Balance the three copper reactions: Cu (s) + HNO_3 (aq) rightarrow Cu(NO_3)_2 (a

Question

Balance the three copper reactions: Cu (s) + HNO_3 (aq) rightarrow Cu(NO_3)_2 (aq) + NO_2 (g) + H_2 O (I) Cu (NO_3)_2 (aq) + NaOH(aq) rightarrow Cu(OH)_2 (s) + NaNO_3 (aq) Cu(OH)_2 (s) rightarrow CuO (s) + H_2 O (I) In reaction suppose that you add 12.8 mL of 6 M nitric acid to a sphere of copper metal that weighs 1.06 grams. Which reactant is the limiting reagent? Why should the Cu(OH)_2 precipitate that is formed during reaction be heated slowly during reaction? Why does reaction have to be carried out in the fume hood? Reaction is considered to be combination single displacement precipitation acid-base decomposition

Explanation / Answer

1) The balanced equations are

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

    Left side = 1 Cu, 4H, 4N, 12 O

   Right side = 1 Cu, 4H, 4N, 12 O

Therefore, the reaction is balanced.   

ii) Cu(NO3)2 (aq) + 2NaOH (aq) --------------> Cu(OH)2 (s) + 2NaNO3 (aq)

   Left side = 1 Cu, 2N, 2Na, 2H, 8 O

   Right side = 1 Cu, 2N, 2Na, 2H, 8 O

Therefore, the reaction is balanced.   

iii)   Cu(OH)2 (s) -----------> CuO (s) + H2O (l)

left side = 1 Cu, 2O, 2H

right side = 1 Cu, 2O, 2H

Therefore, the reaction is balanced.

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