During the electrolysis of a solution of Zn(NO3)2, 1.572 g of metal plated out at the cathode. How many  Coulombs (C) of charge does this represent?

Q: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A: Electric current : It is defined as the rate at which a particular charge flows. It is represented…

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: During a period of discharge of a lead-acid battery, A g of Pb from the anode is converted into…

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

A: Faraday's Law: It can be defined as by saying that the amount of substance produced at each…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by…

Q: What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution…

A: Faradays first electrolysis Law states that the quantity of reaction taking place in terms of mass…

Q: 4. A metallurgist wants to gold-plate a thin sheet with the following dimensions: 1.5 in x 8.5 in x…

A: Given current = 7 A standard value  density of gold = 19.3 g/cm3

Q: It took 116 hours to produce 603 g of metal X by performing electrolysis on molten XC13 with a…

A: From Faraday’s first law of electrolysis the quantity of charge is calculated as: Where, Q is…

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: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given that: Mass of chromium deposited = 14.5 g Amount of current passed through solution = 4.57 A…

Q: How many grams of Au would be deposited from an aqueous solution of Au 3+ with a current of 2.213 A…

A: Given, Molecular mass of Au = 196.96 u Current = 2.213 A time = 480 minutes = 28,800 sec

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: An electrolysis cell contains a solution of 0.10 M NiSO4. The anode and cathode are both strips of…

A: Electrolysis is spitting of chemical decomposition of ionic substances due to passage of electric…

Q: What are the products obtained in the electrolysis of a molten mixture of KIKI and KBr

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Q: 6. A 1M aqueous solution of chromium (I) bromide will be electrolyzed to "chrome plate" a faucet.…

A: As per the Faraday's 1st law of electrolysis: w=ZIt      ----(1)where,w = weight of the substance…

Q: A voltaic cell is constructed at 25 °C from a half-cell in which a nickel rod is dipped into a…

A: The voltaic cells are electrochemical cells which has an anode and cathode separated and is…

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

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Q: If a galvanic cell is constructed using Au3+ and Al3+, which ion will most likely be in the anode?

A: Reduction Addition of electron is called reduction Oxidation Removal of electron is called oxidation

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

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Q: What volumes of H3(g) and O,(g) at STP are produced from the electrolysis of water by a current of…

A:

Q: Aluminum metal can be made from aluminum(III) ions by electrolysis. What is the half-reaction at the…

A:

Q: If a current is flowing from a battery that's used to electroplate an object with silver, how do I…

A: Given:1.45 A.hr = 1.45 amp current per hour.

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

A:

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of (NH4)2SO4 in…

A: Electrolysis is the process in which electric energy is converted into chemical energy. During…

Q: At a steady current of 5 A and a time of 20 minutes, which of the metal will deposit more metal at…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr2+ (aq) is…

A:

Q: How many grams of metal Ca (40.08g/mol) are produced by electrolysis of CaBr2 using a current of 28…

A: Kindly get the answer given below.

Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

A: Current = Charge/Time  Q = I/t  1F =96500 C/mol  Mass of 1 mole =Molar mass

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: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

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: 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: 7. A current of 1000. A flows for exactly 1 hour, through a cell in which the following reaction…

A:

Q: 7. How many grams of aluminum metal (26.982 g/mol) can be produced by the electrolysis of Al2O3…

A: In Al2O3, the oxidation number of Al is +3 and that of O is -2.  Hence uring electrolysis of Al2O3,…

Q: The electrolysis of an aqueous solution of potassium iodide, KI, results in the formation of…

A: Electrolysis: It is a chemical reaction that occurs when an electric current is conducted through a…

Q: (a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Interpretation -  In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are…

Q: How many seconds

A:

Q: Chrome is plated from solutions of chromium (III) chloride. If a current of 4.57 A is passed through…

A: Given data:  Current = 4.57 A  Cr deposited = 14.5 g  Molar mass of Cr = 52 g.mol-  CrCl3  ==>…

Q: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A  (given) Molar mass of copper = 63.55 g/mol   (given) Cu is having n factor of 2…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: Faraday's first law of electrolysis It states that the mass of a substance deposited on any…

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

A: Given,  Current in ampere = I =  0.150 A  Electrolysis of Ni2+ (aq) ion  Time period in minutes = t…

Q: According to the calculation, the electrolysis formed 0.107 mol M. During this time, 7.00 g M are…

A: Given: No. of mole of  (M ) = 0.107 mole Mass of ( M ) = 7 g   Find Molar mass of ( M )= ???

Q: write the half-reactions that occur at the anode and cathode during the electrolysis of NH4Cl in…

A: Answer  Electrolysis of NH44Cl

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: Suppose the galvanic cell sketched below is powered by the following reaction: Cu(s)+2 A£NO3(aq) →…

A: Given thatthe cell reaction that takes place in the Galvanic cell is given by Cu(s)   + 2AgNO3(aq) →…

Q: a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc…

A:

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…