Q: A galvanic cell is constructed using the two hypothetical half-reactions E° = 1.50 V E° = -0.50 V A…

A: Ecell0 of a galvanic cell, Ecell0 = Ecathode0- Eanode0 ∆Go of a cell = -nFEcell0, where n = number…

Q: an acidic solution containing BiO+ is electrolyzed using a current of 0.500 A. what weight of Bi…

A: From Faradays First law of electrolysis, the amount of the substance deposited(W) at the given…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

Q: Help with part D

A: In a concentration cell, the current flow is due to the difference in the concentration of the two…

Q: When the Cu2+ concentration is 1.47 M, the observed cell potential at 298K for an electrochemical…

Q: The batteries used in automobiles are rechargeable and consist of Pb and PbO2 anodes and cathodes…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current…

A: Charge = current *time (in s) Charge = 1*2.54*60 = 152.4 C

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl,(aq). How long does it…

A: Given: Mass of Copper= 111mg Current = 3.8A To find: The time taken to plate the Copper.

Q: 5. Copper can accumulate on the cathode surface according to the following reaction. Cu* (aq) Cu2"…

A: According to the Faraday's first law of electrolysis , " The amount of substance deposited during…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

Q: 2 a) Write the half-reaction for a hydrogen electrode in acidic solution when it is serving as the…

Q: Calculate the time to deposit 1.27 g of copper at cathode when a current of 2A was passed through…

Q: What is the calculated value of the cell potential at 298 K for an electrochemical cell with the…

A: The standard cell potential of the cell is: Reaction E0red/V Pb+2 + 2e- → Pb -0.13…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.37 A of current for 1.00 h.…

A: Given I = 0.37 A t = 1 hr = 60*60 S Minimum mass of Cadmium = ? g

Q: 2. Consider a concentration cell which used the following half-reaction at 273 K. Co2*(aq) + 2e- →…

A: According to bartleby answering guidelines I can provide solutions of 1st three subparts of question…

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

A: In this question, we want to determine the time in second would it take for 320mg of copper metal…

Q: A constant current of 3.20 A is used to deposit zinc on a cathode. How much zinc can be deposited in…

Q: When the Pb+ concentration is 1.45 x 10 4 M, the observed cell potential at 298 K for an…

A: Welcome to bartleby ! Introduction : We have to calculate the concentration of [Cr3+]

Q: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

Q: Like any piece of apparatus, an electrolytic cell operates at less than 100% efficiency. A cell…

A: The given data contains, Time = 10 hour. Current = 5.8 A. Mass of Cu = 53.4 g.

Q: When a lead storage battery is recharged by a current of 12.0 A for 15 minutes, what mass of PbSO4…

A: The given data contains, I =12 A Time (t)=15 min x60 s=900 Seconds

Q: Consider the following electrochemical cell (battery): Mg(s) │ Mg2+(aq) ║ Cl- (aq) │ Cl2 (g) │…

Q: Consider a galvanic cell based on the following half reactions: E° (V) Al³+ + 3e → Al -1.66 Ni²+ +…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A: Mass can be calculated as:-

Q: When the Cu2+ concentration is 1.31 M, the observed cell potential at 298K for an electrochemical…

A: Given: An electrochemical cell reaction: Cu2+aq + Mgs → Cus + Mg2+aq Half cell reactions…

Q: Like any piece of apparatus, an electrolytic cell operates at less than 100% efficiency. A cell…

Q: A galvanic cell consists of a nickel cathode immersed in a NISO4 solution and a manganese anode…

Q: When the Cu2* concentration is 1.35 M, the observed cell potential at 298K for an electrochemical…

Q: How long(hours) will it take to plate 275 mg of gold with a current of 5.3 mA ? Given: Gold is…

A: Given, Mass of gold = 275mg I = 5.3mA

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Given that : Mass of copper deposited = 18.5kg = 18.5kg×1000g/kg = 18500g Current(I) = 40.5A =…

Q: (7.15a) What mass of copper is plated out in the electrolysis of CuSO4, in the same time that it…

Q: One of the half-reactions is 2 N3- → N2 + 6 e How many faradays of electricity are required to…

A: For one mole of N2, 6 mole of electron or 6 Faraday electricity is required.

Q: When the Ag* concentration is 6.04×104 M, the observed cell potential at 298K for an electrochemical…

A: Given: Concentration of Ag+ = 6.04×10-4 M T = 298 K Ecell = 2.267 V Known: Standard reduction…

Q: When the Ag+ concentration is 4.98×10-4 M, the observed cell potential at 298K for an…

Q: Consider the following reactions at 298 K: Co^ 2+ (aq)+2 e^ —>Co(s) K^ + (aq) +e^ - -->K (s) a.…

A: The half reactions given are 1) Co2+ (aq) + 2 e- -------> Co (s) Eored =…

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

Q: A galvanic cell consists of a cadmium cathode immersed in a CdSO4 solution and a zinc anode immersed…

A: A galvanic cell is an electrochemical cell, which produce electric current by the redox reaction. In…

Q: 6. Zinc (Zn) can be purified by the electrolysis of aqueous zinc sulfate. Suppose an electrolytic…

A: Given that, In the electrolytic cell : Molarity of ZnSO4 solution = 0.050 M Weight of zinc deposited…

Q: When the Cu2+ concentration is 1.00 M, the observed cell potential at 298K for an electrochemical…

Q: What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0…

Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

Q: Consider the voltaic cell with a standard potential of 0.25V: Ni | Ni2+ (1.0 M) | H+ (1.0 M) | H2…

A: Equilibrium constant is the ratio of products to the reactants. This equilibrium constant can be…

Q: Calculate the potential of a copper electrode immersed in the following solutions. (a) 0.0440 M Cu…

Q: The standard redox potentials for copper and silver electrodes are +0.34 V and +0,80 V respectively.…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Consider the following electrochemical cell (battery): Mg(s) | Mg²“(aq) | Cr (aq) | Cl2 (g) | Pt(s)…

A: SOLUTION: Step 1: Given, Mg (s) │Mg2+(aq) ││Cl- (aq)│Cl2(g) │Pt(s) (a). In an electrochemical cell,…

Q: 5. How long would it take to deposit 15.0 g copper metal at the cathode of an electrolysis cell…

A: In this question, we want to determine the time taken for deposit 15.0g of Cu metal on Cathode. You…

Q: Calculate the time to deposit 1.27 g of copper at cathode when a current of 2 A was passed through…

A: According to Faraday's first law W = z.i.t .....(1) W is the…

Q: When the Ag+ concentration is 1.01 M, the observed cell potential at 298K for an electrochemical…

A: The reaction with standard reduction potentials – 3Ag+aq + Crs →3Ags + Cr3+aqE∘Ag+/Ag = 0.80…

Question

Copper can be electroplated at the cathode of an electrolysis
cell by the half-reaction:
Cu2*(ag) + 2 e - Cu(s)
How much time would it take for 325 mg of copper to be plated
at a current of 5.6 A?

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

Similar questions

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?
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.
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?
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?
You wish to electroplate a copper surface having an area of 1200 mm2 with a 1.0-m-thick coating of silver froma solution of Ag(CN)2 ions. If you use a current of150.0 mA, calculate how much electrolysis time youshould use. The density of metallic silver is 10.5 g/cm3.
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
A current of 0.44 A is passed through a solution of ruthenium nitrate causing reduction of the metal ion to the metal. After 25.0 minutes, 0.345 g of Ru has been deposited. What is the charge on the ruthenium ion, Run+? What is the formula for ruthenium nitrate?