Question

4. Nitrogen is unusual in that it can be many forms in the environment, with oxidation states -III, III and V common in water and N2 or N(0) relatively unreactive with its triple bond. To remove nitrogen pollution (as a nutrient), ammonium (N(-III)) is oxidized to nitrite (N(III)) and then further oxidized to nitrate (N(V)) in a process called nitrification, which is then reduced to N2 in a process called denitrification. Write balanced redox reactions for the following steps (where you are given both the oxidant and the reductant). a) $NH_4^+$ + $O_2$ = $NO_2^-$ b) $NO_2^-$ + $O_2$ = $NO_3^-$ c) $NO_3^-$ + $C_6H_{12}O_6$ = $N_2$ 5. If you started with 100 mg $NH_4^+$/L, a) how many mg $NO_3^-$/L will be formed? b) How many mg $C_6H_{12}O_6$/L will be required turn that nitrate into nitrogen gas?

          4. Nitrogen is unusual in that it can be many forms in the environment, with oxidation states
-III, III and V common in water and N2 or N(0) relatively unreactive with its triple bond. To
remove nitrogen pollution (as a nutrient), ammonium (N(-III)) is oxidized to nitrite (N(III))
and then further oxidized to nitrate (N(V)) in a process called nitrification, which is then
reduced to N2 in a process called denitrification. Write balanced redox reactions for the
following steps (where you are given both the oxidant and the reductant).
a) $NH_4^+$ + $O_2$ = $NO_2^-$ 
b) $NO_2^-$ + $O_2$ = $NO_3^-$ 
c) $NO_3^-$ + $C_6H_{12}O_6$ = $N_2$
5. If you started with 100 mg $NH_4^+$/L,
a) how many mg $NO_3^-$/L will be formed?
b) How many mg $C_6H_{12}O_6$/L will be required turn that nitrate into nitrogen gas?

4. Nitrogen is unusual in that it can be many forms in the environment, with oxidation states
-III, III and V common in water and N2 or N(0) relatively unreactive with its triple bond. To
remove nitrogen pollution (as a nutrient), ammonium (N(-III)) is oxidized to nitrite (N(III))
and then further oxidized to nitrate (N(V)) in a process called nitrification, which is then
reduced to N2 in a process called denitrification. Write balanced redox reactions for the
following steps (where you are given both the oxidant and the reductant).
a) NH4^+ + O2 = NO2^-
b) NO2^- + O2 = NO3^-
c) NO3^- + C6H12O6 = N2
5. If you started with 100 mg NH4^+/L,
a) how many mg NO3^-/L will be formed?
b) How many mg C6H12O6/L will be required turn that nitrate into nitrogen gas?

Added by Jessica C.

Question

Please give Ace some feedback