current of 6.6 A is passed through a solution of AgNO3 to electroplate it onto a surface. Calculate the mass, in grams, of pure silver deposited on the surface after 77 seconds.

Q: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

Q: How many grams of silver metal will be deposited from a solution that contains Ag+ ions if a current…

A: As per the given information the balanced chemical cathode half reaction is as follows:…

Q: Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

A: GIVEN:

Q: Three electrochemical cells were connected in series so that the same quantity of electrical current…

A: Concept introduction: Faradays second law of electrolysis is explained as when the same quantity of…

Q: An electrochemical cell is constructed using a copper cell as the anode and the bromate/bromide cell…

A: The balanced redox reaction involved:3 Cu(s) + BrO3–(aq) + 6 H+(aq) → 3 Cu2+(aq)  + Br–(aq) + 3…

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

A: Current =5.00×10^2A Mass of chlorine=4.18kg=(4.18×1000)g=4180g

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

A:

Q: How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: The balanced chemical equation for the reduction of copper is: Thus, for the production of 1 mole…

Q: According to the reaction, Ag+ (aq) + e- --> Ag(s), silver is deposited. For 30.0 minutes, a 0.800A…

A:

Q: An electrolytic cell produces aluminum from aluminum oxide, Al2O3. What mass of aluminum can be…

A: Applying formula w=Zit

Q: impure

A: According to this law,  mass diposite on cathode is direactly proportion to the current.  So,…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2 Cr³+(aq)…

A: In the given galvanic cell ->Concentration of Cr3+ = [Cr3+(aq)] = 4.87 MConcentration of Ca2+ = […

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

A:

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

A:

Q: A galvanic (voltaic) cell consists of an electrode composed of chromium in a 1.0 Mchromium(III) ion…

A: Here we are required to find the standard cell potential of the given electrochemical reaction

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

A: Since in the above reaction we can see that 1 mole of Cl2 is produced with 2 moles of electrons…

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: In a galvanic cell, one half-cell consists of gaseous chlorine bubbled over a platinum electrode at…

A: (a) Write balanced equations for the half-reactions at the anode and the cathode. The cathode half…

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

A:

Q: How many seconds are required to deposit 0.136 grams of copper metal from a solution that contains…

A: Given, mass of Cu deposited = 0.136 g Current passed = 0.913 A 1 Faraday is the magnitude of charge…

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that  An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

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

A:

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

A:

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: Electroplating is rarely 100% efficient-some of the current usually is consumed by reactions other…

A: Amount of current passed = 6A Time for the flow of current = 15 minutes =15×60 s = 900 s Mass of…

Q: A voltaic cell (also called a galvanic cell) was constructed by connecting two beakers with a salt…

A: Given: Standard half-cell reduction potentials:Fe2+(aq)  +  2e-  ----->  Fe(s)     E o  =  -0.45…

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

A: Faraday's first law of electrolysis It states that the mass of a substance deposited on any…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Cu²+ (aq) = Ti²+…

A: The given red-ox reaction is  Ti(s) + Cu2+(aq) Ti2+(aq) + Cu(s)Given: The concentration of Ti2+,…

Q: How long would it take to deposit 9.38 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: Given, m = 9.38g I= 23.2A

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

A: According to the Faraday's law of electrolysis, the mass of Substance liberated or deposited at any…

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

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.