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6 (a) Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃ - Edexcel - GCSE Chemistry - Question 6 - 2016 - Paper 1

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6 (a) Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃. (relative atomic masses: H = 1.0, N = 14, O = 16) (b) In the extraction of titanium ... show full transcript

Worked Solution & Example Answer:6 (a) Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃ - Edexcel - GCSE Chemistry - Question 6 - 2016 - Paper 1

Step 1

Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃.

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Answer

To determine the percentage by mass of nitrogen in ammonium nitrate (NH₄NO₃), we first need to calculate the relative formula mass of the compound.

Calculate the relative formula mass:
- Relative atomic mass of N = 14 (2 nitrogen atoms)
- Relative atomic mass of H = 1 (4 hydrogen atoms)
- Relative atomic mass of O = 16 (3 oxygen atoms)
$\text{Relative formula mass of NH₄NO₃} = (2 \times 14) + (4 \times 1) + (3 \times 16) = 80$
Calculate the total mass of nitrogen in NH₄NO₃:
- Total mass of nitrogen = $2 \times 14 = 28$
Calculate the percentage by mass of nitrogen: $\text{Percentage by mass of nitrogen} = \left( \frac{\text{Mass of nitrogen}}{\text{Relative formula mass of NH₄NO₃}} \right) \times 100$ $= \left( \frac{28}{80} \right) \times 100 = 35\%$

Step 2

Calculate the maximum mass of titanium that can be obtained from 500 tonnes of titanium(IV) chloride.

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Answer

To find the maximum mass of titanium that can be obtained from 500 tonnes of titanium(IV) chloride (TiCl₄), we need to use the stoichiometry of the reaction:

Identify the stoichiometry:
- From the reaction: TiCl₄ + 4Na → Ti + 4NaCl, we see that 1 mole of TiCl₄ produces 1 mole of Ti.
Calculate the mass of 500 tonnes of TiCl₄ in kg:
- 500 tonnes = 500,000 kg
Calculate the number of moles of TiCl₄:

$\text{Number of moles of TiCl₄} = \frac{\text{mass}}{\text{molar mass}} = \frac{500,000 \text{ kg}}{190 \text{ g/mol}}$
- Converting to grams: $500,000 \text{ kg} = 500,000,000 \text{ g}$
- Thus, the number of moles: $\frac{500,000,000}{190} \approx 2,631,578.95 \text{ moles}$
Calculate the mass of titanium produced:
- Using the molar mass of titanium (Ti = 48 g/mol): $\text{Mass of Ti} = \text{Number of moles} \times \text{molar mass} = 2,631,578.95 \text{ moles} \times 48 \text{ g} \approx 126,315,789.5 g$
- Converting back to tonnes: $\text{Mass of titanium} \approx 126,315.79 \text{ tonnes}$

Step 3

State a problem this may cause for the manufacturer.

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Answer

One significant problem that may arise from reactions producing unwanted products is the increase in production costs. Unwanted by-products require additional separation and purification processes, leading to increased time and resource expenditure. Moreover, the presence of these by-products might reduce the yield of the desired product, further impacting profitability. Environmental regulations related to waste disposal can also present challenges, necessitating waste treatment solutions that can add to operational costs.

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6 (a) Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃ - Edexcel - GCSE Chemistry - Question 6 - 2016 - Paper 1

Worked Solution & Example Answer:6 (a) Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃ - Edexcel - GCSE Chemistry - Question 6 - 2016 - Paper 1

Calculate the percentage by mass of nitrogen in ammonium nitrate, NH₄NO₃.

Calculate the maximum mass of titanium that can be obtained from 500 tonnes of titanium(IV) chloride.

Calculate the number of moles of TiCl₄:

State a problem this may cause for the manufacturer.

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