A steady current of 3 A is maintained for 10 mins in AgNO3 solution. How much Ag is deposited at the cathode?

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 long will it take for a uniform current of 6.00 A to deposit 78.0 g gold (197.0 g/mol) from a…

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Q: (b) A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: How many minutes will it take to plate out 40 g of Ni from a solution of NISO4 using a current of…

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Q: How many grams of gold will be plated out by a current of 0.35 A applied for 65 minutes from a…

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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: A current of 11.8 A is applied to 1.25 L of a solution of 0.549 mol L- aqueous HBr converting some…

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Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

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

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Q: What amount of Cu (in grams) is deposited at the cathode when a current of 6 A is maintained for 15…

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Q: Suppose a metal electrode is being coated with silver according to the half-reaction, Ag+(aq) + e-…

A: Current = 0.850 A Time = 20.0 min  ....Or = 20.0 min × (60 sec / 1 min )   ...(because, 1 min = 60…

Q: Calculate the mass of silver deposited at the cathode during electrolysis when a current of 1.80A…

A: Given that , Current (I) = 1.80 A Time (t) = 45 min = 45 x 60 = 2700 sec Electro chemical equivalent…

Q: How long, in hours, must a current of 5.00 A be applied to a solution of Ag+ to produce 10.5 grams…

A: From the combination of Faraday's first and second law, we have : m = ItM/Fz  Or, t = mFz/IM ...(1)…

Q: S. Given the following reduction half-reactions at 298 K: Half-Reaction E (V) at 298 K Fe" (aq) + e→…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

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

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Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given: Current = 2.96 A Time = 33.4 min Mass of V deposited at cathode = 0.784 g Molar mass of V =…

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: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

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

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Q: Given the following unbalanced½ reactions and their respective reduction cell potentials: Ni0,(s) →…

A: Given that, the unbalanced half-cell reaction and their respective reduction potential values:…

Q: What mass of copper could be deposited from a copper(II) sulfate solution using a current of0.50 A…

A: The given problem can be solved by using the formula as; Q=I×t…

Q: How long will it take to deposit 1.5 g of Cu on a metal when a current of 5 A is applied to a CuSO4…

A: Given- Amount of copper = 1.5 gMetal of interest = CuCurrent = 5 A To find- Time required

Q: For the following galvanic cell: Zn(s) + Ni+2(aq) → Zn+2(aq) + Ni(s) A. Of the two half reactions…

A: Since you have posted question with multiple subparts as per guidelines we can answer only three per…

Q: Gold can be plated out of a solution containing Au3+ according to the following half-reaction: Au 3+…

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

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Q: A solution containing vanadium (chemical symbol V) in an unknown oxcidation state was electrolyzed…

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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: At a steady current of 5 A and a time of 20 minutes, which of the metal will deposit more metal at…

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Q: Consider the following reaction and its AG AG° = -408.0 kJ/mol Mg(s) + Ni?+(aq) → Mg²+(aq) + Ni(s)…

A: Given-> Mg(s) + Ni2+(aq) ----> Mg2+(aq) + Ni(s)  ∆G° = -408.0 KJ/mole = -408000 J/mole (1 KJ =…

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

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Q: Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 A was passed through…

A: Faraday law states that the amount of any substance deposited or liberated during electrolysis is…

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

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Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: A student constructs an electrochemical cell with a half-cell composed of a nickel anode in a 0.10 M…

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Q: Consider the following reaction and its AG" at 25.00 °C. Mg(s) + Ni" (aq) – Mg²* (aq) + Ni(s) AG =…

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Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: Given values:I = 0.912 ATime = 18.5 h It is known that 1 h = 3600 sec.Therefore, 18.5 h = 18.5×3600…

Q: What mass of Sn(s) may be deposited from an aqueous SnCl, solution if a current of 2.50 A is applied…

A: Given,

Q: How many grams of  zinc metal will be deposited from a solution that contains  Zn^2+ ions if a…

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: How long will it take to deposit 1.5 g of Ag on a metal when a current of 2 A is applied to Ag+…

A: In electrolytic cells, electric energy is converted into chemical energy to run a chemical reaction.…

Q: products

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Q: A steady current of 5 A is maintained for 120 seconds in CUSO4 solution. How much Cu is deposited in…

A: The charge deposited is given by the product of charge and time. Q=It where I is the current and t…

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…

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) = ?

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

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.