Jennifer wish to electroplate a sculpture using platinum. She placed electrode and sculpture in a solution containing [PtCl6]2-  An average current of 12A was applied throughout experiment. Calculate the time (in hours) that she required to electroplate of 80 g of platinum (195.08 g/mol). Note that experiment was conducted with 90% electrode efficiency.

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A:

Q: Purification of copper can be achieved by electrorefining copper from an impure copper anode onto a…

A: Current passed = 40 amp Mass of Copper to be deposited = 18.5 g Number of moles of Cu deposited =…

Q: two grams of copper (A.W. = 63.54g g/mol, density = 8.93g/cm^3) dissolves in 500g of water to…

A: Reaction: Cu→Cu2+ + 2e- Using Nernst equation: ECell=Ecell∘-0.05912logCu2+

Q: How many minutes will it take to plate out 40 g of Ni from a solution of NISO4 using a current of…

A:

Q: Please with complete solution and good penmanship

A: Dear student, this question is related to electrolytic cell.

Q: How many hours does it take to form 15.0 L of O, measured at 750 torr and 30°C from water by passing…

A:

Q: In one process used for electroplating metal RRr, a current of 13 A was passed through an…

A:

Q: Chromium can be electroplated from aqueous potassium dich with the reduction shown belovr 14 12e…

A: Q = charge = 165136coulombs I = current = 5.5amperes V = voltage = 7.3volts 1kwh = 1kw x 1hr

Q: The following are the advantages of the dropping mercury electrode except...     It has a wide…

A: Dropping mercury electrode is made from mercury. It is used in polarography.

Q: This is electrochemistry. Use the Nernst equation to find log Cu^2+ of each voltage.

A: When [Cu2+] = 0.050 M ,log [Cu2+] = -1.30 When [Cu2+] = 0.125 M , log [Cu2+] = -0.90 When [Cu2+]=…

Q: What current must be used to plate 1.75 moles of copper on an electrode in 6.25 minutes?

A: ∙Given:-  no. of moles of copper =1.75 moles                     Time =6.25  minutes or  375s

Q: а. Write the balanced electrochemical reaction. Use the reduction potentials to determine E°: i.…

A: An electrolytic cell is a cell which requires an outside electrical source to initiate the redox…

Q: A. If the measured cell potential is 1.800V, what is the concentration of Au3+? B. How long will it…

A: Here we have to determine the concentration of Au+3 of the galvanic cell and mass of gold…

Q: Stacy has class is from 10:30 am-1:20 pm, in which she performed an electrolysis experiment with…

A: This can be proved according to the Faraday's first law of electrolysis. It states that, Mass of the…

Q: How much time (in hours) is required to plate out 25.0 g of gold metal from a solution of Au(NO3)3…

A:

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.3 ampere current. What…

A: We have following reaction Ni2+ +2e ---> Ni(s) moles of electrons required to form 1 mole Ni(s)=2…

Q: How long will it take to plate out 4.9 g Ni from aqueous Ni2+ with a current of 113.1 A?

A:

Q: Purification of nickel can be achieved by electrorefining nickel from an impure nickel anode onto a…

A: This is a problem of electrochemistry.It is basically a study of the chemical processes that cause…

Q: How long will it take to plate out 3.0 g Ni from aqueous Ni2+ with a current of 113.1 A? HOW DO WE…

A: Given:: Mass of Ni=3.0 g  molar mass of Ni = 58.6934 g mol-1 Current i=113.1 A Time, t = ?

Q: A sample of 25 mL prepared for an electrolysis experiment has a zinc concentration of approximately…

A:

Q: Calculate the time required for a constant current of 0.9170.917 A to deposit 0.3190.319 g of…

A:

Q: A concentration cell similar to the one shown is composed of two Ni electrodes and solutions of…

A: In concentration cell same electrode and same substance is used in solution.The only difference is…

Q: How many seconds would be required to produce 50.0 g of Mg from MgCl2 if the current is 100.0 A?

A: According to Faraday's law of electrolysis, the weight of the substance deposited on any electrode…

Q: In a certain electrolysis experiment involving Al" ions, 50.4 g of Al is recovered when a current of…

A: Given data : In a certain electrolysis experiment involves Al3+ ions  50.4 g of Al is recovered by…

Q: Write the reaction taking place on the electroplating cell of nickel and graphite electrodes

A:

Q: Calculate the time required to precipitate 200 milligrams of copper by electrolysis of an acidic…

A: By 1F of charge 1 equivalent of metal can be deposited .

Q: The initial potential you measure is 219.3 mV and the temperature of the solution is 23.8 Celsius.…

A:

Q: chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below: how…

A:

Q: Calculate the time required for a constant current of 0.7520.752 A to deposit 0.2920.292 g of…

A:

Q: Calculate the electromotive force of a platinum electrode immersed in a solution containing tin ions…

A: Given,  Reduction of Sn2+ ion is : Sn2+ (aq) + 2e- -----------> Sn (s) , E0Sn2+/Sn = +0.15 V…

Q: Calculate the time required for a constant current of 0.790 A to deposit 0.385 g of Tl(III) as Tl(s)…

A: Given: Current (i) = 0.790 A Mass of Tl = 0.385 g Molar mass of Tl = 204.38 g/mol

Q: A copper rod was purified using an electrolysis method consisting of a 1.0 M solution of copper (II)…

A: The correct answer is given below ?

Q: applied potential difference of 0.275 V

A:

Q: 5. Iron and Cadmium are coupled together in a poorly designed component. (a) What is the likely…

A: Given: Iron and cadmium couple.

Q: In an electrolysis of copper sulphate between copper electrodes the total mass of copper deposited…

A: The solution is given below -

Q: 5. Iron and Cadmium are coupled together in a poorly designed component. (a) What is the likely…

A: Interpretation: We have to provide likely reaction in the given aqueous environment.

Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: For ferricyanide determination by voltammetry, 20 mL of non-electroactive KCl solution is added to…

A: Molarity = No of moles / Volume (L) Also, No of moles = Molarity * Volume (L)

Q: 4. A copper rod was purified by using it as the anode in the electrolysis of a 1.0 M copper (II)…

A: Anode is the electrode on which oxidation takes place and Cathode is the electrode where reduction…

Q: How long would it take to produce 3.6 g of platinum by passing a 2.0 ampere current through a…

A: The mass of the substance (m) deposited or liberated at any electrode is directly proportional to…

Q: How long would it take to electrodeposit all the Cu2+ in 0.200 L of 0.210 M CuSO4 solution with an…

A:

Q: Given the following electrode reactions: 2+ Co +e Co“ E'=1,92 V 3+ Co(NH,) , +e Co(NH,), E-0,06 a.…

A:

Q: How long will it take to deposit 0.0047 mol of gold by electrolysis of KAuCl4 using a constant…

A:

Q: A small part with a surface area of 3.0 cm2 is plated with a gold coating that is 5.00x10-4 mm…

A: In gold plating, the chemical reaction occurs due to the passage of electric current in an ionic…

Q: 7) How long would it take to electrodeposit all the Cu2+ in 0.250 L of 0.210 M CuSO4 solution with…

A: The number of moles of Cu+ ions is calculated as,

Q: 2 In an electrolysis of copper sulphate between copper electrodes the total mass of copper deposited…

A:

Q: How long does it take to deposit a coating of gold 1.00 µm thick on a disk-shaped medallion 4.00 cm…

A:

Q: Using data table 4, assign the identities of each of the metals (A-D). Using the identity of Metal…

A: From the given table 4 We can infer that copper is the metal with positive standard reduction…

Q: What mass of platinum can be played onto an electrode dipped in Pt(NO3)2 solution if a 2.5 current…

A: The reaction taking place will be  Pt2+  + 2 e- ----> Pt  This is because we have Pt2+ in…