Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a current of several amperes through a copper sulfate solution (CuSO4) for a period of time and determining the mass of copper plated onto the cathode. If it is found that a current of 1.00 A flowing for 3600 s deposits 1.185 g of copper, find (a) the number of copper atoms deposited, (b) the weight of a copper atom, and (c) the molar mass of copper.

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Cu²* (aq)+…

A: The reaction given is, Cu2+aq+Zns→Cus+Zn2+aq Cu2+ is being reduced to Cu and Zn is being oxidised to…

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

A: Step 1:

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

Q: A certain half-reaction has a standard reduction potential Ed=+0.73 V. An engineer proposes using…

A: Given,The standard reduction potential: , this is the reduction potential of the anode.Also,  (at…

Q: A certain half-reaction has a standard reduction potential Ed +1.01 v. Ar engineer proposes using…

A: E°red(at cathode ) =+1.01 V E°cell=1.30 V

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

A: The reaction given is Hence in the above reaction, Sn2+ is being reduced to Sn and Ba is being…

Q: A certain half-reaction has a standard reduction potential Ered = +0.73 V. An engineer proposes…

A: Ecello=1.00 VEcathodeo= +0.73 V

Q: A galvanic cell is based on the following reaction(at 25°C)： Cu (aq)+Sn(s) → Cu(s)+Sn (aq) If the…

A: Note - The given reaction is incorrect. So, we will use the correct reaction for the question.   A…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2Cr (aq)…

A: The oxidation and reduction half cells are as follows: Oxidation: 3Ca (s) →3 Ca+2     E0= -2.87…

Q: In the commercial preparation of aluminum, aluminum oxide, Al,O3, is electrolyzed at 1000°C. (The…

A: Since from the above reaction we can see that 1 mole of Al is produced when 3 moles of electrons is…

Q: Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be…

A:

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: 1 F = 96500 C  Moles of chlorine = 1090 / 71 = 15.35 moles  Total charge = 2 × 15.35  F = 2 × 15.35…

Q: Calculate the maximum work available (in kJ) from 52.3 g of aluminum in the following cell when the…

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Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

A:

Q: A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9…

A: We will use relation of mass and gm equivalent

Q: Metallic magnesium can be made by the electrolysis of molten MgCl2 What mass of Mg is formed by…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A: Given data,Current=29.0ATime=69.0sReaction at cathode;Pb2++2e-→Pb(s)

Q: When lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

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

A:

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

A: The cell reaction taking place is given as, => Sn2+ (aq) + Ba (s) -------> Sn (s) + Ba2+ (aq)…

Q: Consider the galvanic cell. In a certain experiment, the emf () of the cell is found to be Q.54 V at…

A: Solution :    Nernst equation is used to calculate the potential of the cell at non-standard…

Q: A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M1.0 M iron(II) ion…

A:

Q: A certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using…

A: Eoanode= 0.21 V - 1.0 V = -0.79

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

A:

Q: A current of 13.4A is passed through an electrolysis cell containing molten NaCl for 16.8 minutes.…

A: The objective of the question is to predict the products of electrolysis of molten NaCl and to…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn n²* (aq)…

A:

Q: When a lead acid car battery is recharged by the alternator, it acts essentially as an electrolytic…

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: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A:

Q: Determine the amount of time (in hours) that a 16.8 ampere current must be applied to a 2.0…

A: The objective of the question is to find out the time required to produce a certain amount of Zinc…

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.