does anyone know how copper is extracted plz ancwer this question anyone that knows the ancwer thank you all?
913610
Copper ore is extracted from the Earth usually in rocks dug from strip mines. Kennecot copper in Utah has this humongous open pit near the Great Salt Lake that looks like a mountain dug into the Land. The ore rock is crushed and then run through a blast furnace (Smelter) at extremely high heat (Thousands of degrees fereinheit) which melts out the different metals in the rock including the copper. Then each metal is extracted from that mix and we have pure copper.
867590
Well, for a start your equation shows copper(II) sulphide, not sulphate, and your equation is wrong even then.  That makes a bit of a difference!\n\nLet us imagine that you've got the formula right, but the name wrong.\n\nThe equation is simply Cu + S ---> CuS\n\nThen 64g will give (64+32)g.\n\nThus 64g will give 96g.\n\nSo 64 x (200/96)g of Cu will give 200g of product.
759753
I just saw the question and I realize you've run out of time.  I'll answer it for you anyway for "enrichment" purposes.\n\nThe equation is 2HCl + CuO --> CuCl2 + H20\n\nBasically you need two moles of HCl for every mole of CuO.  So let's find out how many moles of CuO we have first.  \n\nWe know that CuO has a molar mass of 63.546+16 = 79.546 grams/mol\n\n(.402 grams CuO) x (1 mol / 79.546 grams CuO) = .00505 mol CuO\n\nThat means we need (.00505)(2) = .0101 mol of HCl\n\nWe know that the HCl is 6 mol/L.  If we need .0101 mol, we do the following calculation:\n\n(.0101mol) x (1L / 6 mol) = .0017 L\n\nWe need .0017 L or 1.7 mL of HCl to dissolve .402g of CuO.\n\nHave fun!
545055
To answer that question, another must be posed.....\n\nHow thin can you make copper wire?\n\nThe answer is yes, you can insulate copper wire with hemp plastic, as thin as a biodegradable plastic grocery bag\n\nHemp plastic is a cellulose based plastic.\nOnce you introduce it to the soil it will deteriorate, and once again become part of the earth. Hence Biodegradable
1086041
all the information you need is in the handy periodic table.   First, think about the charges of the molecules....\n\n In the molecule CuSO4, copper has two electrons to give.  The SO4 molecule wants TWO more electrons to acheive noble gas configuration (a stable electron state).   This appears to be a match in heaven.  \n\nWell all is fine until Zinc comes along.  If you look at the periodic table, Zinc is just to the right of copper.  It too has 2 electrons to donate......but, it is more electronegative than copper. (remember, electronegativity  is the lowest in the bottom left corner of the table(Fr) and increases on  a diagonal path  with F being the most electronegarive.)  \n\nSince Zinc is more reactive than Copper,  a replacement reaction occurs.  Zinc bumps Copper off of the SO4 molucule.  Zinc can be whitiish to yellowish in solution.  As all the Zinc is coming off the rod, it bumps the copper off the SO4 and also disperses the colour of the copper.  If you had one drop of blue dye (the copper), but added a cup of milk. ( the Zinc)...... you would barely see the blue color.
929154
copper can't produce electricity. it conducts electricity
513117
use a potato and two different metals as electrodes. The link will help you, do your own homework, or web searching atleast! it was the second link in google for g** sake!
831330
After looking it up on the internet, it looks like a scam.  Try looking up Iridium Copper and see for yourself.
887687
Below is a link to a practical for finding the % copper in pennies.  The same method will work using brass in place of pennies.\n\nhttp://www.creative-chemistry.org.uk/alevel/module5/documents/N-ch5-17.pdf
961700
...\n_The_ First experiment was to observe the reaction when AgNO3 was added to the copper metal. The copper metal was placed in a test tube, (<--no comma needed here) and 0.1 M AgNO3 was added. Just after AgNO3 was added, the (<-- delete the) shiny silver things were observed. Finally, the copper metal was completely changed to shiny silver powder. In the chemical equation, (change to "only the color of")  (the color of only) Ag was shiny silver. Therefore the color of the product matched the color of Ag, and must have been powdered silver. In this experiment, because copper replaced silver in the compound, this was a single replacement reaction.
951188
4. How many grams of zinc chloride can be formed from the reaction of 7.96 grams of zinc with excess HCL?\n\nZn + 2HCl → ZnCl2 + H2\n\n1 mole Zn produces 1 mole ZnCl2\nTherefore 65.7g Zn produces (65.7 + 2 x 35.5)g ZnCl2\nie ~65.7g Zn produces ~136.7g ZnCl2\nSo 7.96g Zn produces ~7. 96 x 136.7/65.7g ZnCl2\nie ~ 16.6g ZnCl2\n\n5. How many kilograms of copper sulfide could be formed from the reaction of 1.80 mol of copper with excess sulfur.\n\nCu + S → CuS\n\nSop 1 mole Cu produces 1 mole CuS\nTherefore 1.8 mole Cu produces 1.8 mole CuS\n1 mol CuS weighs ~(63.5 + 32.1)g = 95.6g\nSo 1.8 mol CuS weighs ~ 1.8 x 95.6g ≈ 172.1g = 0.1721kg\n\n6. If Copper(one) sulfide is partially roasted in air (reaction with 02), copper(one) sulfite is formed. Subsequently upon heating, the copper sulfite thermally decomposes to copper (one) oxide and sulfur dioxide. Write balanced chemical equations for these 2 reactions\n\nCu2S + 3O2 → Cu2SO3\nCu2SO3 → Cu2O + SO2
56086
Depending upon your application, copper probably does not make a good coil core.  If you wrap many turns of wire around a steel nail and pass a current through the wire (say from a battery) the nail will concentrate the magnetic field and you will have an electromagnet in which the tiny magnets within the steel are all aligned.  This will not happen with copper because you can not pick up copper with a magnet.  The coil will still produce a magnetic field but the copper core will not concentrate it.
930459
Pure copper has a certain crystal structure as does pure tin.  Bronze will have a different crystal structure, the exact form of which will depend on the ratio of copper and tin.  (I am treating this as a general scenario, there is a chance that the crystal structure of copper and tin takes the same form - but this would be coincidental; and by chance/coincidence I don't mean theory doesn't define them - i just don't know crystal theory all that well)
378767
You would complete dissolve it in strong acids and then separate the metals by qualitative analysis techniques.  Not simple and very expensive.
1154066
It is not due to the chemistry of copper or gold.\n\nIt is due to the electronic band structure. The two metals unusually have a band structure that causes them to absorb light at certain frequencies rather than reflecting it.
847907
copper most easily interact with oxygen than the other metals\ncoins are made of
975863
Connection? or disconnection...\n\nSemiconductors are not metals - nor do they intend to be.