1. a)How many grams of zinc metal will be deposited from a solution that contains Zn2+ ions if a current of 0.984 A is applied for 56.8minutes. ________grams

Q: E°zn2-/z0) = -0.763 V MMz = 65.38 g/mol Zn2+(aq) +2e--Zn(s) a.) If a current of 35.0 amps flows for…

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

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Q: (b) A constant current was passed through a solution of AuCl; between gold (Au) electrodes. After a…

A: Given, Mass of gold deposited = 2.628g Time = 20min = 1200 second

Q: What current strength in ampere will be  required to liberate 10 g of chlorine from  sodium chloride…

A: To solve this question, use faraday's law of electrolysis which is given as follows:- m = I×tFMZ Use…

Q: The standard addition method is used to determine the concentration of vitamin C in apple juice by…

A: Given : Initial volume of sample of apple juice = 2.00 mL Final diluted volume of apple juice = 25.0…

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: How many seconds are required to deposit 0.266 grams of cadmium metal from a solution that contains…

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

A: Given :  Current (I) = 0.599 A  Time(t) = 28.4 min = 28.4 x 60 sec = 1704 sec  Molar mass of Hg =…

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: Q2: Calculate the potentials of the following cells (a) Pb|Pb2+ (0.1393 M)||Cd²+(0.0511)|Cd (b)…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

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

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Q: What mass of Ni(s) may be deposited from an aqueous NiCl2 solution if a current of 2.50 A is applied…

A: Reaction occuring  Ni+2 (aq) + e-  --------> Ni(s)

Q: mass of copper

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Q: when using the equation Q=It in electro chem, how do you find the Q value if not given t. Is it mols…

A: In the equation, shown in equation (1), t is defined by time duration for the current of I (in A),…

Q: 16. An electrochemical cell containing zinc sulfate with a Zn electrode is connected in a series…

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

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

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

A: Given,

Q: Question attached

A: The SHE (Standard Hydrogen Electrode) is one of the reference electrodes used in the electrochemical…

Q: The moving boundary method was applied to a solution of GdCl3 33.27 mmol/L at 25°C using LiCl. Using…

A: In the moving boundary method, the speed of displacement of the boundary is measured between two…

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

A: The charge is directly proportional to the current and time associated with it. According to…

Q: Which species can be oxidized by Pb2+(aq)? Calculate the voltage for this/these process(es).

A: In the electrochemical series from Li (-ve Standard reduction potential) to F (+ve standard…

Q: A certain metal is used in catalytic converters to reduce harmful emissions from vehicles. A 12.55 A…

A: Given, Current (I) = 12.55 A Time (t) = 22.41 min = 22.41 × 60 s = 1344.6 s number of moles of M…

Q: A particular manufacturing metal is used in the of steel, aircraft parts, and batteries. A solution…

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

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Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

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: At the Nernst potential for Na+, the current is 0.

A: Given information,At the Nernst potential for Na+, the current is 0.

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

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Q: 405−mL solution of NaCl was electrolyzed for 5.80 min. If the pH of the final solution was 12.23,…

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Q: How long must a current of 0.40 AA   A pass through a sulfuric acid solution in order to liberate…

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Q: If a current of 5.00 A is applied for 96.00 minutes, how many grams of magnesium will be formed?…

A: To find weight of magnesium

Q: How many grams of aluminum metal will be deposited from a solution that contains Al3+ ions if a…

A: Faraday's first law of electrolysis states that during an electrolysis reaction the mass of the…

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: What amount of electrons, in moles, is required to perform the electrolysis? 0.420 mol Sc desired 3…

A: Molar mass of Sc = 44.95 g/mol

Q: How long will it take to plate out 1.2 g Ni from aqueous Ni2+ with a current of 112.4 A? WHERE ARE…

A: Given,   1.2 g Ni plate out from aq Ni2+ with a current of 112.4 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: Ascorbic acid (Vitamin C) in a 50.0mL sample of orange juice was analyzed by an electrochemical…

A: Given:Initial Volume of juice(ascorbic acid) Vi = 50 mLVolume of Standard ascorbic acid solution…

Q: How many seconds are required to deposit 0.278 grams of manganese metal from a solution that…

A: Electrical charge is defined as the multiplication of current and time. It is measured in coulombs.…

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 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 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: The limiting current of lead in an unknown solution is 5.60 μA. One milliliter of a 1.00 × 10-3 M…

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

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

A:

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

A:

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.