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Question

The usefulness of a fertilizer depends upon percentage of nitrogen present in it. Find which of the following is a better fertilizer:
(a) ammonium nitrate [NH4NO3]
(b) ammonium phosphate [(NH4)3PO4]
(N = 14, H = 1, O = 16, P = 31)

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Solution

(a) Molecular mass of ammonium nitrate [NH4NO3] = [14 + (1 × 4) + 14 + (3 × 16)] g = 80 g
Mass of nitrogen in ammonium nitrate [NH4NO3] = (14 + 14) = 28 g
Percentage of N =Mass of N in the compoundMolecular mass of NH4NO3×100 = 2880×100=35

(b) Molecular mass of ammonium phosphate [(NH4)3PO4] = {[3×(14 + (1 × 4)] + 31 + (4 ×16)} g = 149 g
Mass of nitrogen in ammonium phosphate [(NH4)3PO4] = (14 × 3) g = 42 g
Percentage of N =Mass of N in compoundMolecular mass of NH43PO4×100=42149×100=28.2

Percentage of nitrogen is higher in ammonium nitrate; hence, it is a better fertiliser than ammonium nitrate.


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