. Electrodepositing all the Cu and Cd from a solution of CuSo, and Cdso, required 1.20 F of electricity (1 F = 1 mol e ). The mixture of Cu and Cd that was deposited had a mass of 50.36 g. What mass of CusO, was present in the original mixture?

Q: Calculate the number of grams of metal M produced in 1.055 hour by the electrolysis if the…

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Q: If 10 amp of current is passed through a solution of CaCl2 for 10 minutes in an electrolytic cell,…

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Q: If a constant current of 2.0 amperes is passed through a cell containing Cr3+ for 1.0 hour, how many…

A: Mass of Cr deposited can be calculated using Faraday's first law of electrolysis: Mass deposited=…

Q: in one process used for electroplating metal RRr, a current of 23 A was passed through an…

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Q: Suppose you are given a 1M solution of SnCl2 and another 1M solution of MgCl2. Leaving the…

A: The question is based on concept of redox chemistry. we have to determine the concentration of tin…

Q: What is the oxidizing agent and what is the reducing agent in the galvanic cell formed by Mg and Cu?

A: Given: Galvanic cell formed using Mg and Cu elements.

Q: During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.…

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Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

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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: What amount of Cu (in grams) is deposited at the cathode when a current of 6 A is maintained for 15…

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Q: A solution of silver nitrate containing 12.14 g of silver in 50 ml of soluti on was electrolysed…

A: Initial mass of Ag in silver nitrate = 12.14 g Volume of solution = 50 ml After electrolysis, mass…

Q: 2. If a solution of CuCl2 is electrolyzed, what reaction will occur at the anode when the minimum…

A: At anode, oxidation takes place. Thus, Cl- ions are discharged first due to higher oxidation…

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: In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 16.552 g. This…

A: Given : Mass of Cu before electrolysis = 16.552 g Current passed = 0.887 A Time = 26 min = 26 X 60 =…

Q: 1. A constant current of 90 mA is applied to an electrochemical cell for 22 minutes. What is the…

A: The charge transport in a unit time is known as electric current. The current is calculated by using…

Q: A cell consisting of a saturated calomel electrode and a lead ion electrode developed a potential of…

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Q: 13.77 When a lead storage battery is recharged by a current of 12.0 A for 15 minutes, what mass of…

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Q: n the electrolysis of a solution containing Ni2+(aq) , metallic Ni(s)  deposits on the cathode.…

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Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

Q: A cell is prepared by dipping a copper rod in 0.01 M CuSO4 solution and zinc rod in 0.02 M of ZnSO4…

A: Given :  E°Zn+2/Zn  = -0.76 V  E°Cu+2/Cu = 0.34 V  [CuSO4] = 0.01 M  [ZnSO4] = 0.02 M

Q: Use the Ksp value and the standard reduction potential of Fe2+1aq2 to calculate the standard…

A: Ksp of a compound determines the equilibrium between solid and its ions formed in a solution. It…

Q: A student was asked to set-up a galvanic cell in the laboratory. He used two copper electrodes, one…

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Q: Between the galvanic couple Pb and Al, which metal is the cathode?

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Q: A concentration cell similar to the one shown is composed of two Cu electrodes and solutions of…

A: The cell potential can be calculated using Nernst equation, Ecell = E° - 0.0592n log QSince, the…

Q: This process is done in an alkaline environment, and one of the solutions used for this process is…

A: Given, galvanization process is done by passing electricity through Na2Zn(OH)4. What is the balanced…

Q: A total of 1.569 F of electricity (1 F = 1 mol e¯) was required to electrodeposit all of the Zn and…

A: Answer: This question is based on Faraday's law of electrolysis. To deposit each mole of Zinc ion…

Q: A total of 1.855 F of electricity (1 F = 1 mol e") was required to electrodeposit all of the Zn and…

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Q: 5. If 2.46 g of Fe 2+ were oxidized in the reaction Fe2+(aq) + Ce4+( aq ) à Fe3+ (aq) + Ce3+ (aq ),…

A: The molar mass Fe atom is:- 55.85g/mol

Q: 4. Knowing that the standard reduction potential of the redox pair F2 F is Eo = +2.87 V, what…

A: The question is based on the concept of electrochemistry. We have been given standard reduction…

Q: Predict the products of the electrolysis of an aqueous solution of sodium chloride in cell using…

A: Electrolysis is a spontaneous redox process Here we are required to find the product when aqueous…

Q: A galvanic cell using Mg / Mg*" and Cu / Cu" half-cells operates under standard-state conditions at…

A: Cell delivers = 0.31 A or 0.31 C/sec In 1 sec charges delivered = 0.31 C  32.1 hr = 3600 sec × 32.1…

Q: Enter your answer in the provided box. Copper is purified by electrolysis. A 4.75-kg anode is used…

A: Given:  Mass of anode = 4.75 kg = 4750 gm  Current (I) = 37.8 A

Q: Electrolysis of molten NaCl is done in a Downs cell operating at 7.0 volts and 4.0 x 10^4 A. How…

A: Molten NaCl electrolysis is given by the following expressions- At anode - 2 Cl- (aq) → Cl2(g) + 2…

Q: 3) How many minutes will it take to plate out 16.22 g of Al metal from a solution of AS using a…

A: Given  Mass of Al =16.22g  Used Current =13.8amps Number of electrons =3 electrons (Al-->Al+3)…

Q: An object is electroplated with rhodium for 28.2 minutes at current of 1.4 A. Rh3+ + 3 e Rh Molar…

A: According to Faraday's law of electrolysis, the amount of solid deposited is given by m =…

Q: How long will it take in hours to create 1.026 grams of Cr at the cathode of an electrolytic cell if…

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Q: What mass of silver would plate onto the cathode if a current of 7.9 A flowed through the cell for…

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Q: What mass of gold is produced when 15.2 A of current are passed through a gold solution for 25.0 min

A: Given information: Current (I) = 15.2 A Time (t) = 25.0 min

Q: new coin having a mass of 2.5133 g is dissolved in nitric acid and only the resulting copper ions…

A: Nitric acid is a strong oxidizing agent. It can oxidize metals to their respective cations.

Q: Inert graphite electrodes were used to create Fe2+ and Al3+___ (what were the ions) solutions. A…

A: Given: Ions present in the solution = Fe+2 and Al+3 Voltage present = 9.73 V Graphite electrodes…

Q: In the electrolysis of a sodium chloride solution, what volume of Cl2 (g) is produced in the same…

A: Given data,Volume of H2=6.0LTemperature=0oC=273.15KPressure=1.0atm

Q: ow many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of…

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Q: The electrolysis of CUCI(ag) produces Cu(s) and Cl2(g). What is the minimum external emf needed to…

A: Standard reduction potential of Cu+/Cu = 0.52 V Standard reduction potential of Cl2/Cl- = 1.36 V

Q: In the electrolysis of a solution containing Ag* (aq), metallic Ag(s) deposits on the cathode. Using…

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Q: - A student wanted to plate a silver ring with a layer of gold, He passed an electric current of 10…

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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: Electrolysis of molten  NaCl is done in a Downs cell operating at 7.0 volts (V) and 4.0×104 A . How…

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