Like any piece of apparatus, an electrolytic cell operates at less than 100% efficiency. A cell depositing Cu from a Cu2+ bath operates for 10 h with an average current of 5.8 A. If 57.6 g of copper is deposited, at what efficiency is the cell operating?

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu?* (aq)…

A: Since in the above reaction, Cu2+ is being reduced to Cu and Al is being oxidised to Al3+  Hence the…

Q: Given the standard reduction potentials for an element A, at 25 °C: А2"(аg) + е > A (ag) E1° = 1.09…

A: Standard cell potential is an intensive property which does not depend on amount or mass of the…

Q: An electrolysis cell for aluminum production operates at 5.0 V and a current of 8.5 x 10° A.…

A:

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: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 17…

A: The reduction reaction is as follows: Z3+(aq) + 3e- → Z(s). The atomic mass of element Z, (M) =…

Q: Copper metal (63.546 g/mol) is purified by electrolysis. How much copper metal (in grams) could be…

A: Molar mass of copper = 63.5 gm  N-factor (valancy) = 2

Q: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu2*(ag) +…

A: Given: Mass of copper= 325 mg Current= 5.6A The given reaction is Cu2+(aq) + 2e-→Cu(s)

Q: Nickel and silver rods are placed in a solution of nickel ion and silver ion solutions of…

A: The considered cell is made of nickel and silver electrodes.

Q: An electrolysis cell that deposits copper (from Cu2+ ions) operates for 30 minutes at an electric…

A:

Q: Copper metal can be purified electrolytically according to the following arrangement. The anode is…

A: W = I × t × M / n × F Where ; W = mass of  purified Cu = ? I = current = 15 A  t = time = 8.5 hours…

Q: 3. A factory wants to produce 1.0 x 103 kg Barium from the electrolysis of molten barium chloride.…

A: The given values are: m=1.0×103 kg=1.0×106 gt=4.0 h=4.0 ×3600 s The electrolysis step to form barium…

Q: A battery can provide a current of 4.00 A at 1.60 V for 1.00 hr. How much energy (in kJ) is…

A: Given that a current of 4.00 A was provided by battery at 1.60 V. The power can be calculated as…

Q: Calculate the mass of hypothetical element Z deposited by an electrolytic cell that operates for 15…

A: Given :  Current (I) = 2.6 A  Time(t) = 15 min = 900 sec  Atomic mass of Z = 182.54 g/mol

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: An electrolytic cell consists of a pair of inert metallic electrodes in a solution buffered to pH =…

A: Part a: The electrolytic cell consists of two electrodes, anode and cathode. Oxidation occurs at…

Q: If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2 amps in an…

A: Given, If 2.19 g of chromium metal was deposited from a solution of Cr3+ using a current of 35.2…

Q: 4. Calculate the equilibrium constant, Keg, for each electrochemical cell at 298 K if E° cell=2.11 V…

A: ΔG°cell = - nFE°cell ΔG°cell = - RTlnKeq Thus, nFE°cell = RTlnKeq F = Faraday constant  n = number…

Q: An electrolysis cell for aluminum production operates at 5.0 V and a current of 3.0 × 10° A.…

A: The half cell reaction will be as follows: Al3+(aq) + 3e- -------->Al(s). The currect, (I) =…

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: A galvanic cell consist of a metallic zinc plate immersed in 0.1 M Zn(NO3)2 solution and metallic…

A:

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: Metallic magnesium can be made by the electrolysis of molten MgCl2.How many minutes are needed to…

A: According to Faraday’s first law, the chemical deposition which takes place during electrolysis is…

Q: Elemental calcium is produced by the electrolysis of molten CaCl2. (a) What mass of calcium can be…

A: Given: Current applied  = 7.5 x 103 A Time of supply   = 48 h Efficiency of cell = 68%

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: Based on the cell notation of an electrochemical cell, Pt(s) | H2 (aq, 0.02 M) || Ag' (aq,0.15 M) |…

A: The standard electrode potential is the measurement of potential at equilibrium under standard…

Q: Zinc metal is deposited onto a cathode surface by passing a current of 1.87 amps through a solution…

A:

Q: A galvanic cell is powered by the following redox reaction: 2+ 4 Cu (aq) + N,H(aq) + 4OH (aq) 4 Cu"…

A:

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

A:

Q: A galvanic cell is powered by the following redox reaction: Cl,(g) + H,(g) + 2 OH (aq) → 2 Cl (aq) +…

A: Given : We have to write half reaction taking place at anode and cathode.

Q: A battery can provide a current of 2.20 A at 1.40 V for 10.0 hr. How much energy (in kJ) is…

A: GIVEN: Current = 2.20 A Voltage = 1.40 V Time= 10.0 hr To CALCULATE: Energy (kJ)

Q: b. Assuming the two half cells operate at standard conditions, calculate the standard reduction…

A: Recall the given half-cell reactions :                        HgO s  +  H2O l  +  2 e-  →  Hg l  +…

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: 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: The electrodeposition of copper can be used to determine the copper content of a sample. The sample…

A:

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: A galvanic cell is powered by the following redox reaction: 3 Cl,(9) + 2 Cr(OH),(s) + 10 OH (aq) 6…

A: The overall reaction taking place is given as,

Q: Gold (atomic mass = 197.0) is plated from a solution of chloroauric acid, HAuCl4; it deposits on the…

A: Given: Mass of god produced = 0.34 g. Current passed = 0.10 A

Q: current of 5.79 amps passes over 500 seconds in 300ml aqueous solution of CuSO4 copper…

A: Faraday's laws of electrolysis were proposed to solve such problems. According to the first law of…

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

A:

Q: An electrolysis cell for aluminum production operates at 4.5 V and a current of 7.5 x 10° A.…

A:

Q: A galvanic cell is powered by the following redox reaction: 3+ 4 Fe (aq) + N,H,(aq) + 4 OH (aq) 2+ 4…

A: a galvanic cell is powered by the following redox reaction:    4Fe3+ + N2H4 + 4OH- >>>…

Q: Calculate ΔG∘rxn and E∘cell for a redox reaction with n = 2 that has an equilibrium constant of K =…

A: To calculate E 0 cell  and ΔG 0, we can use the following formula : ∆G ° = - 2.303 RT  log K  and…

Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: identify the reaction at the anode, reaction at the cathode, the overall reaction, and the…

A:

Q: An electrochemical cell is made of theoretical metals Ma/Ma and Mb/Mb.  If the reduction potentials…

A:

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

A:

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

A: According to Faraday's law of electrolysis ; Weight of the substance deposited on the electrode is…

Q: Copper(I) ion can act as both an oxidizing agent and a reducing agent. Hence, it can react with…

A: Answer :- 1.45 × 1012  The equilibrium constant (K) at 25°C for the given reaction = 1.45 × 1012…

Q: An electrolysis cell for Aluminum production operates at 4.5V and a current of 1.5 x 10 A. Calculate…

A: Given the current passed, I = 1.5*105 A Potential, V = 4.5 V  Mass of Al(s) needs to be produced =…

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.