What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a current of 0.25 amperes flowing for 21.9 hours?

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: How many seconds are required to deposit 0.189 grams of manganese metal from a solution that…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

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

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

Q: How many grams of nickel remains in a 100 ml of 1.50 M NİCI4 solution if 3.0 ampere current is…

A: V = 100 ml = 0.1 L M = 1.50 M I = 3 Amp t = 1 hr = 60 x 60 = 3600 sec W = ? nf = 4 By using Faraday…

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: 1. What mass of the following substances can be produced in 1.0 h with a current of 15 A? a. Co from…

A:

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr converting some of the H+ to…

A: Equivalents of H+ ions reduced = QF=I×t96500=11.3 ×73 ×6096500= 0.513 Total equivalents of H+ ions…

Q: The passage of a current of 0.750 A for 25.0min deposited 0.369 g of copper from a CuSO4 solution.…

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: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Given: Amount of current = 1.03 A Time duration = 28.4 minutes.

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

A:

Q: Determine the current (in A) to produce 6.50 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: Given information  Mass of Ag = 6.50 g Time = 2.00 h To calculate: Current

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: Determine the current (in A) to produce 3.10 g Ag when Ag"(aq) is electrolyzed for 2.00 h. (F =…

A:

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 many minutes will it take to electroplate 42.1 g of gold by running 5.00 A of current through a…

A: In an electrolytic cell for the electrolysis of a metal conversion of electrical energy in to…

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

A:

Q: A solution containing a 3+ metal ion is electrolyzed by a current of 5.0 A for 10 minutes. What is…

A:

Q: Determine the current (in A) to produce 6.50 g Ag when Ag*(aq) is electrolyzed for 2.00 h. (F =…

A: The faraday's second law states that "when same amount of current is passed through different…

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

A:

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 seconds are required to deposit 0.239 grams of zinc metal from a solution that contains…

A:

Q: How many seconds are required to deposit 0.168 grams of lead metal from a solution that contains…

A: We have deposit of pb as 0.168g . Current passed is 0.974 A We have to calculate the time required…

Q: A current of 11.3 A is applied to 1.25 L of a solution of 0.552 M HBr, converting some of the H* to…

A: Given: Current (I) = 11.3 A     Volume of solution (L) = 1.25 L    Concentration of HBr = 0.552 M…

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: How many grams of tin metal will be deposited from a solution that contains Sn2+ ions if a current…

A: The metal deposited or liberated is given by the Faraday's first law of electrochemistry which is…

Q: How many milligrams of hydrogen can be produced by the electrolysis of water with a current of 0.308…

A: The electrolysis of water reaction producing hydrogen is  2 H+ + 2 e- -----> H2  Hence we can see…

Q: How many grams of nickel metal will be deposited from a solution that contains Ni2+ ions if a…

A: 1)  According to Faraday second Law :-     When 1 F or  96485 e change passes it deposite…

Q: The Nickel-Cadmium battery cell has a standard potential of 1.2 V. What is the standard free energy…

A: The relation between Gibbs free energy change and emf of cell is given by,  ∆G = -n F Ecell Ecell is…

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: How long must a current of 5.00 A be applied to a solution of Ag + to produce 10.5 g silver metal?

A: The electrolysis reaction taking place to produce Ag (s) from Ag+ (aq) solution will be  Ag+ (aq) +…

Q: How many seconds are required to deposit 0.223 grams of lead metal from a solution that contains…

A: Given that, 0.223 grams of lead metal (Pb) is deposited from a solution that contains Pb2+ ions and…

Q: How many minutes would it take to plate 12g of silver from an aqueous Ag(l) solution using a current…

A:

Q: How long would it take to deposit 2.72 g of copper from an aqueous solution of copper II sulfate by…

A: Given that : Mass of copper to be deposited (w) = 2.72 g Current (i) = 2 amps

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

A:

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

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

A: Current passed = 21.4 A Mass of chromium to be deposited = 1.72 x 102 g Time required is to be…

Q: How many seconds

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Q: how many minutes are required to plate 10.0g of nickel metal from a solution of NiSO4, if the…

A:

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M…

A: ·  change(Q)=current(i)×time(t)· 1F change passed to cu2+ solution to deposite…

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

A: Kindly get the answer given below.

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: we know the expression for the faraday's law of electrolysis is => m/E = It / F Where,  m is the…

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

A: In the electrolysis process, the cations move towards the cathode and the anions move towards the…

Q: The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO, solution.…

A:

Q: How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of CrCl3 using a…

A: Faraday's law of electrolysis draws a relationship between the amount of substance deposited by an…

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.