Question

6. For the following redox reaction: Cu(s) + HNO3(aq) + Cu(aa) + NO) a) Assign oxidation states to each of the elements in the reaction. b) Tell what is being oxidized, what is being reduced, what is the oxidizing agent and what is the reducing agent. c) Use the half-reaction method to balance the reaction as if it were taking place in acidic solution. d) Then balance the reaction as if it were taking place in basic solution. You do not have to re-show any steps you already did in part c.

Answer 1

a, oxidation states :

Cu-0

HNO_{3 :} H-⁺1, N-⁺5, O-^-2

Cu²⁺-⁺2

NO: N-⁺2, O-^-2

b, Cu gets oxidesed

Nitrogen gets reduced.

copper is the reducing agent

nitrogen is the oxidising agent

c, in acidic solution

2+ - Step 1: Cu + HNO3 ~ Cu + Step 2 Assign oxidation number. number of split into. sedot couple and split into two half reaction 2 + cue cu + zë. -> MO? +5 -2 R. HNO3 + 3 é Step 3. Balancing the akoms, charge. I then oxygent. > + 20 +3ě +34 + cu 2+ Cw + 2H+. +1 +5 -2 +2 No R. HNO3 + 2 H2O.

Step Make electoon gain equivalent to electron last. je, o x3 RXZ. O: 3cu. +2 3 Cir. +6 +64t. +1 +5 -2 R! 2 HNO3 toé +64t 20² + 4H20 Step 5 . Add Half Reactions togethes. + +5 -2 3 cu + 8.2 HNO₃ + bê +6h 3 ou + 2 No bé 4H2O + 6H² Step 6: simplity +1 +5 -2 2+. 3 cu 2 HNO₃ 3 cu 27 + 2 + 4H2O

d, in basic solution:

Basic Medium. Step 1 : Same. Step 2 same. Step 3: cu + 204 - Cu2+ + Zé + 2 H₂O. HNO₃ +30 + H₂O No + 304 Ox 3 Rx2. +2 Step 4. 3 cu + gou -> 3 cu + 6é + 6H2o. R: 2HNO₃ + 60 + 2H20 - 2 NO + Gori Step 5 3 cu + 2HNO₃ +60 +604 + 2H₂0 3ch² +2 Not 60+ 6ou + 6+4o. Step 6. 2+ 3 cu + 2HNO₃ 3 cud+ 2 NO + 4H2O.

note: please do like the asnwer