Calculate the time required for a constant current of 0.790 A to deposit 0.385 g of Tl(III) as Tl(s) on a cathode. T=____s Calculate the mass of Tl(I) that can be deposited as Tl2O3(s) on an anode at a constant current of 0.790 A over the same amount of time as calculated previously. mass=____g

Q: Consider the following cell: |Zn (s) | Ca2* (aq) , so3²" (aq) || Hg2+ (aq) , F° (aq) | Pt (s) | a)…

A: In a cell notation, the left side represent anode reaction or oxidation-half reaction, and the right…

Q: (o?locator=Dassignment-take A voltaic cell is constructed in which the following cell reaction…

A: The cell reaction is as follows-       Cl2(g) + 2I-(aq) ----> 2Cl-(aq) + I2(s)  At cathode,…

Q: Consider the electrolysis reactions cathode Cu?"(aq, 0.177 M) + 2e-= Cu(s) H,O) =0,(g, 1 bar) + 2H*…

A:

Q: 3. A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

A:

Q: Calculate the time required for a constant current of 0.967 A to deposit 0.388 g of Tl(III) as Tl(s)…

A:

Q: Given the balanced redox reaction equation for a galvanic cell as below. Mg(6) + 2 Ag" (ag) → Mg…

A: We have 0.01 M Ag+ 0.15 M of Mg+2, we have to predict shorthand notation ,cell potential and predict…

Q: Calculate E cell for the following voltaic cell. Ag|Ag *(0.00003 M)||Au 3+(0.93 M)|Au Use standard…

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Q: You have a 5.00 cm diameter sphere that you would like to have plated with copper metal. How long…

A: This answer is given below.Explanation:

Q: How many milligrams of primary cathodic material is produced if aqueous FeCl3 solution is…

A:

Q: 40. In a galvanic cell, the cathode consists of a Ag"(1.00 M)|Ag half-cell. The anode is a platinum…

A:

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

A:

Q: Consider the reaction,    2Ag+ + Cd →   2Ag + Cd2+    The standard electrode potentials for Ag+…

A: Given electrochemical reaction: 2Ag+ + Cd → 2Ag + Cd2+ And, the standard electrode potential as…

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: 1. For the following electrochemical cell at 25°C: Fe(s) Fe (aq) ||H(aq) | Pt, H₂(g) (P=1.00 atm) a.…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: A certa.. .f-reaction has a standard reduction potential E=+1.23 V. An engineer proposes using this…

A:

Q: Consider the following cell: | Zn (s) | Ca²* (aq) , SO3² (aq) || Hg²* (aq) , F` (aq) | Pt (s) | a)…

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

Q: Calculate the time required for a constant current of 0.830 A to deposit 0.312 g of Tl(III) as Tl(s)…

A: Information of question

Q: 21). The electrolysis of a gold nitrate Au(NO3)3 solution to get gold metal is carried out using a…

A: Since the salt Au(NO3)3 has Au3+ ions. Hence the electrolysis reaction taking place is Au3+ (aq) + 3…

Q: An electrochemical cell is set up with the following configuration: Hg|Hg2+||Mn2+|Mn.  The solutions…

A:

Q: A galvanic cell is built by connecting two half cells formed by silver and copper electrodes…

A: Given [AgNO3] = [Ag+(aq] = 1 M [CuSO4] = [Cu2+(aq)] = 1 M  Since Ag+(aq) has higher reduction…

Q: An electrochemical cell is constructed according to the line notationPt | Sn2+ (1.00 M), Sn4+ (1.00…

A: Electrochemistry is the branch of chemistry that studies the change of chemical energy into…

Q: A. H2O2 (aq) + Cl2 (g) B. acidified H2O2+ MnO2 (s) C. NaCl (aq) + acidified H2O2 (aq D. NaCl (ag) +…

A: Correct Answer is (D) where there is no effervescence of gas.  In (A), (B) and (C), all case there…

Q: An aqueous solution of PdCl,2 is electrolyzed for 83.4 seconds and during this time 0.1064 g of Pd…

A:

Q: 2. The net equation for a given voltaic cell is: Sn (s) + 2 Agt → Sn²+ + 2 Ag (s) Write the two…

A: The question is based on the concept of electrochemistry.We need to identify half cell reactions and…

Q: 20. A galvanic cell is constructed at 25°C as indicated in the shorthand cell notation: Determine…

A: In a given question, we have to find out the free energy of Cell , equilibrium constant and cell…

Q: A current of 0.80 A was applied to an electrolytic cell containing molten CdCl2 for 2.5 hours.…

A: Given: Current, i=0.80 A Time, t=2.5 hours Molar mass of cadmium=112.40 One Faraday=96,500 coulombs

Q: A certain half-reaction has a standard reduction potential Ered=-1.02 V. An engineer proposes using…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: . What mass of lead is deposited on the cathode during the electrolysis of lead (II) sulphate…

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

Q: CHEMWORK An aqueous solution of PdCl, is electrolyzed for 90.7 seconds and during this time 0.1064 g…

A: We have given that  Mass of Pd deposited = 0.1064g  time = 90.7sec  F = 96485C/mol  i = current = ?…

Q: Suppose a galvanic cell is established using the following cell reaction, Cu(s) +2Ag*(0.100 M)…

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Q: A galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V…

A: In the given question we have to calculate the gram of CuSO4 dissolve in the 250 mL of solution.

Q: The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?+ (0.20 M) || H* (test…

A: The given cell is, Therefore,

Q: nO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify…

A: Electrochemistry  is branch of chemistry  that deals with chemical changes  produced by electricity…

Q: Electrolysis of water using platinum electrode produces oxygen gas at the anode and hydrogen gas at…

A: Given : Current = 0.2 A Time = 5 mins = 5 X 60 = 300 s…

Q: You have a 2.50 cm diameter sphere that you would like to have plated with platinum metal. How long…

A: Given: Diameter  of sphere = 1.25cm Thickness of coating = 40.0micron density of plating =  21.45…

Q: A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

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.