Calculate the number of moles of electrons driven through an electrolytic cell with 3865 A of current passing through for 5 minutes. Round your answer to 2 decimal places.

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: 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: Calculate the number of moles of electrons driven through an electrolytic cell with 3941 A of…

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Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3457 A of…

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Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3906 A of…

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Q: An aqueous solution of gold nitrate is electrolyzed with a current of 0.555 ampere until 1.32 g of…

A: The relationship between charge (q), time (t), and current (I) can be given as: q=I×t…

Q: A current of 2.345 A passes through the cell shown for 45 minutes. What is the volume of the…

A: It is a term used in chemistry when a substance undergoes a reaction in which it ends up gaining an…

Q: How many moles of oxygen, O 2, will be produced by the electrolysis of water with a current of 1.5…

A:

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: The charge carried by 610A of current in 77 seconds is the product of current and time.q is the…

Q: Electrolysis was performed to determine the identity of an unknown metal X. It was determined that 3…

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Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3778 A of…

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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: In an electrolytic cell, two inert carbon electrodes were immersed in an aqueous solution of tin…

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Q: Calculate the mass of cobalt plated onto the cathode of an electrolytic cell by a current of 15.0 A…

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Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3455 A of…

A: 1- First we will determine the charge of number of electrons :  We used the formula,  Q = I × t…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3097 A of…

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Q: Suppose a current of 590.mA flows through a copper wire for 277. seconds. Calculate how many moles…

A: It is given that:Amount of current flowing through the copper wire = 590 mATime = 277 seconds

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: Calculate the number of moles of electrons driven through an electrolytic cell with 3376 A of…

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Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A:

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: ASAP How many moles of Aluminum are produced by decomposing molten Al2O3 in 1.05 hours when the…

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Q: What volumes of H2(g) and O2(g) at STP are produced from the electrolysis of water by a current of…

A: According to Faraday's 1st law weight of the substance from in each electrolyte  W = ZIt where , W…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3512 A of…

A: The given data is as follows: Current = 3512 A Time = 4.5 minutes =4.5×60 seconds=270 seconds The…

Q: Suppose 0.680 mols of electrons must be transported from one side of an electrochemical cell to…

A: The relation between current, charge and time is given by the Ohm’s law according to which the…

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: Calculate the number of moles of electrons driven through an electrolytic cell with 3444 A of…

A: Consider the given information is as follows; Current (I) = 3444 A Time (t) = 4.6 min = 4.6 min × 60…

Q: A 0.1 M aqueous CaCl, solution is electrolyzed by usina inert electrodes. If 1.25 ampere current is…

A: At cathode this reaction is taking place,Ca2+  +  2e-   →  Ca  Calculate the charge first,Q = it and…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3304 A of…

A: Consider the given information is as follows; Current passed (I) = 3304 A Time (t) = 3.5 minutes =…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3676 A of…

A: Given data: Current passed (I) = 3676 A Time (t) = 4.4 minutes = 4.4×60=264 sec        Number of…

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3032 A of…

A: Number of moles of electrons,n=Charge (Q)Faraday constant (F) Charge,Q=Current (I)×Time(t)

Q: In the industrial "chlor-alkali" process, pure chlorine and sodium hydroxide are produced by…

A: When 96500 coulombs are passed through a solution of NaCl, one mole of chlorine is deposited.

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

A:

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3715 A of…

A:

Q: Calculate the number of moles of electrons driven through an electrolytic cell with 3503 A of…

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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.