You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many moles of solid aluminum metal would be formed? Report your answer in units of moles rounded to the nearest thousandth.

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: Faraday’s first law of electrolysis:                 The mass of the substance deposited at the…

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

A: Faraday's first law of electrolysis states that the mass of substance deposited is directly…

Q: If the given statement is true, write T. Otherwise, write F and explain why it is false. 1) The…

A: Given the statement: The electrons in a galvanic cell can be transferred through a wire, making it…

Q: A current of 12.0 A is passed through molten magnesium chloride for 14.0 h. How many moles of…

A: Given: Current = 12.0 A Time = 14.0 h

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: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

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: The mass of three different metal electrodes, each from a different galvanic cell, were determined…

A: The active electrode which is found to lose mass during redox reaction in a cell is termed as anode…

Q: Consider the electrolysis of tin (II) sulphate during which tin is deposited at one electrode and…

A: A numerical problem based on electrolysis, which is to be accomplished.

Q: Use information from Table 17.1 (pp. 907-909 of your textbook) to answer this question.  What is the…

A: In the given cell we can see that the oxidation of Al is taking place and reduction of Cr3+  Hence…

Q: A steady current was passed through molten CoSO. until 2.35 g of metallic cobalt was produced.…

A:

Q: Explain the different parts of a galvanic cell and also include its functions.

A: A galvanic cell is a device in which chemical energy is converted into electrical energy as a result…

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: A current 6.0 amperes is passed for 10 hours between copper electrodes in 800 ml of copper nitrate…

A: The charge carried by one electron is 96500 C. The electrode reaction:

Q: Suppose 220. mmol of electrons must be transported from one side of an electrochemical cell to…

A: Given  mmol of electrons = 220  Time = 214 s  We have to calculate current

Q: A current of 5.25 A is passed through an aqueous solution of copper(II) nitrate for 71.0 min. How…

A: An swer:- this question is answered by using the simple concept of calculation of mass of a metal…

Q: Calculate the theoretical cell potential of the following cell. If the cell is short-circuited,…

A: The given cell notation is: Ag(s)|Ag+(aq)(0.0575 M) || H+(aq)(0.0333 M)| O2(g)(1.12 atm), Pt The…

Q: 1. What is a cell potential? 2. In what way does a galvanic cell becomes an electrolytic cell?

A: Galvanic cell is the spoteneous redox reaction where chemical energy transferred to electrical…

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: Zinc metal is deposited onto a cathode surface by passing a current of 1.87 amps through a solution…

A:

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: A constant current of 90 mA is passed for 22 minutes into an electrolysis cell. How much electrical…

A: Charge passing per unit time is known as  electric current.

Q: 4. In a process called flash electroplating, a current of 2.5 x 10'A passes through an electrolytic…

A:

Q: An aqueous solution contains a mixture of cations at the following concentrations.…

A: An aqueous solution containing a mixture of three cations, for which the order of reduction is to be…

Q: How are standard electrode potentials measured?

A: Standard electrode potential is referred to Eo of a cell and is in an electrochemical cell at a…

Q: standard potential

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Q: what is the standard cell potential (in Volts) for a a galvanic cell that can do 567 kJ of work. The…

A: The solution is as follows :

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

A: Electrolysis is a process in which current is passed through a substance .In this chemical reactions…

Q: In an electrolytic cell, does the reaction of electrolysis of water take place in a standard state?

A: Here we to explain whether the reaction of elctrolysis of water takes place in standard state or…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

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: Using the Standard Reduction Potential Table, use half-reaction potentials to identify whether the…

A:

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: The mass of aluminum metal calculated as follows

Q: Given the following cell notation for a galvanic cell, calculate the cell potential. Mg(s)|Mg²+ (aq)…

A:

Q: a) A proposed battery involves the reaction of Zn(s) and Cl2(g) to give ZnCl2. If you want such a…

A: Hii there, since there are multiple questions posted. We are answering first question. If you need…

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: Electroplating is a process of coating layer of metal over another metal by the process of…

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: Will the potential of the galvanic cell change if we add the same amount of water to the electrolyte…

A: Cell potential is given by Nernst equation , which is as: Ecell = Eocell - RTnFlnQ  Cell potential…

Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

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Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 5.1…

A: Solution: From the Faraday first law we have, the amount of chemical change being produced by a…

Q: A galvanic cell runs for 1 minute with a current of 0.25 A. How much charge passed through the cell…

A: Given : Current passed = 0.25 A And time = 1 min F=96500 C/mol

Q: Faraday constant. Suppose that after the electroplating was complete, you wiped the cathode copper…

A: Explanation to the correct answer is given below

Q: Why is it necessary to use salt bridge in A galvanic cell?

A: Galvanic cell is the other name for electrochemical cell in which chemical energy is transformed…

Q: A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery…

A: m=Mass of Hg=1.10g Equivalent wt of Hg =200.59/2 =100.295 Current = 0.10 mA or 0.10x10-3 F=96500C…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A:

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…

Q: Calculate the standard free-energy change of a voltaic cell with a potential of 0.35 V under…

A: Given data: E0cell = 0.35V no of moles(n) = 2moles of electron formula used: ∆G0 = -nFE0cell  Where…

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.