Consider an electrolytic cell where silver metal is plated (reduced) from an  aqueous silver nitrate solution.  If a constant current of 2.00 A is applied, how long will it take to plate 50.0 g of silver?

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Ans is 0.546g

Q: How many seconds are required to deposit 0.189 grams of manganese metal from a solution that…

A: Hey, since there are multiple questions posted, we will answer first question. If you want any…

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: an acidic solution containing BiO+ is electrolyzed using a current of 0.500 A. what weight of Bi…

A: From Faradays First law of electrolysis,  the amount of the substance deposited(W) at the given…

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: How many amperes of current needs to be passed through molten Sodium chloride to produce 2.4 g of…

A: Faraday's First law,           m α Q          m = eQ               = ect               = E96500ct…

Q: How many seconds are required to deposit 0.224 grams of manganese metal from a solution that…

A:

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Given: Amount of current = 1.03 A Time duration = 28.4 minutes.

Q: The mass of three different metal electrodes, each from a different galvanic cell, were determined…

A: The active electrode which is found to lose mass during redox reaction in a cell is termed as anode…

Q: Suppose a current of 690 mA is passed through an electroplating cell with an aqueous solution of…

A:

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 25 minutes to a 0.50-M…

A:

Q: What flows in the internal circuit of a galvanic cell.

A:

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2+ ions if a current…

A:

Q: A pathway by which counter ions can flow between the half-cells of a galvanic cell without the…

A: Salt bridge consists of U-tube glass rod filled with solution of KCl. It connects oxidation and…

Q: A factory wants to produce 1.00 × 10 kg barium from the electrolysis of molten barium chloride. What…

A: Electrolysis is a chemistry and industrial process that uses direct electric current (DC) to drive 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: How many grams of mercury metal will be deposited from a solution that contains Hg* ions if a…

A:

Q: Calculate the theoretical cell potential of the following cell. If the cell is short-circuited,…

A: The given cell notation is: Ag(s)|Ag+(aq)(0.0575 M) || H+(aq)(0.0333 M)| O2(g)(1.12 atm), Pt The…

Q: Calculate the standard cell potential, ?∘cell, for the equation   Zn(s)+F2(g)⟶Zn2+(aq)+2F−(aq) Use…

A:

Q: An electrochemical cell is constructed in which the silver ions in silver chloride are reduced to…

A: Given,  A current of 0.500 A is passed through the cell for 101 minutes. The mass of copper metal…

Q: How many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a…

A: Mass of cobalt is calculated as:-

Q: If a constant current of 115 A is applied for 15.0 hours to the plating of cobalt from a cobalt(III)…

A:

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

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: Here we use the formula of metal deposited= ZIt , where Z is molecular weight, I= current, t= time…

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: b. Assuming the two half cells operate at standard conditions, calculate the standard reduction…

A: Recall the given half-cell reactions :                        HgO s  +  H2O l  +  2 e-  →  Hg l  +…

Q: many grams of cobalt metal will be deposited from a solution that contains Co2+ ions if a current of…

A: Given:  Current = 0.974 A  Time = 67.4 min = 67.4 x 60 = 4044 sec

Q: A certain half-reaction has a standard reduction potential En=+0.45 V. An engineer proposes using…

A: Given, Ered=0.45 VEcell=1.40 V

Q: How is the cell potential of an electrochemical cell related to the potentials of the half-cells?

A: An electrochemical cell or a galvanic cell is a device that can generate electricity due to the…

Q: Using the Standard Reduction Potential Table, use half-reaction potentials to identify whether the…

A:

Q: How many seconds are required to deposit 0.184 grams of zinc metal from a solution that contains…

A:

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

A: Answer: the standard potential for this cell at 25°C is 1.96 V.

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: In a copper plating experiment in which copper metal is deposited from a copper(II) ion solution,…

A:

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal…

A: For the reaction to occur , or cell will form then standard cell potential for the reaction should…

Q: A voltaic cell undergoes a .......................... cell reaction and has a…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation.  Hence when a…

Q: Determine the cell potential for a galvanic cell composed of copper and zinc at standard condition.…

A: A multiple choice question based on electrochemical cells that is to be accomplished.

Q: How many seconds are required to deposit 0.252 grams of tin metal from a solution that contains Sn2*…

A: Mass of Sn = 0.252 g  Time = ?

Q: If a constant current of 7.3 amperes is passed through a cell containing Cu²+ for 1.5 hours, how…

A:

Q: How many grams of  zinc metal will be deposited from a solution that contains  Zn^2+ ions if a…

A: In this question, we will determine the mass of Zn metal which is deposited from the Solution in…

Q: How many grams of copper will be plated out by a current of 2.3 A applied for 35 minutes to a 0.50 M…

A: ·  change(Q)=current(i)×time(t)· 1F change passed to cu2+ solution to deposite…

Q: How many grams of copper metal will be deposited from a solution that contains Cu2+ ions if a…

A: we know the expression for the faraday's law of electrolysis is => m/E = It / F Where,  m is the…

Q: A factory wants to produce 1.0 x 10³ kg Barium from the electrolysis of molten barium chloride. What…

A:

Q: Why is it necessary to use salt bridge in A galvanic cell?

A: Galvanic cell is the other name for electrochemical cell in which chemical energy is transformed…

Q: A galvanic (voltaic) cell contains a copper cathode immersed in a copper(II) chloride solution and a…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: If a current of 15 A is run through an electrolysis cell for 2.0 hours, how many moles of electrons…

A: First find number coulombs (C) charge  i.e  Q = i x t  Where  Q= charge in coulombs  i = current  in…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal…

A:

Q: A solution containing vanadium (chemical symbol V) in an unknown oxidation state was electrolyzed…

A: Given-> Current (I) = 1.48 ampere  Time (t) = 37.4 min = 37.5 × 60 second = 2250 seconds Weight…

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.