ow many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of 3.8 A?   X4+ + 4e- → X(s)

Q: How much time in minutes would it take to deposit 1.74 grams of X (MW = 133.98 g/mol) on a cathode…

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

A: The chemical reaction corresponding to electroplating of Chromium is given as:Cr2O72- (aq) + 14 H+…

Q: 3. A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

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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: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A:

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

A: (a) Current is the amount of charge flowing per unit time. If I is the current(in A) andt is the…

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

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

A: first we have to find the volume,volume=length ×width×heightthen we know,density=massvolumeby…

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A:

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited,  W = ZCt Where,   t = time in second…

Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

A:

Q: A metal object is to be gold-plated by an electrolytic procedure using an aqueous AuCla solution.…

A: Given : Time = 3.0 min = 3.0 X 60 = 180 s                                              (Since 1 min…

Q: If 12.3 g of Cu is deposited at the cathode of an electrolytic cell after 5.50 h, what was the…

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Q: (a) The half-reaction for formation of magnesium metalupon electrolysis of molten MgCl2 is Mg2+ + 2…

A: (a) The value of current for formation of magnesium is 60.0 A. The value of time taken for formation…

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The electrical energy which is generated in the lead storage battery will be equivalent to the…

Q: 10

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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…

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

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

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Q: How many seconds would be required to produce 50.0 g of Mg from MgCl2 if the current is 100.0 A?

A: According to Faraday's law of electrolysis, the weight of the substance deposited on any electrode…

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 lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

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, Current deposited = 2.50  Time = 2.95 h F = 96500 C/mol

Q: One of the half-reactions for the electrolysis of water is: 2H2O (l) -----> O2 (g) + 4H+ (aq) + 4e-…

A: According to the ideal gas equation, PV=nRT where P, V, n, R and T are the pressure, volume, number…

Q: How many grams of X (MW = 157.49 g/mol)(in g) will be deposited on a cathode in 2.11 h by a current…

A: Faradays First Electrolysis Law provides that the amount of reaction taking place on the basis of…

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 lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The discharging reaction if lead storage battery is given as:Pb (s) + PbO2 (s) + 2SO42- (aq) + 4H+→…

Q: Question attached

A: Given that: ECell=0.64 VEoPb2+/Pbs=−0.1263 VPb2+=0.010 MVO2+=0.10 MV3+=1.0×10−5 M Cathode:…

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: Copper from a 200.0 mL solution of copper (II) sulfate is plated on to the cathode of an…

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Q: • Part A A lead-acid battery uses a redox reaction in which lead(0) and lead(IV) are both converted…

A: The reaction given is, => Given: Time passed = 5.00 hours = 5 × 60 × 60 = 18000 s…

Q: An object is electroplated with rhodium for 28.2 minutes at current of 1.4 A. Rh3+ + 3 e Rh Molar…

A: According to Faraday's law of electrolysis, the amount of solid deposited is given by m =…

Q: alculate the value of the faraday if electrolysis of a NaCl solution with a current of 1.60 A for a…

A:

Q: 2. Tin-plated steel is used for tin cans. If the production of sheets of tin-plated steel requires…

A: Formulas used : I = q/t     where I is the current in amperes                            q is the…

Q: n a certain electrolysis experiment involving Al3+ ions, 63.7 g of Al is recovered when a current of…

A: 1 Faraday = 96500Columbs  Time = Charge/Current  Charge = current *time

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: (a)

Q: Thomas Edison invented an electric meter that was nothing more than a simple coulometer, a device to…

A: Introduction: According to Faraday's first law of electrolysis, the quantity of ion deposited ay…

Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation:…

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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 data Time : t=1.45 hr Current : i=2.50 A Faraday constant : F=96500 C/mole Mass of Cu…

Q: Calculate the value of the faraday if electrolysis of a NaCl solution with a current of 1.60 A for a…

A:

Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: (a) In the electrolysis of aqueous Naz2C204, how many liters of H2(9) (at STP) are generated by a…

A: The balanced chemical reaction can be written as follows: Na2C2O4 (aq) +  2H2O (l)  →  2CO2 (g) + H2…

Q: Electrosis... A current of 0.650 A deposits 0.413 g of a certain metal in 55.0 minutes.  Calculate…

A:

Q: A torch bulb glows with a current of 2.25 A for 24 minutes, what is the charge flowing through it?

A: We have given that Current (I) = 2.25 A t = 24 min = 24×60 = 1440 s Q = ?

Q: What mass of Cu(s) is electroplated by running 17.5 A of current through a Cu²“(aq) solution for…

A: Part A :  First we would Calculate charge using current and time.  From charge , we would calculate…

Q: How many grams of X (MW = 91.45 g/mol)(in g) will be deposited on a cathode in 1.15 h by a current…

A:

Q: 6) Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below.…

A: The reaction considered is, Cr2O7+ (aq) + 14H+ (aq) + 12 e-→12 Cr (s) + 7 H2O

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.