Electrolytic Refining

Learn more about Electrolytic Refining at the website RouhNeckChronicles.com.

Q: What are the advantages and disadvantages of smelting compared to electrolytic refining of chalcopyrite?
To be precise, it is pyrometallurgical smelting

A: hmm. i don’t think you should be asking for answers for your chemistry performance task here.

Q: Chemistry help!!! what is the difference between electrolytic refining and electroplating?
Can someone please tell me that what is the difference between using electrolysis for refining metals(Electrolytic refining) and Electroplating?

A: electroplating

Process of coating with metal by means of an electric current. Plating metal may be transferred to conductive surfaces (e.g., metals) or to nonconductive surfaces (e.g., plastics, wood, leather) if a conductive coating has been applied. Usually the current deposits a given amount of metal on the cathode (workpiece) and the anode (source of metal) dissolves to the same extent, maintaining a fairly uniform solution. Silver plating is used on tableware, electrical contacts, and engine bearings. The most extensive use of gold plating is on jewelry and watch cases. Zinc coatings prevent the corrosion of steel articles, and nickel and chromium plate are used on automobiles and household appliances. See also terneplate, Sheffield plate.
electrolytic refining in (chemical engineering)
electrorefining

Petroleum refinery process for light hydrocarbon streams in which an electrostatic field is used to assist in separation of chemical treating agents (acid, caustic, doctor) from the hydrocarbon phase.
(metallurgy)
Purifying metals by electrolysis using an impure metal as anode from which the pure metal is dissolved and subsequently deposited at the cathode. Also known as electrolytic refining.

Q: Is the electrolytic refining of chalcopyrite a spontaneous reaction?
I am just asking for information about what a spontaneous reaction is as well as what a reduction potential is.
Is the electrolytic refining of chalcopyrite melt a spontaneous reaction?

A: Yes, at 945 Degrees Kelvin it is a spontaneous reaction. However it can be achieved at lower temperatures when magnesium chloride is added at 5 parts per million.

Q: Which metal/s is/are contained in anode mud during the electrolytic refining of Cu?

A: Less electropositive metals like Ag,Au,Pt etc.

Q: why copper sulphate is taken as electrolyte for electrolytic refining of copper?

A: So that the anode, cathode and electrolyte only contain one metal, and that is copper.

Q: give me more on refining of through electrolysis?
all about electrolytic refining of copper

A: Metals in general can be refined by electrolyis. The most important is probably aluminum, but copper and lead and precious metals are also refined by this method. Here’s a summary:

http://science.jrank.org/pages/2353/Electrolysis-Refining-copper.html

See this one for a very detailed article on copper refining at high current densities:

http://www.ari.itu.edu.tr/pre_art3/timur.pdf

Q: Electrolytic Cells?
Nickel is deposited at the cathode of a nickel-refining electrolytic cell. If 12.4A are applied for 53.0 min, what mass of nickel is produced?
M= mass
I= current
A= atomic mass
Q= 9.65 X10^4
V= electronics in half reaction
T=time put into seconds
Okay:
M=?
I=12.4a
A= 58.6
Q= 9.65 X10^4
V= 2
T= 53 x 60= 3180 sec

M= ItA/ Qv
= (12.4a) (3180) (58.6) / (9.65 X10^4) (2)
= 2310715.2 / 19300
= 11.97
Is this right if not can you please fix what I did wrong thanks!

A: good

Q: Urgent! aluminium refining process some (whys??) cannt find it on the net, some one who is good at this help?
Topic is
Refining of Aluminium by HOOPE’s Electrolytic method::

q1) why an iron box used
q2) why is it lined with carbon at the bottom (what role does c play)
q3)alloy of impure aluminium with copper is called called Si-alloy(silicon alloy) right or wrong??
q4)why r there carbon rods in contact with the frozen layer of Al what role do they play??
and finally a extremely stupid but really confusing to me is

where does the aluminuim obtained(99% pure,, from electrolysis of alumina )) come into play in this particular HOOPS PROCESS

A: 1) Not always iron, the tank is usually steel. The reasons being because it is strong, it helps to conduct to the graphite (carbon) lining and is relatively inexpensive.

2) Not just the bottom, but often up the sides as well. The graphite acts as the contact for the anode for the reaction.

3) The Al,Cu,Si-alloy is used for the anode.

4) The carbon rod are the Cathodes and contact the frozen impure Aluminum.

The Hoppe’s process is used to make very pure Aluminum (99.99%). This is essential for making Al-Ti alloys for aircraft and spacecraft.

Q: help with electrolysis please.?
can anyone kindly tell me in simple words and clearly what happens in the electrolytic refining if copper……………………………………..please……….. i shall be grateful to all

A: I think this will help you:

http://en.wikipedia.org/wiki/Copper_extraction#Electrorefining

Basically, the copper in the anode is oxidized into copper(II) ions along with other impurities. However, at the cathode copper(II) ions are reduced back to copper while the impurities that are not as reduceable as copper remain in solution or precipite out. So one ends up with a high purity copper at the cathode.

Q: check please!?!?!?
Silver is deposited at the cathode of a silver-refining electrolytic cell. If 25.6 g are produced with a current of 15.5 A, for what length of time was the cell running?
M= mass
I= current
A= atomic mass
Q= 9.65 X10^4
V= electronics in half reaction
T=time put into seconds

M= 25.6
I= 15.5A
T=?
A=107.87
Q=9.65 X10^4
V= 2
T= MQV/ IA
= (25.6) (9.65 X10^4) (2) / (15.5A) (107.87)
= 4940800 / 1671.99)
= 2955.05 –> 49 min

A: for me is OK

Q: what are the answers for following questions?
The Ka for a acid is 6.75 x 103. What is the pH of a 0.15 M aqueous acid solution?
a) 2.49 b) -2.49 c) 4.17 d) 9.22
e) 4.99 f) 2.08 g) 0.82 h) 4.61

A 0.10 M aqueous solution of which of the following compounds will most likely
have a pH greater than 7.0?
a) NaNO3 b) KCl c) NH4Cl d) Ca(C2H3O2)2

5. _____ What is the silver ion concentration for a saturated solution of Ag2CO3 if the Ksp
for Ag2CO3 is 8.4 x 10-12?
a) 2.90 x 10-6 M b) 2.03 x 10-4 M
c) 2.56 x 10-4 M d) 4.06 x 10-6 M
2

6. _____ The solubility of 1:1 salts is measured by the equilibrium constant for the general reaction: MX (s) = Mn+ (aq) + Xn- (aq). Given the following salts and their equilibrium constants for the reaction above at 25oC, which salt is the least soluble?
a) MgCO3, Kc = 6.8 x 10-6 b) CaCO3, Kc = 5.0 x 10-9
c) SrCO3, Kc = 5.6 x 10-10 d) BaCO3, Kc = 2.6 x 10-9

7. _____ A salt bridge is used to
a) provide reactants in a fuel cell
b) determine the direction of the cell reaction
c) control whether the cell is electrolytic or galvanic
d) allow the ion flow necessary for cell neutrality

8. _____ Which one of the following acids has the strongest conjugate base?
9. _____ Which of the following statements is not true?
a) the reverse of a spontaneous reaction is always nonspontaneous.
b) A spontaneous process always moves toward equilibrium
c) A non spontaneous process cannot be caused to occur.
d) A highly spontaneous process need not occur rapidly.

Calculate Ksp for PbI2 at 25oC based on the following data:
Species DGo
f (kJ/mol)
Pb2+ (aq) -24.4
I1- (aq) -51.6
PbI2 (s) -173.6
a) 4 x 10-31 b) 8 x 10-18 c) 9 x 10-9 d) 5 x 10-5

12. _____ For the reaction 2 Al (s) + 3 Co2+ (aq) ® 2 Al3+ (aq) + 3 Co (s), DGo is –799 kJ.
What is Eo for a standard cell based on this reaction?
a) 1.38 V b) 2.76 V c) 4.14 V d) 8.28 V

13. _____ Calculate the standard free energy change, DGo
f, at 25oC for the reaction
2 NO (g) + O2 (g) « 2 NO2 (g)
a) -4.69 kJ b) -70.46 kJ c) -157.82 kJ d) -532.57 kJ

14. _____ The cell reaction for a lead storage battery is:
Pb (s) + PbO2 (s) + 2 H+ (aq) + 2 HSO4
1- (aq) ® 2 PbSO4 (s) + 2 H2O (l)
Eo = + 1.92 V
a) To provide a potential of about 12 V, one could
b) adjust the pH to 12.
c) Adjust the pH to 1.
d) Connect six cells in series.
e) Greatly increase the surface area of the Pb(s) and PbO2 (s)

15. _____ How long must a 50.0 A current be passed through an electrolytic cell for
refining copper to produce 3.00 moles of copper?
a) 1.50 hours b) 1.61 hr c) 2.50 hr d) 3.22 hr

A: looks like someone should do their homework.

Q: Electrolysis exam question. Help?
Here’s the question I’m having trouble with:
Q: In the electro-refining of an ore, the ore is dissolved and the solution placed in an electrolytic cell. A specific ore produces a solution which contains Na+, Cu+2, Pb+2, and Ag+. Which of these metals can be plated out from the solution by electrolysis?
a. all four metals
b. Cu and Pb only
c. Na, Cu and Pb only
d. Cu, Pb and Ag only

The answer is D. Any help understanding this would be appreciated a lot!

A: These three metals are below hydrogen in the activity series. The electrolysis allows these metal ions to be reduced to the metallic form. Sodium ions cannot be reduced in aqueous solution because of the ability of sodium metal to react with water.

========= Follow up ==========

Sodium is indeed a metal, an alkali metal, a very reactive metal.

======== More follow up =======

I noticed that Sunder has changed his tune from sodium not being a metal to parroting my answer.

Is imitation a form of flattery?

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