A pond’s water contains 25.0 mg/l of algae.
Find the theoretical carbonaceous oxygen demand (CBOD) of water in the pond
Find the total theoretical (carbonaceous plus nitrogenous ) oxygen demand (BOD) on water in the pond
Note: algae can be represented by the chemical formula C6H15O6N.
Theoretically oxygen in pond can be consumed following equations 1 and 2.
C6H15O6N + 6O2 → 6CO2 + 6H2O + NH3 (1)
NH3 + 2O2 → NO3- + H+ + H2O (2)
Let's consider 1L of the pond's water
Given the mass of algae = 25.0 mg = 25.0 mg x(1 g / 1000 mg) = 0.0250 g
Molecular mass of algae (C6H15O6N) = 197.18 g/mol
Moles of algae(C6H15O6N) = mass / molecular mass = 0.0250 g / 197.18 g/mol = 1.268x10-4 mol
The given chemical reaction for the oxidation of the organic compound is
C6H15O6N + 6O2 → 6CO2 + 6H2O + NH3
1 mol 6 mol 6 mol 6 mol 1 mol
Hence moles of oxygen required for the oxidation of 1.268x10-4 mol of C6H15O6N
= (1.268x10-4 mol C6H15O6N) x (6 mol O2 / 1 mol C6H15O6N) = 7.61x10-4 mol O2 /L
Molecular mass of O2 = 32 g/mol
Hence mass of O2 required = 7.61x10-4 mol x 32 g O2 / mol = 0.0243 g O2 / L = 24.3 mg / L
Hence theoretical carbonaceous oxygen demand (CBOD) of water in the pond = 24.3 mg / L (answer)
Nitrogenous Oxygen demand:
1 mol of C6H15O6N forms 1 mol of NH2.
Hence moles of NH3 formed by 1.268x10-4 mol C6H15O6N
= (1.268x10-4 mol C6H15O6N) x ( 1mol NH3 / 1mol C6H15O6N) =1.268x10-4 mol NH3
Now NH3 undergoes oxidation through the following reaction
NH3 + 2O2 → NO3- + H+ + H2O
1 mol 2 mol
Hence moles of O2 required by 1.268x10-4 mol NH3 moles of NH3
= 1.268x10-4 mol NH3 x ( 2 mol O2 / 1 mol NH3) = 2.536x10-4 mol O2.
Molecular mass of O2 = 32 g/mol
Hence mass of O2 required = 2.536x10-4 mol x 32 g O2 / mol = 0.00811 g O2 / L = 8.11 mg / L
Hence theoretical nitrogenus oxygen demand of water in the pond = 8.11 mg / L
Hence total theoretical (carbonaceous plus nitrogenous ) oxygen demand (BOD) on water in the pond
= 24.3 mg / L + 8.11 mg/L
= 32.4 mg/L (answer)
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