Part A What mass of Ni+ is produced in solution by passing a current of 67.0 A for a period of 14.0 h, assuming the cell is 89.0 % efficient?

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Ans is 0.546g

Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current of 7.5 * 104 A flowing…

A: the problem is related to Faraday`s 1st Law of Electrolysis, states that " mass of the substance…

Q: How many minutes would be required to deposit 0.375g of calcium using a current of 3.93A?

A: Given,  Mass of Ca = w = 0.375 g  Current = I = 3.93 A  Time required = t = ?

Q: How many grams of chromium metal can be deposited using an electrolytic cell with an electrolyte…

A: Given : Current = 8.30 A  Time = 6 min = 6 X 60 s = 360 s  And the salt given is CrCl3.

Q: An aqueous solution of copper sulphate, CuS04 was electrolysed between platinum electrodes using a…

A: a) The solution is containing CuSO4 solution with Cu2+ ions. Since a cathode, the reduction reaction…

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2+ ions if a current…

A: The Faraday's 1st law of electrolysis is one of the most important law which explains the…

Q: How many grams of copper metal can be deposited from Cu²*(aq) when a current of 2.50 A is run for…

A: The amount of substance deposited is directly proportional to the applied charge. Then the total…

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: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

A: current =2.50 A Time = 1.90 hours  The calculation of the amount of charge is as follows: Charge =…

Q: How long would it take to electroplate all the Zn^ 2+ in 0.280 L of .210 M ZnSO 4 solution with a…

A: The question is based on the concept of electrochemistry. It involves  application of first law of…

Q: 1) Molten metal chloride (MC13) subjected to a current of 6.50 A for 0.388 hours deposits 1.41g of…

A: It is given that current = and time for which it flows Charge,

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

A:

Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

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: What mass of copper , in mg , can be deposited from copper (II) sulfate solution using a current of…

A:

Q: 7. Determining volume of a gas by electrolysis. What volume of chlorine gas at standard temperature…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 25 minutes to a 0.50-M…

A:

Q: Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below:…

A:

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: 9. A concentrated Pb(NO3)2 (aq) solution is electrolyzed using a current of 10.5 A. a) What mass of…

A: SOLUTION: Step 1: Hello. Since the question contain multiple sub-parts, the first three subparts are…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

A:

Q: How long will it take to plate out 1.0 g Ni from aqueous Ni2+ with a current of 105.9 A? HOW DO WE…

A: Given: Mass of Ni to be plated out = 1.0 g. Current pass = 105.9 A.

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: Calculate the mass in grams of a metal Q ( Molar mass= 88.23 g/mol) that will be deposited from a…

A:

Q: What mass of Cu(s) is electroplated by running 12.5 A of current through a Cu 2+ (aq) solution for…

A: We have to calculate the mass of Cu(s) is electroplated : First, we will write down all the given…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Mass of cobalt is calculated as:-

Q: How many grams of copper metal can be deposited from Cu2"(aq) when a current of 2.50 A is run for…

A: Given:: Mass of Cu = ? molar mass of Cu = 63.546 g mol-1 Current = 2.50 A Time (t) = 2.45 h = 2.45 ×…

Q: Calculate the mass of Li formed by electrolysis of molten LiCl by a current 6525 A flowing for a…

A: Given, Current = 6525 A or 6525 C/sTime = 50h = 50×3600 s = 180000seconds

Q: What mass of Cu may be deposited from a Cu2+ solution during electrolysis by a current of 3.00 A for…

A: From the reaction it is clear that 1 mole Cu2+ requires 2 e-s fo the reduction of Cu2+ ions.…

Q: How many hours are required to produce 5.00 g of chromium metal from an acidic solution of potassium…

A:

Q: A current of 5.90 A is passed through a Sn(NO3)2 solution. How long, in hours, would this current…

A: The solution is having salt Sn(NO3)2 which contains ion Sn2+  Hence on passing the current, below…

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: What mass of Ni2+Ni2+ is produced in solution by passing a current of 67.0 AA for a period of 14.0…

A: Electrochemical cell

Q: How many grams of copper metal can be deposited from Cu2*(aq) when a current of 2.50 A is run for…

A: It is given that a current of 2.5 A is passed and for a time of 2.6 hours, in a solution containing…

Q: How many grams of mercury metal will be deposited from a solution that contains Hg²+ ions if a…

A:

Q: How much silver was there in the solution if all the silver was removed as Ag metal by electrolysis…

A: Given, Time (t) = 0.60 hr = 2160 s Current (I) = 1.00 mA = 1.00 × 10-3 A Amount (in grams) of silver…

Q: Calculate the mass (in grams) of K formed by a current of 6.5 x 104 A flowing for 24 hours if the…

A:

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni= 4.9 g molar mass of Ni=58.6934 g mol-1 charge = ?

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper II)…

A:

Q: How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr3+using a…

A:

Q: A cell that consists of a standard hydrogen half-cell and a Cu/Cu2+ half-cell has Eo = 0.34 V. If…

A: A standard hydrogen electrode is used to measure standard electrode potential. It is used as a…

Q: How many grams of copper metal can be deposited from Cu²⁺(aq) when a current of 2.50 A is run for…

A:

Q: Gallium is produced by the electrolysis of a solution made by dissolving gallium oxide in…

A: We have to calculate the amount of gallium solid that can be formed.

Q: A current of 5.26 A is passed through a 2Sn(NO3)2 solution. How long, in hours, would this current…

A: In Sn(NO3)2 we have Sn in Sn2+ form  Hence to get tin that is Sn from Sn2+ the reaction will be Sn2+…

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.