QUESTION 5 ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.65 minutes for a current of 1.09 A to plate 0.0951 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.) QUESTION 6

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: Gold ion gains 3 electrons to get reduced to gold as per below equation Au3+ + 3e-  --> Au

Q: In an electrolytic cell, there is a mixture of the molten salts NaCl and KBr. If a current of 0. 12…

A: Electrolytic cell is a cell where electric current flow is responsible for happening a non…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

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

A:

Q: A constant current of 9.25 amperes is passed through a cell containing iridium (III) nitrate,…

A: We have current as 9.250 A , time as 7.57 hrs, deposit of Ir is taking place, we have to calculate…

Q: 1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic…

A: Since you have asked multiple questions we will solve the first one for you. If you want the answer…

Q: Calculate the mass of Ag metal generated when Ag(NO3)(aq) is electrolysed for 20.5 minutes with a…

A:

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.54 minutes for a current…

A: Charge = current *time (in s)  Charge = 1*2.54*60 = 152.4 C

Q: Zn 0.10 60 The diagrams above illustrate the equipment used to electroplate four identical objects…

A: Electrochemistry is the branch of chemistry which studies the change of chemical energy into…

Q: Consider an electrolytic cell with a steady current of 158 amperes which produces Als) (atomic mass…

A:

Q: 6. A 1M aqueous solution of chromium (I) bromide will be electrolyzed to "chrome plate" a faucet.…

A: As per the Faraday's 1st law of electrolysis: w=ZIt      ----(1)where,w = weight of the substance…

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

A: Using Faraday's First of electrolysis: w = ZIt Z = Equivalent mass of metal96500w = Molar mass of Cu…

Q: For Questions 1 to 4: Giorno Giovanna likes golden stuff. However, since he is currently broke, he…

A: 1.) To calculate number of electrons needed , we would write an equation to change Au3+ to Au . 2.)…

Q: how can standard reduction potential be applied in real-world applications

A: Uses of standard electrode potentials are listed below – It is used to measure relative strengths…

Q: The following questions refer to the electrochemical cell shown in the diagram above. a. Write a…

A: Standard cell potential  E°cell = E°reduction - E°oxidation  E°oxidation and E°reduction are the…

Q: 10

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Q: half-reaction occurs at the cathode

A: Reduction takes place at cathode and oxidation takes place at anode.

Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: NOTE: Since there are no question in part (i), I'm solving the next 3 sub-parts.

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A: Gold ion is triply charged Au3+ To get reduced to metal, ions gain electrons

Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: Use the first law of Faraday.

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

A:

Q: Masakatsu plans to create counterfeit gold badges through electroplating. In a filled 500-mL tub, A…

A: Given: Current passed = 875 mA = 0.875 A                                 (Since 1 A = 1000 mA) And…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.61 minutes for a current…

A:

Q: Determine the molar mass (amu) of Metal (M) if it took 2.95 minutes for a current of 1.8 A to plate…

A:

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: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

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

A: Mass can be calculated as:-

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 2.21 minutes for a current…

A: To solve this problem we will the formula  m = Z •i•t  Where ,  m = mass of metal  Z =…

Q: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer :  We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current…

A: Answer :- Molar Mass = 144.52  ------------------------------------------------

Q: d) What is the equilibrium direction of the reaction? Write "a" if the reaction is spontaneous in…

A: Answer              Consider the following cell Mns|Mn Br20.046…

Q: Giorno Giovanna likes golden stuff. However, since he is currently broke, he has to settle for…

A:

Q: A concentration cell based on the following half reaction at 310 K Mg + 2e – Mg; SRP = -2.37 is made…

A: Since the standard cell potential of a concentration cell is 0, the potential of a concentration…

Q: 1. An electrochemical cell is made of two electrodes: (Zn²+/Zn) and (Ag*/Ag). Use the standard…

A: Electrochemical cell: Cell in which electricity is produced by the action of chemical reaction…

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 current of 0.46 A was passed through a copper (II) sulfate solution using copper electrodes for 16…

A: According to faraday law of Electrolysis:

Q: ) Show the equation and describes Faradays law which relates moles of analyte to charge in coulombs…

A: #(d): Faraday's first law describes the relation between the moles of the analyte deposited at the…

Q: 1. Fischl, a scientist from Mondstadt specializing in electrochemistry, performed an electrolytic…

A: Given: The mass of metal deposited = 9.701 g. The current passed, (i) = 1.500 A. The time of passage…

Q: The diagrams above illustrate the equipment used to electroplate four identical objects with silver…

A: The correct answer is explained below.

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

Q: In a standard electrochemical cell, A4+ is reduced to solid A, while gaseous Z2 is oxidized to Z3-.…

A:

Q: Suppose the current flowing from a battery is used to electroplate an object with silver. Calculate…

A: The electrochemical reaction of silver is –

Q: Use the Nernst equation to calculate the cell potential,  EcellEcell, for a galvanic cell…

A: The half cell reactions are   Pb+2 (aq)+ 2e− ⇌ Pb  E° =  –0.126 V   Fe+2 (aq)+ 2e− ⇌ Fe (s)   E° =…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.63 minutes for a current of 1.04 A to plate…

A:

Q: A galvanic cell runs for 1 minute with a current of 0.20 A. How much charge passed through the cell…

A: Given : Current passed = 0.20 A And time = 1 min

Q: 5. Consider the reaction, Li+28r → Brz+Li What is the standard potential for this reaction? For the…

A: 6) Given that: Current (I) = 5.2 A Time (t) = 8 s Charge (Q) = ?

Q: How many grams of Ca metal (atomic mass = 40.08 g/mol) are produced by the electrolysis of CaBr,…

A:

Q: Consider an electrolytic cell with a steady current of 174 amperes which produces Als) (atomic mass…

A:

Q: 2. A spoon of surface area 20.0 cm² needs to be electroplated with silver to a thickness of 100 µm.…

A: The question has asked to calculate the time for which current will flow to deposit the required…

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.