What is the current efficiency of a nickel-plating bath if the cathode of a copper coulometer inseries with the experimental cell was found to have gained 1.025 g and the weight of nickeldeposited was 0.905 g?

Weight of nickel deposited = 0.905 g Weight of copper deposited = 1.025 g

What is the current efficiency of a nickel-plating bath if the cathode of a copper coulometer i series with the experimental cell was found to have gained 1.025 g and the weight of nickel deposited was 0.905 g?

What is the current efficiency of a nickel-plating bath if the cathode of a copper coulometer i series with the experimental cell was found to have gained 1.025 g and the weight of nickel deposited was 0.905 g?

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 89QAP: An electrolysis experiment is performed to determine the value of the Faraday constant (number of...

See similar textbooks

Related questions

Q: A current of 10.0 amperes flows for 2.00 hours through an electrolytic cell containing a molten salt…

A: According to the reaction given, we have Xn+ (aq) + ne-→X (s) t=2 hours=7200 sec (since 1 hr =3600…

Q: Purification of chromium can be achieved by electrorefining chromium from an impure chromium anode…

A: According to faradays first law of electrolysis, charge required to deposit cr metal is given by: Q…

Q: Determine the mass of nickel that shall be electroplated from a solution of nickel (II) chloride by…

A: Given Current (i) = 0.25 amperes Time (t) = 10 hours = (10×60×60) seconds t = 36000 seconds Mass…

Q: hours will it take to plate

Q: one process used for electroplating silver, a current of 10.23 A was passed through an electrolytic…

A: Electroplating is a process in which a thin layer of one metal is deposited on another metal surface…

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

Q: (b) In Hittorf experiment an aqueous solution of XCI at 25 °C containing 1.462 g in 100 g solution…

A: During performing the Hittorf experiment for calculating the transference number of X+ ions, an…

Q: If 12.3 g of Cu is deposited at the cathode of an electrolytic cell after 5.50 h, what was the…

Q: impure

A: According to this law, mass diposite on cathode is direactly proportion to the current. So,…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.0 M NISO4 solution…

A: A question based on electrochemical cell that is to be accomplished.

Q: An antique automobile bumper is to be chrome plated. The bumper, which is dipped into an acidic…

A: The mass accumulation of metal during electrolysis wholly depends on the flow of current and…

Q: A current of 2.90 A was applied to an electrolytic cell containing molten CdCl2 for 54 minutes.…

A: We have to calculate the mass of cadmium metal deposited when current passed is 2.90 A for 54…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.5 M NISO4 solution…

Q: A current of 4.52 A is passed through a Ni(NO3)2 solution. How long, in hours, would this current…

A: In a multiple question, we can solve only one question according to the Bartleby guidelines. Use the…

Q: It is desired to deposit 0.87 g of iron (MW = 55.85) from a FeCl3 solution by the passage of 2.5 A…

A: Given mass of of iron = 0.87 g MW for iron = 55.85 Current = 2.5 A Efficiency 85%

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.8 M NISO4 solution…

Q: Copper and palladium electrodes were immersed in solution containing copper (II) and palladium (II)…

A: In the Galvanic cell containing copper (II) and palladium (III) ions, the working electrode or the…

Q: 05 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

A: Dear student I have given answer to your question in the image format.

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.…

A: An electrolytic cell uses electric energy to perform a redox reaction not spontaneous. A kind of…

Q: The dilute sulfuric acid solution is electrolyzed with platinum electrodes with a current of 1.25 A…

A: Volume of gases evolved can be calculated from the moles of gases evolved..

Q: A current of 0.4 Amps flows for 2 hours through an electrolytic cell containing copper sulphate…

A: This problem can be solved by using Faraday's first law of electrolysis accordingto which weight of…

Q: The emf of a standard X-Y galvanic cell is -2.763V. If the standard half-cell emf for the oxidation…

A: The overall cell reaction is the sum of the two half-reactions, but the cell potential is the…

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.3 M NISO4 solution…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

Q: . Electrodepositing all the Cu and Cd from a solution of CuSo, and Cdso, required 1.20 F of…

A: The two half-reactions are as follows: Cu2+ + 2e- → Cu Cd2+ + 2e- → Cd Let us assume that x is mol…

Q: A 0.1 M aqueous CaCl, solution is electrolyzed by usina inert electrodes. If 1.25 ampere current is…

A: At cathode this reaction is taking place,Ca2+ + 2e- → Ca Calculate the charge first,Q = it and…

Q: The same cell was used to study 0.100 M NH4CI (ag), and the measured resistance was 28.50 ohms.…

A: The molar conductivity of any solution is given as - Molar conductivity = (K x 1000)/M where, M =…

Q: In an electrolysis of copper sulphate between copper electrodes the total mass of copper deposited…

A: The solution is given below -

Q: A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution…

Q: What mass of Molybdenum (Mo) could be deposited by electrolysis of an aqueous solution of Mo2(SO4)3…

A: Molar mass of Mo=95.95g/mol Provided current (i)=12.0A Provided time=125minutes Or,…

Q: 7) How long would it take to electrodeposit all the Cu2+ in 0.250 L of 0.210 M CuSO4 solution with…

A: The number of moles of Cu+ ions is calculated as,

Q: When an aqueous solution of CuSO, is electrolyzed copper metal is deposited. If a constant current…

Q: 17) The number of Faraday of charge needed to deposit 3.54 x 10-4 moles of Cr+3 ion from its…

A: In this question, we want to determine the number of Faraday of charge. Given : moles of Cr3+ ion…

Q: An unstirred solution of 2.00 M NaCl was electrolyzed for a period of 28.9 min and then titrated…

A: Concentration of NaCl = 2M Time duration of electrolysis = 28.9min Concentration of HCl = 0.314M…

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

A: GIVEN: Mass of nickel=12.5KgCurrent passed through the cell=32.5 A. To Solve: calculate time in…

Concept explainers

Potentiometric Titrations

Potentiometric titration is one of the important titration methods and is mainly carried out to characterize acid solutions. It follows a method similar to that of the normal titration technique, but the main difference is that there is no indicator used in the potentiometric titrations. Instead of using an indicator, electrodes are employed for monitoring the whole titration process. A scientist named Robert Behrend did the potentiometric titration for the first time, and it was done using the mercurous solution and potassium chloride.

Question

What is the current efficiency of a nickel-plating bath if the cathode of a copper coulometer in
series with the experimental cell was found to have gained 1.025 g and the weight of nickel
deposited was 0.905 g?

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: Given :

VIEW

Step 2: Calculations :

VIEW

Step 3: Calculation

VIEW

Solution

VIEW

Step by step

Solved in 4 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

An aqueous solution of an unknown salt of vanadium is electrolyzed by a current of 2.50 amps for 1.90 hours. The electroplating is carried out with an efficiency of 95.0%, resulting in a deposit of 2.850 g of vanadium. a How many faradays are required to deposit the vanadium? b What is the charge on the vanadium ions (based on your calculations)?
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)?
An active (metal) electrode was found to lose mass as the oxidation-reduction reaction was allowed to proceed. Was the electrode part of the anode or cathode? Explain.
Calculate the voltages of the following cells at 25°C and under the following conditions: (a) Cu|Cu+(0.80M)Hg22+(0.10M)|Hg|Pt (b) Cr|Cr3+(0.615M)Ni2+(0.228M)|Ni
In the electrolysis of a solution containing Ag+(aq), metallic Ag(s) deposits on the cathode. Using a current of 1.12 A for 2.40 hours, what mass of silver forms?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)
Using values from the table of standard reduction potentials, calculate the cell potentials of the following cells. (a) Fe(s)|Fe2+(aq)Hg2+(aq)|Hg(l) (b) Pt(s)|Fe2+(aq),Fe3+(aq)MnO4(aq),H+(aq),Mn2+(aq)|Pt(s) (c) Pt(s)|Cl2(g)|Cl-(aq)Au+(aq)|Au(s)
13.106 Hydrazine, N2H4 , has been proposed as the fuel in a fuel cell in which oxygen is the oxidizing agent. The reactions are N2H4(aq)+4OH-(aq)N2(g)+4H2O(l)+4eO2(g)+2H2O(l)+4e4OH-(aq) (a) Which reaction occurs at the anode and which at the cathode? (b) What is the net cell reaction? (C) If the cell is to produce 0.50 A of current for 50.0 h, what mass in grams of hydrazine must be present? (d) What mass in grams of O2 must be available to react with the mass of N2H4 determined in part (c)?
Determine the overall reaction and its standard cell potential at 25 C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half—cell consisting of an aluminum electrode in 1 M aluminum nitrate solution. 15 the reaction spontaneous at standard conditions?
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.
Consider the reduction of nitrate ion in acidic solution to nitrogen oxide (Ered=0.964V) by sulfur dioxide that is oxidized to sulfate ion (Ered=0.155V) . Calculate the voltage of a cell involving this reaction in which all the gases have pressures of 1.00 atm, all the ionic species (except H+) are at 0.100 M, and the pH is 4.30.
Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the Chapter on electrochemistry for relevant examples.