How many grams of silver metal are produced from Ag*(aq) in 2.90 h with a current of 3.50 A? (F = 96,500 C/mol)

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

A: Electrolysis is defined as a process of decomposition of an electrolyte by passing current through…

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 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: An electrolytic cell contans 50.0 mL of a 0.152 M solution of FeCl3. A current of 0.775 A is passed…

A:

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 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: 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: 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: How many grams of magnesium metal will be deposited from a solution that contains Mg2+ ions if a…

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: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

A:

Q: How many seconds are required to deposit 0.268 grams of iron metal from a solution that contains…

A: Given  Mass deposited (m) = 0.268 g Current (i) = 1.22 A Time (t) = ? S The equation is Fe2+ + 2e-…

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

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

A:

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: How long must a current of 5 amperes (A) be maintained to electroplate 60 g of calcium from the…

A:

Q: In the commercial production of sodium metal by electrolysis, the cell operates at 7.0 V and a…

A: The faraday's first law explains that the quantity of any species deposited is directly proportional…

Q: A current of 5.99×104 A is passed through an electrolysis cell containing molten CaCl2 for 20.1…

A: Answers given as follows

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

A: Dimensions of the thin sheet is: 1.5 in x 8.5 in x 0.0012 inThickness of gold plating = 0.0020 in…

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

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

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: How many grams of mercury metal will be deposited from a solution that contains Hg* ions if a…

A:

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 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: What mass of Iron, Fe, will be produced in a cell using Fe(NO3)3 if a current of 5.0A is maintained…

A: Given, Current flow = 5 A, Time = 2 hours = (2 * 3600)…

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: Electrolysis of a solution of Zn(NO3)2(aq) to give zinc metal is carried out using a currentof 2.12…

A:

Q: 2) How long, in minutes, will it take to plate out 25.0g of Au from a AuCl3 solution if the current…

A:

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: What mass (in grams) of nickel could be electroplated from a solution of nickel(II) chloride by a…

A: From Faraday's first law of electrolysis, the weight of a chemical substance(w) deposited at an…

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: A current of 3.27 A is passed through a Pb(NO3)2 solution. How long, in hours, would this current…

A:

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

A: As per the given information  current =2.50 A Time = 5.30 hours or  The calculation of amount of…

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

A:

Q: Determine the current (in A) to produce 3.00 g Ag when Ag⁺(aq) is electrolyzed for 2.00 h. (F =…

A: The half reaction when Ag+ (aq) is electrolyzed.                                           Ag+ (aq)…

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 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: How many seconds

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: Current = 2.50 A = 2.50 Coulomb's /sec Time = 2.00 hr = 2×60×60 = 7200 sec F = 96500 C/mol

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: 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: 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.