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What is the balanced equation for Cu(OH)2(s)?
Cu2 + 2OH --> 2CuOH
How is silver minded?
Cu+H2SO4 Gives CU2(SO4)2+H2O+S2O2
What is the electron configuration of cu plus 1?
The electron configuration of Cu2+ is [Ar]3d94s0.
How can iron be used to get copper from copper sulfate solution?
Since iron (Fe) is more reactive than copper (Cu) it will be 'plated' with copper when the metal iron is stuck in copper sulfate solution. Fe(s) + Cu2+(aq) + [SO42-]aq ---> Fe2+(aq) + Cu(s) + [SO42-]aq
Do magnesium and copper sulphate react?
No. This is a redox question. It is asking whether the reaction will occur spontaneously. In order for Mg+2 to spontaneously oxidize Cu(s), Mg+2 needs to have a higher reduction potential (the tendency to be reduced) than Cu+2. Check a redox table to see: Mg2+ + 2 e− --> Mg(s) E° = −2.372 Cu2+ + 2 e− --> Cu(s) E° = +0.340 (More favorable reaction) Cu2+ has a higher reduction potential, meaning Mg2+ will not oxidize Cu(s).
What cations does Cu form and what are their charges?
Cu2+ is more stable, though Cu+ compounds are known
Calculate the standard emf of a cell that uses the Mg Mg2 plus and Cu Cu2 plus half cell reactions at 25 degrees C?
Cu + Mg2 --------> Cu2 + Mg Cu --------------> Cu2 + 2e Mg2 + 2e --------> Mg Cu --------------> Cu2 + 2e (E = +0.35) Mg2 + 2e --------> Mg (E = -2.36V) +0.35 + (-2.36) = -2.01V --------------------------------------… Mg + Cu2 --------> Mg2 + Cu Mg --------------> Mg2 + 2e Cu2 + 2e --------> Cu Mg --------------> Mg2 + 2e (E = +2.36V) Cu2 + 2e --------> Mg (E = -0.35V) +2.36 + (-0.35) = +2.01V
Why do Cr and Cu doesn't contain a a full 4s orbital?
In the case of chromium (Cr), the electron configuration of 3d54s1 is more stable than 3d44s2. A half-filled sublevel is more stable than a sublevel that is less than half full. In the case of copper (Cu), the electron configuration of 3d104s1 is more stable than 3d94s2, again because a full sublevel and a half-filled sublevel is more stable.
What metals would copper nitrate react with?
Copper Nitrate -> has Cu2+ and NO3- NO3- won't touch other metals but Cu2+ will be displaced from solution, by ANY metal more reactive than copper. However, the speed of the reaction depends on many other factors. (Check the reactivity series on the internet) E.g. Na: 2 Na + Cu2+ => 2 Na+ + Cu (oxidation-reduction reaction, Cu as the oxidising agent) Examples of metals more reactive than copper (but might not react with Cu(NO3)2 immediately) are: Na, K, Fe, Zn, Al... and many many more
Will paper clip react to Copper Sulfate?
When your paper clip is made of (or coated with) more reactive metals than copper, like Fe, Zn or Sn, it might react with Cu2+ ions in your solution. Cu2+ + Fe(s) --> Cu(s) + Fe2+
What is the balance equation of cupric ion?
Cu-------Cu2+ + 2 e-
What molecule What is the name for Cu2?
The name of Cu^2+ or (Cu2+) is called: "The name of Cu2+ is _________ ion or ________ ion" 1st blank is: copper(II) 2nd blank is: cupric It is correct. i am a teacher.
What is the balanced equation for Cu(OH)2(s)?
Cu2 + 2OH --> 2CuOH
In the equation Cu+ Fe2+ > Cu2+ Fe what has been oxidized?
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How is silver minded?
Cu+H2SO4 Gives CU2(SO4)2+H2O+S2O2
How Leaching carried out in low grade copper ores?
Copper is leached out using acid or bacteria. The solution containing Cu2+ ions is treated with scrap or H2 to recover copper. Cu2+(aq) + Fe(s) ---------> Cu(s) + Fe2+(aq) Cu2+(aq) + H2(g) ---------> Cu(s) + 2H+(aq)
What is the net ionic equation of the reaction between zinc and copper 2 sulfate?
Zn + CuSO4 -> ZnSO4 + Cu (molecular equation) Zn (s) + SO4 2+ + Cu 2+ --> Cu (s) + Zn 2+ + SO4 2+ (ionic equation) Cu + Zn(s) ---> Cu (s) + Zn (net ionic)
