GCSE OCR Gateway Chemistry 10.4 Haber Process & NPK Fertilisers: Ammonium sulfate, (NH4)2SO4, is

Ammonium sulfate, (NH4)2SO4, is a fertiliser - OCR Gateway - GCSE Chemistry - Question 20 - 2019 - Paper 2

Question 20

Ammonium sulfate, (NH4)2SO4, is a fertiliser. Ammonium sulfate can be manufactured from ammonia and sulfuric acid. a) Sulfuric acid is manufactured in a series of ... show full transcript

Worked Solution & Example Answer:Ammonium sulfate, (NH4)2SO4, is a fertiliser - OCR Gateway - GCSE Chemistry - Question 20 - 2019 - Paper 2

Step 1

Step 1: Write balanced symbol equations for each step of this process.

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Answer

The reaction for the combustion of sulfur in oxygen is:

ightarrow SO_2 $$

Step 2

Step 2: Write balanced symbol equations for each step of this process.

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Answer

The reaction for the formation of sulfur trioxide is:

ightarrow 2SO_3 $$

Step 3

Step 3: Write balanced symbol equations for each step of this process.

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Answer

The reaction for the production of sulfuric acid is:

ightarrow H_2SO_4 $$

Step 4

What type of reaction is this?

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This is a neutralization reaction, where an acid (sulfuric acid) reacts with a base (ammonia) to form a salt (ammonium sulfate).

Step 5

Show that the maximum mass of ammonium sulfate that can be made from 51.0 g of ammonia is 198.0 g.

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Answer

Using molar masses:

Molar mass of NH3 = 17.0 g/mol
Molar mass of (NH4)2SO4 = 132.14 g/mol

Calculating moles of ammonia: $n(NH3) = \frac{51.0 \, g}{17.0 \, g/mol} = 3.0 \, mol$

From the balanced equation: 2 moles of NH3 produce 1 mole of (NH4)2SO4. Thus, the moles of (NH4)2SO4 produced are: $n((NH4)2SO4) = \frac{3.0 \, mol}{2} = 1.5 \, mol$

Calculating the mass of ammonium sulfate produced: $mass = n \times molar \, mass \rightarrow 1.5 \, mol \times 132.14 \, g/mol = 198.21 \, g$

This confirms that the theoretical maximum mass of ammonium sulfate is 198.21 g.

Step 6

Describe how he can obtain a pure dry sample of ammonium sulfate.

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Answer

To obtain a pure dry sample, the student can perform the following steps:

Evaporation: Heat the solution of ammonium sulfate to evaporate the water, which concentrates the solution.
Crystallization: Allow the concentrated solution to cool slowly so that pure ammonium sulfate crystals form.
Filtration: Filter the solution to collect the crystals of ammonium sulfate.
Drying: Gently dry the crystals using filter paper or a warm oven to obtain a pure dry sample.

Ammonium sulfate, (NH4)2SO4, is a fertiliser - OCR Gateway - GCSE Chemistry - Question 20 - 2019 - Paper 2

Worked Solution & Example Answer:Ammonium sulfate, (NH4)2SO4, is a fertiliser - OCR Gateway - GCSE Chemistry - Question 20 - 2019 - Paper 2

Step 1: Write balanced symbol equations for each step of this process.

Step 2: Write balanced symbol equations for each step of this process.

Step 3: Write balanced symbol equations for each step of this process.

What type of reaction is this?

Show that the maximum mass of ammonium sulfate that can be made from 51.0 g of ammonia is 198.0 g.

Describe how he can obtain a pure dry sample of ammonium sulfate.

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