Write a balanced equation for the reactions listed below. Click Work Problem and

Question

Write a balanced equation for the reactions listed below. Click Work Problem and carefully read the directions on how to enter the coefficients, formulas, charges and states of matter. In some cases, this information is provided. Note that molecular compounds (i.e. H2O) have a charge of zero.

1.) CoCl2•6H2O (aq) + Ethanol (EtOH) (l)

2.) CoCl2•4H2O (aq) + Water (l)

3.) Copper + conc. Nitric Acid

4.) Copper sulfate (aq) + Sodium hydrogen carbonate (aq)

5.) Copper sulfate (aq) + Ammonia (aq)

6.) Copper Hydroxide (aq) + Ammonia (aq

7.) Magnesium + Copper sulfate (aq)

8.) Magnesium + Hydrochloric acid

9.) Calcium carbonate (s) + Hydrochloric acid

2.) CoCl2•4H2O (aq) + Water (l)

3.) Copper + conc. Nitric Acid

4.) Copper sulfate (aq) + Sodium hydrogen carbonate (aq)

5.) Copper sulfate (aq) + Ammonia (aq)

6.) Copper Hydroxide (aq) + Ammonia (aq

7.) Magnesium + Copper sulfate (aq)

8.) Magnesium + Hydrochloric acid

9.) Calcium carbonate (s) + Hydrochloric acid

Explanation / Answer

1.  when CoCl2*6 H2O dissoves in water it makes the pink ion [Co(H2O)6]+2 it the presence a excess alcohol it converts into the blue ion [Co(Cl-)4]-2 . Ethanol is not a part of that reaction, it rather removes available water from the reaction & according to LeCatlier, removing water will shift the equilibriumto the right in an attempt to restor the water which alcohol took out,... producing the blue [Co(Cl-)4]-2

[Co(H2O)6]2+(Aq) + 4Cl-(aq) + EtOH(l) <=> [CoCl4]2- + 6H20(l) + EtOH(l)

3. Copper is oxidized by concentrated nitric acid, HNO3 and produces Cu2+ ions; the nitric acid is reduced to nitrogen dioxide it is a poisonous brown gas with an irritating odor.

Cu(s) + 4HNO3(aq) ——> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)

4. CuSO4(aq) + 2NaHCO3(aq) ---> Na2SO4(aq) + Cu(OH)2(s) + 2CO2(g)

Copper(II) sulfate, CuSO4, and sodium carbonate, Na2CO3 react with each each other to produce copper(II) carbonate, CuCO3, its an insoluble solid that precipitates out of solution, and aqueous sodium sulfate, Na2SO4.

5. When an Ammonium solution or NH4OH is added to Copper Sulfate (CUSO4) it forms Tetraamminecopper(II) complex. The color of the soultion is deep blue and may form a white precipitate

NH3(l) + CuSO4(s) + nH2O [Cu(NH3)4(H2O)n]2+(Aq) + SO42-(Aq)

6. Copper (II) hydroxied reacts with ammonia to form tetraamminecopper (II) ion.

Cu(OH)2(s) + 4NH3(aq) [Cu(NH3)4]2+(aq) + 2OH(aq)

7. magnesium is more reactive than copper, thus it loses it electrons easily. Magnesium displaces copper in the solution, thus copper metal is formed as a precipitate.

Mg(s) + CuSO4(aq) --> MgSO4(aq) + Cu(s)

8. A reaction between a metal and an acid gives the salt of the metal and hydrogen gas.

2Mg(s) + 2HCl(aq) ---> 2MgCl(aq) + H2(g)

9. 2 HCl + CaCO3 --> CaCl2 + H2O + CO2

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