Write redox reactions for the following:
1) C6H12O6, if partially oxidized to C6H10O7
2) C5H7O2N if oxidized to CO2 and NH3
1) C6H12O6, if partially oxidized to C6H10O7
We begin to balance of our equations in the same was as before by balancing the major atoms first. Let us consider Glucose as a substrate
C6H12O6 --------> C6H10O7
Balance the major atoms, such as C and/or N.
C6H12O6 --------> C6H10O7 already balanced
Balance the oxygen with water. (as it is oxidation)
C6H12O6 + O2 --------> C6H10O7 + H2O
No need to balance Hydrogen with H+.
Note that there are no electrons needed to balance the equation. This results because there is no net oxidation or reduction.
2) C5H7O2N if oxidized to CO2 and NH3
C5H7O2N + 5 O2 --------> 5 CO2 + NH3 + 2 H2O
The above equation is written with two half reactions as before, balanced and assuming the end product for nitrogen is ammonia. This assumes that there is no nitrification.
If end product was NH4+, then we needed to add extra H+, as given below.
C5H7O2N + 5 O2 + H+ --------> 5 CO2 + NH4+ + 2 H2O
Write redox reactions for the following: 1) C6H12O6, if partially oxidized to C6H10O7 2) C5H7O2N if...
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