In: Chemistry
Write the balanced half-reaction for the following redox reaction (include physical states like I did in final answer):
2CO2(g) + 12H+(aq) + 6Zn(s) -----> C2H5OH(l) + 3H2O(l) + 6Zn2+(aq)
First, define the “ACIDIC” solution/conditions as H+ presence and
Basic solution implies OH- once it is balanced.
Also; note that ALL species must be balanced, as well as charges
Typical steps:
1) split half redox cells
CO2 = C2H5OH
Zn = Zn+2
2) balance atoms other than O,H
2CO2 = C2H5OH
Zn = Zn+2
3) balance O by adding H2O
2CO2 = C2H5OH + 3H2O
Zn = Zn+2
4) balance H by adding H+
12H+ + 2CO2 = C2H5OH + 3H2O
Zn = Zn+2
5) balance charge by adding e-
12e- + 12H+ + 2CO2 = C2H5OH + 3H2O
Zn = Zn+2 + 2e-
6) balance e- by multiplying by the Greatest common divisor
12e- + 12H+ + 2CO2 = C2H5OH + 3H2O
6Zn = 6Zn+2 + 12e-
7) Add both equations
6Zn + 12e- + 12H+ + 2CO2 = C2H5OH + 3H2O + 6Zn+2 + 12e-
8) simplify repeating elements, H+, H2O, and e- typically
6Zn + 12H+ + 2CO2 = C2H5OH + 3H2O + 6Zn+2
therefore, half reactions are:
12e- + 12H+(aq) + 2CO2(g) = C2H5OH(l) + 3H2O(l)
6Zn(s) = 6Zn+2(aq) + 12e-