a copper mental strip is place in a soluation of silver nitrate. write?
821643
Copper is more reactive than silver, hence displacement of silver occurs.\nCu (s) + 2AgNO3 (aq) --> 2Ag (s) + Cu(NO3)2 (aq)\n\nSum of the coefficients? 6...\n\nHope this helps :)
117425
Silver nitrate. \nThe Ag(+) is silver, and the NO3(-) is nitrate. \nDon't get this stuff on your hands; it stains!
307574
No, it's Ag2S. The 2 is a subscript, denoting 2 Silver atoms to 1 Sulphur atom. Silver has a valency of 1+, while Sulpur has a valency of 2-, hence 2 Silver atoms are needed to balance with 1 Sulphur atom to form a compound. Besides, the equation would make sense then. 2 Silver atoms and 1 Sulphur atom on both sides of the equation, the equation is now balanced. 10 marks please, thank you!
606075
Cu(s) + 4HNO3 (aq)--> Cu(NO3)2(aq) + 2H2O(l) +2NO2(g)
1002183
Concentrated Nitric Acid and copper.  Be careful.  Nasty stuff... really!
316653
Depends on the application you have for the copper. You can shield it from oxygen and other corrosive agents using a protective atmosphere.\n\nAt 500°C exposed to atmospheric oxygen you will want a solid metal with a stable passivizing surface or too noble to react. Titanium or platinum will probably be overkill, stainless steel may discolour.\n\nOr you might be thinking about a sacrificial anode, leaving the copper intact but dissolving the connected material (e.g. zinc or magnesium).
787695
The nitrate ion is a good oxidizer, meaning it is reduced and the other species it reacts with is oxidized. The flame test is color dependent on the oxidation state (or number of electrons) present in the metal you are analyzing. So I would imagine that if you were analyzing something like the copper (I) cation in the flame, the color would change due to the fact that the nitrate ion is causing another oxidized copper species to be produced, such as copper (II), which has a blue color. Hope this helps and let me know if you have any other questions!
837660
Silver is one of the most reflective elements.  It will reflect the heat back into the vessel instead of allowing it to escape.
241514
to remove a desired metal from a solution. IE gold, silver, copper.
437503
Q = m.s.ΔT\nHeat loss by the copper = heat gained by the metal.\nCopper (heat loss) = 200.0g x 0.38J/g.ºC x (195.5ºC-228.4ºC) = -2500.4J\ndivide the heat by the mass and ΔT of the metal to get the specific heat of the metal:\n2500.4J/(65.0g x (195.5ºC-18.3ºC)) = 0.2171 = 0.21 J/g.ºC (correct SF)
888667
Cu2S + 12HNO3 -> Cu(NO3)2 + CuSO4 + 10NO2 + 6H2O\n\nThere you go.
731827
Firstly, and most importantly, the word 'cuprum' isn't a word, at least not in latin or english, as far as I know, and I study latin. The word for copper in latin is '(h)enus'\n\nSecondly, you need to at least act sure about what you're saying. Write with conviction, even if you don't have any. Don't say "never really discovered", either it was or it wasn't. \n\nThirdly, you need punctuation. After "certain point in time" add a comma. You also need a comma after pipes in the phrase "guns, pipes, and even blue fireworks." Plus, fireworks is one word. You need to turn this from one paragraph into at least two different ones. \n\nRephrase the whole section with the two sentences "in the bloodstream. But large amounts" etc. That can be turned into better sentences, or one sentence. \n\nIn the sentence "But large amounts" after 'but' add an 'in' and get rid of the comma after amounts. Also, you should change deathly to deadly, or something else. The sentence should look like this:\n\n"But in large amounts copper can be poisonous or even deadly to organisims."\n\nor:\n\n"But, in large amounts, copper can be poisonous or even deadly to organisms."\n\nYou might also want to add an adjective describing the organisms. \n\n\nWith the next sentence, add 'the' between 'in' and 'water'. \n\n\nRephrase the last setence too- it doesn't really make sense,\nPossibilities:\n\n"The effect of too much copper is damage to gills, liver, kidneys, and the nervous systems of fish and other animals."\n\nIt's too long. you should probably change it into two sentences. \n\n"This has many bad effects on land animals and fish. Some things that could happen are damage to the gills, liver, kidneys, and the nervous system." \n\n\n\nI hope I helped.
913031
Standard electrode potential for Ag(NH3)2 = 0.37V
723937
copper. because it can oxidize easier. That is why statue of liberty is green.
418443
Copper can react with nitric acid on two different ways based on the concentration of nitric acid.\n\nIf cold and dilute nitric acid is used, then the reaction yields copper(II) nitrate, nitrous oxide(N2O) and water.\n\nCu + HNO3 ----- Cu(NO3)2 + N2O + H2O\n\nIf hot and conc. nitric acid(a stronger oxidising agent) is used, the reaction yields copper(II) nitrate, nitrogen dioxide(NO2) and water.\n\nCu + HNO3 ----- Cu(NO3)2 + NO2 + H2O\n\nP.S. - Balance the equations yourself(might take some time but use the oxidation no. method)
221298
2.5% copper, 97.5% zinc
1094858
Chemistry Comes Alive!\n    Electrochemical Series: Metal Trees\n\n    A piece of metal (Cu, Zn, Ag, Cd, or Pb) is placed in an aqueous solution of a metal ion (Cu2+, Zn2+, Ag+, Cd2+, or Pb2+). In some cases the growth of metal crystals indicates that a chemical reaction has occurred. This set of experiments may be used to rank the metal ions in order of reduction potential.\n\n    (86 )\n    Keywords\n\n    copper, crystals/crystallization, descriptive chemistry, electrode potentials, metals, redox reaction, single exchange/replacement reaction, zinc\n    Multimedia\n\n    The five metals\n    Metals in Silver Nitrate Solution, same time\n    Play movie (QuickTime 3.0 Sorenson, duration 15 seconds, size 1.1 MB)\n\n    Five different metals have been placed in silver nitrate solutions. Note the formation of silver metallic crystals on the metals' surfaces and the eventual darkening of the crystals.\n\n    \n    \n\n    Copper metal \n    Zinc metal \n    Silver metal\n\n    Cadmium metal \n    Lead metal\n\n    Additional still images for this movie\n\n    All Five Metals in all five Solutions\n\n    \n\n    \n\n    Silver Nitrate Solution\n    \n\n    Copper(II) Nitrate Solution\n    \n\n    Zinc(II) Nitrate Solution\n    \n\n    Cadmium Nitrate Solution\n    \n\n    Lead(II) Nitrate Solution\n\n    \n\n    \n\n    (Ag+ ion)\n    \n\n    (Cu2+ ion)\n    \n\n    (Zn2+ ion)\n    \n\n    (Cd2+ ion)\n    \n\n    (Pb2+ ion)\n\n    Copper\n    Metal\n    (Cu)\n    \n\n    \n\n    Copper Metal in Silver Nitrate Solution\n    \n\n    Copper Metal in Copper(II) Nitrate Solution\n    \n\n    Copper Metal in Zinc(II) Nitrate Solution\n    \n\n    Copper Metal in Cadmium Nitrate Solution\n    \n\n    Copper Metal in Lead(II) Nitrate Solution\n\n    Zinc\n    Metal\n    (Zn)\n    \n\n    \n\n    Zinc Metal in Silver Nitrate Solution\n    \n\n    Zinc Metal in Copper(II) Nitrate Solution\n    \n\n    Zinc Metal in Zinc(II) Nitrate Solution\n    \n\n    Zinc Metal in Cadmium Nitrate Solution\n    \n\n    Zinc Metal in Lead(II) Nitrate Solution\n\n    Silver\n    Metal\n    (Ag)\n    \n\n    \n\n    Silver Metal in Silver Nitrate Solution\n    \n\n    Silver Metal in Copper(II) Nitrate Solution\n    \n\n    Silver Metal in Zinc(II) Nitrate Solution\n    \n\n    Silver Metal in Cadmium Nitrate Solution\n    \n\n    Silver Metal in Lead(II) Nitrate Solution\n\n    Cadmium\n    Metal\n    (Cd)\n    \n\n    \n\n    Cadmium Metal in Silver Nitrate Solution\n    \n\n    Cadmium Metal in Copper(II) Nitrate Solution\n    \n\n    Cadmium Metal in Zinc(II) Nitrate Solution\n    \n\n    Cadmium Metal in Cadmium Nitrate Solution\n    \n\n    Cadmium Metal in Lead(II) Nitrate Solution\n\n    Lead\n    Metal\n    (Pb)\n    \n\n    \n\n    Lead Metal in Silver Nitrate Solution\n\n    \n\n    Lead Metal in Copper(II) Nitrate Solution\n    \n\n    Lead Metal in Zinc(II) Nitrate Solution\n    \n\n    Lead Metal in Cadmium Nitrate Solution\n    \n\n    Lead Metal in Lead(II) Nitrate Solution\n    Discussion\n\n    Each of the videos in this section shows the reaction (or absence of reaction) when a sample of a metal is placed into a solution containing a metal ion. By viewing the videos students can determine which metal ion is the strongest oxidizing agent and which metal is the strongest reducing agent. The videos could be used in homework or quiz questions that ask students to rank the metals in order of reducing strength or to rank the metal ions in order of oxidizing strength.\n\n    The reactions that occur are\n\n    2 Ag+(aq ) + Cu(s ) --> 2 Ag(s ) + Cu2+(aq )\n    2 Ag+(aq ) + Zn(s ) --> 2 Ag(s ) + Zn2+(aq )\n    2 Ag+(aq ) + Cd(s ) --> 2 Ag(s ) + Cd2+(aq )\n    2 Ag+(aq ) + Pb(s ) --> 2 Ag(s ) + Pb2+(aq )\n    Cu2+(aq ) + Zn(s ) --> Cu(s ) + Zn2+(aq )\n    Cu2+(aq ) + Cd(s ) --> Cu(s ) + Cd2+(aq )\n    Cu2+(aq ) + Pb(s ) --> Cu(s ) + Pb2+(aq )\n    Cd2+(aq ) + Zn(s ) --> Cd(s ) + Zn2+(aq )\n    Pb2+(aq ) + Zn(s ) --> Pb