10.1 The incomplete equations below show the four steps involved in the industrial preparation of sulfuric acid (H₂SO₄) - NSC Physical Sciences - Question 10 - 2021 - Paper 2
Question 10
10.1 The incomplete equations below show the four steps involved in the industrial preparation of sulfuric acid (H₂SO₄). A and B represent two compounds.
Step I: S(... show full transcript
Worked Solution & Example Answer:10.1 The incomplete equations below show the four steps involved in the industrial preparation of sulfuric acid (H₂SO₄) - NSC Physical Sciences - Question 10 - 2021 - Paper 2
Step 1
10.1.1 Compound A
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Compound A is
Sulphur dioxide (SO₂).
Step 2
10.1.2 Compound B
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Compound B is
Sulphur trioxide (SO₃).
Step 3
10.1.3 The catalyst used in Step II
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The catalyst used in Step II is
Vanadium pentoxide (V₂O₅).
Step 4
10.1.4 Write down a balanced equation for this reaction.
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The balanced equation for the preparation of ammonium sulphate from sulfuric acid is:
H2SO4+2NH4NO3→(NH4)2SO4+2HNO3
Step 5
10.2.1 Write down the meaning of NPK.
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NPK stands for
Nitrogen (N), Phosphorous (P), and Potassium (K), which are the primary nutrients in fertilisers.
Step 6
10.2.2 Calculate the mass of the fertiliser in the bag.
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To calculate the total mass of fertiliser contained in the bag, we first determine the mass of nitrogen:
The molecular weight of ammonium nitrate (NH₄NO₃) is:
N: 14 g/mol × 2 (2 nitrogen atoms) = 28 g/mol
H: 1 g/mol × 4 (4 hydrogen atoms) = 4 g/mol
O: 16 g/mol × 3 (3 oxygen atoms) = 48 g/mol
Total = 28 + 4 + 48 = 80 g/mol.
The total mass of nitrogen in 4 kg of ammonium nitrate is:
ext{Mass of N} = 4 ext{ kg} imes rac{28 ext{ g}}{80 ext{ g}} = 1.4 ext{ kg}.
The ratio of nitrogen to phosphorous and potassium is:
extN:P:K=1:3:2
Therefore,
Total mass of fertiliser = 1.4 kg (N) + 2.8 kg (P) + 4.2 kg (K) = 8.4 kg.
