A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at 25.0°C and each compartment has a volume of 219 mL. The cell delivers 0.25 A for 31.5 h. (a) How many grams of Cu are deposited? 4) 9.3 (b) What is the [Mg2+ ]? Assume constant volumes. 40.66826 X mol·L-1

Q: What is the electrical current, in Amperes, that must be applied if 6.50 g Ag is deposited at the…

A:

Q: Magnesium metal can be produced industrially by electrolysis of MgCl2. What mass of magnesium metal,…

A:

Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s) + Au³+ (aq)= Al3+(aq)…

A:

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

A: Given-> Concentration of VO2+ = 3.63 M Concentration of H+ = 1.38 M Concentration of VO2+ = 0.607…

Q: A metallic object to be plated with copper is placed in a solution of CuSO.. What mass of copper…

A: Given,  Current, I = 0.22 amp  Time, t = 1.5 hours               = 5400 sec  Molar mass of Cu =…

Q: If the potential of a cell is 0.51 V at 25°C when [Zn2+(aq)]=0.111M and the pressure of the hydrogen…

A:

Q: In the electrolysis of water, how long will it take to produce 155.0Lof H2 at 1.0 atm and 273 K…

A:

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

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

Q: A molten binary salt, Cal2, is electrolyzed. Write the half reactions that occur and identify which…

A: The binary salt given is CaI2  hence it has cation Ca2+ and anions I-

Q: Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate…

A:

Q: In the electroplating of nickel from a solution containing Ni2+ ions what weight of nickel-metal…

A:

Q: A galvanic cell is constructed that carries out the reaction 2Ag(s) + Cl2 (g) → 2Ag+(aq) + 2CI- (ag)…

A:

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited,  W = ZCt Where,   t = time in second…

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: How much Ca will be produced in an electrolytic cell of molten CaCl2 if a current of 0.452 A is…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq)…

A:

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

A: The standard electrode potential for the given cell is calculated as shown below. The standard…

Q: Suppose a metal electrode is being coated with silver according to the half-reaction, Ag+(aq) + e-…

A: Current = 0.850 A Time = 20.0 min  ....Or = 20.0 min × (60 sec / 1 min )   ...(because, 1 min = 60…

Q: A common car battery consists of six identical cells each of which carries out the reaction:…

A:

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: Faraday's law states that the amount of chemical change that is produced by passing a current to an…

Q: A student wishes to set up a voltaic cell that is a concentration cell made using two solutions of…

A: Concentration cell and cell potential calculation :

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

A:

Q: 3. The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a Cuso,…

A: The Faraday's laws are the main concepts of electrochemistry.  The first law shows  the connection…

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

A:

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

A: Oxidation is lose of electrons. Reduction is gaining of electrons. Galvanic cell is an…

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: ulate the potential of the following cells: a galvanic cell consisting of a lead electrode on the…

A:

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

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

Q: An electrochemical cell is constructed by dipping a zinc rod in a solution of Zn(NO3)2(aq), dipping…

A: The equilibrium constant can be written as the ratio of concentration of products to the…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au³*(aq) =…

A: Given:  Temperature (T)=25oC                             =(25+273)K…

Q: In an electrolytic cell, how many grams of nickel (MM = 58.69 g/mol) will be deposited on a metal…

A: we have to calculate the mass of Ni deposited

Q: A solution of CuSO4 is electrolysis for 10 minutes with a current of 1.5 amperes. What is the mass…

A:

Q: The electrolysis of an aqueous solution of potassium iodide, KI, results in the formation of…

A: Electrolysis: It is a chemical reaction that occurs when an electric current is conducted through a…

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: A Zn Zn2 + Co 2+ Co  galvanic cell is constructed in which the standard cell potential is 0.48 V.…

A: Given: A galvanic cell :                    ZnZn2+Co2+Co                  E0cell = 0.48V = 0.48 JC-1…

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

A: Answer = 1268.9 min

Q: Under standard conditions, the galvanic cell shown above has a cell potential of+1.56 V using the…

A: Using nernst equation of cell we can determine the effect of precipitation of Zn(OH)2.

Q: Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs…

A: In order to figure the cell potential of any reaction in an electrochemical cell, first derive…

Q: A galvanic cell is constructed that carries out the reaction 2 Ag(s) + Cl, (g) 2 Ag* (aq) + 2 CI…

A:

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: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A  (given) Molar mass of copper = 63.55 g/mol   (given) Cu is having n factor of 2…

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

A: The cell reaction taking place is given as, => 3 Cu2+ (aq) + 2 Al (s) -------> 3 Cu (s) + 2…

Q: a galvanic cell consists of a zinc electrode immersed in 0.1 M ZnSO4 solution and another zinc…

A:

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

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.