Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag+(aq)+e−→Ag(s) What mass of silver plates onto the cathode when a current of 6.4 A flows through the cell for 69 min ? Express the mass in grams to two significant figures.

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: Consider the following cell notation : Cr (s) |Cr^ 3+ (aq)||H 3 AsO 4(aq) ,H^ * (aq),H 3 AsO 3(aq)…

A: In the cell notation, the left most part indicates anode. At anode oxidation takes place. After the…

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

A: Given: Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s)

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

A: The given reaction is, 2Cr3+aq+3Cas→2Crs+3Ca2+aq The half cell reactions and their standard…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized…

A: In cell notation anode is written on left side and cathode on right side.

Q: NO3 + H* + Zn → Zn²+ + NO2 + H2O

A: Given skeletal equation is: NO3-+H+ +Zn →Zn2++NO2 +H2O Calculate its standard cell potential(Eo) and…

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

A:

Q: Cl2 + Br → Ch + Br2

A: The questions are based on the concept of redox reactions.   Redox Reaction  are those reactions in…

Q: A galvanic cell is powered by the following redox reaction: 3 Cl,(g) + 2 MnO,(s) + 8 OH (aq) + 6 Cl…

A:

Q: A galvanic cell with a voltage of 1.3 V utilises the reaction: Zn + Cu2+ →→ Cu + Zn2+, as a source…

A: Given: The cell voltage is 1.3 V. The amount of Cu and Zn used is 6.3 g and 11 g, respectively.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq)+…

A:

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

A:

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: Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction:…

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

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

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

A:

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 8.3 amperes passes…

A:

Q: Write the cell notation for an electrochemical cell consisting of an anode where Pb (s) is oxidized…

A:

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

A: Given cell reaction  Sn2+(aq) + Ba(s) ----> Sn(s) + Ba2+(aq) At Ba electrode oxidation taking…

Q: When an aqueous solution of potassium iodide is electrolyzed using platinum electrodes, the…

A: 8.15mA current flows which is equal to 0.00815A time is 12.6min = 756s The molar mass of I2 =…

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: How many grams of chromium metal are plated out when a constant current of 8.00 A is passed through…

A:

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: Calculate the standard emf of a cell that uses Ag/Ag¯ and Al/Al³* half-cell reactions. Write the…

A: Please find your solution below :

Q: Tin-plated steel is used for "tin" cans. Suppose that in the production of sheets of tin-plated…

A:

Q: How long, in minutes, will it take to produce 370.0 g of pure lithium by running a current of 330 A…

A: Given, Current passing = 330 A Mass of Li = 370.0 g  Molar mass of Li = 6.94 g/mol

Q: Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an…

A: Please find the answer attached here as handwritten note.

Q: construct a cell under standard conditions. The anode and cathode are iron and silver rods. Using…

A: We have to give information about the given cell

Q: Write the cell notation for an electrochemical cell consisting of an anode where Co (s) is oxidized…

A:

Q: A current of 0.452 Amps is passed through an electrolytic cell containing molten CaCl2 for 1.50 hrs.…

A:

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

A: The given redox reaction is,                                   3 Cu2+(aq) + 2 Al (s) ----> 3…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn²* (ag)+Ba…

A:

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl, (g). The reaction that…

A:

Q: You pass a 2.5 amp current through an aqueous solution of aluminum nitrate for 5 hours. How many…

A: Aluminium nitrate Al(NO3)3 has Al3+ ions Al3+ + 3 e-  -----> Al So to reduce 1 mole Al3+ ions to…

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

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

A: The cell reaction taking place is given as, => 2 Cr3+ (aq) + 3 Ca (s) -------> 2 Cr (s) + 3…

Q: In the electrolysis of molten MgCl 2, what mass of Mg metal is deposited by a current of 16 amperes…

A: Electrolysis is the process of conversion of electrical energy to chemical energy. This reaction…

Q: Write the cell notation for an electrochemical cell consisting of an anode where Cr (s) is oxidized…

A: Cell notation is a way to represent an electrochemical cell with anode and cathodes.

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: What is the maximum electrical work obtainable from this cell when 0.150 g of Al is consumed?

A: Provided data :- E°cell = 1.63 V  Cell reaction :- Al(s) + Cr3+(aq) -> Cr(s) + Al3+(aq) It means…

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…

Q: Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these…

A: For a.) Adding these 2 eqn we get,

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.