A constant current of 0.445 A is passed through an electrolytic cell containing molten BaCl2 for 21.9 h. What mass of Ba(s) is produced? The molar mass of barium is 137.3 g/mol. Provide your answer rounded to 3 significant digits.

Q: How many moles of oxygen, O2, will be produced by the electrolysis of water with a current of 1.5…

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Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Given that : The two half-reactions of the cell are :

Q: / minutes

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Q: How many seconds (s) are needed to deposit 3.62 g of copper metal from an aqueous solution of CuCl2,…

A: We have given current of 5.3 A . Mass of copper deposit required is 3.62 g Time required is being…

Q: Suppose a current of 890. mA flows through a copper wire for 18.0 minutes. Calculate how many moles…

A:

Q: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A  Mass of Cu = 79.5 g  Molar mass of Cu= 63.55 g mol-1 Time t= ?

Q: Suppose 490.mmol of electrons must be transported from one side of an electrochemical cell to…

A: Given that:  Electron transferred during reaction in electrochemical cell = 490mmol =…

Q: Metallic magnesium can be made by the electrolysis of molten MgCl₂. ▼ Part A What mass of Mg is…

A: Details

Q: The following reaction occurs in a galvanic cell. What is the shorthand notation of this cell?…

A: It is based  on  the concept of electrochemical  cell Here we are required  to  write  the…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

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Q: What current must be supplied to deposit 4.77 g of gold from a solution of AuCl 3 in 27.2 min?

A:

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: How many minutes does 5.857 A of current need to be applied to plate 3.870 g of aluminum onto a…

A: Given, the half-reaction: Al3+(aq) + 3e- → Al(s) We have to find the time required that a current of…

Q: Nickel can be produced when a current is passed through an aqueous solution of nickel (II) acetate.…

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Q: In a laboratory experiment, a student set up an electrochemical cell that contained sodium bromide,…

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Q: How many minutes does it take to plate 126.4 g of chromium onto a car part using 18.46 A of current?…

A:

Q: An alternator recharges an automobile battery when the engine is running. If the alternator produces…

A: Given, Current produced by alternator = 1.540 A Engine operations requires = 1.179 A  mass of…

Q: What is the amperage of a current if it takes 6.00 hours of the current passing through a 2.0 M…

A: The solution of the given question is

Q: Find the voltage of the cell if the right half-cell contains 0.330 M AgNO₃ (aq) and the left…

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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: Suppose a current of 520. mA flows through a copper wire for 27.0 minutes Calculate how many moles…

A: Given information: Time (t) = 27.0 minutes Current (I) = 520 mA

Q: How many minutes does it take to plate 228.6 g of chromium onto a car part using 19.24 A of current?…

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Q: current

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Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ Cu*…

A: Answer :- Ecell = 1.09 (V) The cell voltage (Ecell) for given cell = 1.09 V…

Q: The gold plating of a ceramic figurine requires a total of 4.19 g of solid gold.  If the current…

A: Given  Mass of solid gold required = w = 4.19 g Current being used is = I = 11.0 amperes how many…

Q: A certain metal M forms a soluble sulfate salt MSO4. Suppose the left half cell of a galvanic cell…

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

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.