A current of 3.22 A is passed through a Ni(NO,), solution. How long, in hours, would this current have to be applied to plate out 5.90 g of nickel? time required: h

Q: Using a current of 4.75 A, how many minutes does it take to plate onto a sculpture 1.50 g of Cu from…

A: From given  i(current) = 4.75A m(mass) of Cu(s) = 1.5g We know  Atomic mass of Cu(s) = M = 63.55amu…

Q: How many seconds are required to deposit 0.167 grams of cadmium metal from a solution that contains…

A:

Q: An electroplating solution is made up of nickel(II) sulfate. How much time in minutes (DON'T INCLUDE…

A: Given,  Mass of Nickel (W) = 0.500 g Current (C) = 3.00 A Time (t) = ? minute

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

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: How many seconds are required to deposit 0.143 grams of tin metal from a solution that contains Sn2+…

A: Answer: Since, Sn2+ is getting reduced into Sn, therefore its valency factor will be 2 and its…

Q: Consider the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). The measured Ecell for…

A: Given that, the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M).  So, [Cu2+] = 0.1 M,…

Q: ate the cen of galvanic cell which consist of two half rea shown below

A:

Q: A current of 3.62 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: Formula used :-    W = E×c×t\F  Where E = equivalent mass of the ion              c = Current passed…

Q: a solution containing a metal ion is electrocyzed by a current of 5 A. after 10 minutes, 1.19g of…

A: According to the first law of electrolysis mass of an element liberated during electrolysis is…

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

A:

Q: A current of 3.86 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: Faraday law of electrolysis states that the amount of substance deposited at the electrode is…

Q: A current of 3.16 A is passed through a Cr(NO,), solution. How long, in hours, would this current…

A:

Q: How much time in minutes would it take to deposit 1.05 grams of X (MW = 64.75 g/mol) on a cathode in…

A:

Q: An unstirred solution of 2.00 M NaCl was electrolyzed for a period of 21.5 min and then titrated…

A:

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

A:

Q: 3.53 L of 0.362 M  solution are electrolyzed (Cu is plated out of solution as metal.) A current of…

A: NOTE: Assuming that the solution contains Cu2+ ions and the concentration data given is for the Cu2+…

Q: (a) A Cr3+(aq) solution is electrolyzed, using a current of7.60 A. What mass of Cr(s) is plated out…

A: The mass of chromium deposited after two days can be calculated as follows-

Q: A current of 3.75 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: Required time calculation for Electrolysis:

Q: How many moles of chromium would be electroplated by passing a current of 5.2 amperes through a…

A: Given, Current (I) = 5.2 A Time (t) = 45.0 min = (45.0 × 60) s = 2700 s Moles of chromium (Cr) = ?…

Q: How many seconds are required to deposit 0.270 grams of copper metal from a solution that contains…

A: Given weight of deposited copper metal from a solution(w) = 0.270 g  Current applied (I)= 0.828 A =…

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

A: I=0.785 amperes t=61.9minutes n = 2 w=ZIt = 65.3 × 0.785× 61.9 ×60 /2× 96500 w =0.986gm

Q: A current of 4.26 A is passed through a Fe(NO,), solution. How long, in hours, would this current…

A: Applying Faraday law  W= Zit

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: A current of 3.50 A is passed through a Ni(N0,), solution for 1.20 h. How much nickel is plated out…

A: Solution Electricity charge is the body's basic property that causes it to receive energy when…

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

A:

Q: A current of 3.16 A is passed through a Cr(NO,), solution for 1.20 h. How much chromium is plated…

A: From given data  Current C = 3.16 A  Time t = 1.20 hr= 4800 seconds  Formula used…

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

A:

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

A: The mass of metal deposited can be given by Faraday's first law of electrochemistry which is -  W =…

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

A: Reduction: It is a chemical reaction which is associated with an increase in the number of electrons…

Q: How many seconds are required to deposit 0.175 grams of cadmium metal from a solution that contains…

A:

Q: How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that…

A:

Q: A current of 3.58 A is passed through a Ni(NO,), solution. How long, in hours, would this current…

A:

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: A current of 4.48 A is passed through a Fe(NO,)2 solution. How long, in hours, would this current…

A: Given, Amperes of current passed =4.48 A Solution = Fe(NO3)2 Iron plated = 6.30 g

Q: A current of 3.32 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: We need to find the mass of lead deposited during the electrolysis process by the amount of current…

Q: the Relerences to access Important values Il needed lor this Salt bridge A concentration cell…

A: Since the given electrochemical cell is a concentration cell. Therefore, the E° = 0.0 V The…

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

A: According to Faraday law:-     1F or 96485 c change passes to deposite equivalent mass of any…

Q: How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn2*…

A: Mass of Sn = 0.252 g  Time = ?

Q: A current of 3.73 A is passed through a Cr(NO,), solution. How long, in hours, would this current…

A: The charge on Cr is +2. Hence 2 moles of electrons are required,

Q: How many hours will it take to plate out all the copper in 250 ml of a 0.250 M Cu+ solution using a…

A:

Q: A current of 5.65 A is passed through a Cu(NO,), solution for 1.10 h. How much copper is plated out…

A: The balanced chemical reaction is as follows:

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: How many seconds are required to deposit 0.107 grams of copper metal from a solution that contains…

A: Given data is as follows: The mass of copper metal = 0.107 grams The current applied = 0.903 A The…

Q: How many seconds are required to deposit 0.263 grams of silver metal from a solution that contains…

A:

Q: A current of 4.62 A is passed through a Sn(NO,), solution for 1.30 h. How much tin is plated out of…

A:

Q: When an aqueous solution of CuSO, is electrolyzed copper metal is deposited. If a constant current…

A:

Q: How many seconds are required to deposit 0.150 grams of tin metal from a solution that contains Sn2+…

A: Mass = 0.150 g Current (i) = 0.652 A = 0.652 C/s  Time (t) = ?

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.