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The industrial production of sulfuric acid involves several steps - Edexcel - GCSE Chemistry - Question 7 - 2018 - Paper 1
Question 7
The industrial production of sulfuric acid involves several steps. One of these steps is the reaction of sulfur dioxide, SO₂, with oxygen to form sulfur trioxide, SO... show full transcript
Worked Solution & Example Answer:The industrial production of sulfuric acid involves several steps - Edexcel - GCSE Chemistry - Question 7 - 2018 - Paper 1
Step 1
What volume of sulfur trioxide, in dm³, is produced by the complete reaction of 750 dm³ of sulfur dioxide?
Answer
To determine the volume of sulfur trioxide (SO₃) produced, we can use the stoichiometry of the reaction from the equilibrium:
From the equation, 2 volumes of SO₂ produce 2 volumes of SO₃. Therefore, the relationship is 1:1. Thus, the volume of sulfur trioxide is the same as the volume of sulfur dioxide reacted:
- Volume of SO₃ produced = 750 dm³.
Step 2
Calculate the volume of oxygen needed to react completely with 750 dm³ of sulfur dioxide.
Answer
Using the balanced equation:
We can see that 2 dm³ of SO₂ react with 1 dm³ of O₂. Therefore, for 750 dm³ of SO₂, the volume of O₂ required is calculated as follows:
- Volume of O₂ needed = ( \frac{750 , \text{dm}^3}{2} = 375 , \text{dm}^3 )
Step 3
Calculate the mass, in kilograms, of 750 dm³ of sulfur dioxide, measured at room temperature and pressure.
Answer
To calculate the mass of sulfur dioxide (SO₂), we first need to determine the number of moles of sulfur dioxide using the molar volume at room temperature (24 dm³ per mole):
- Moles of SO₂ = ( \frac{750 , \text{dm}^3}{24 , \text{dm}^3/ ext{mol}} )
This gives us:
- Moles of SO₂ = 31.25 mol
Next, we use the relative formula mass of SO₂ (64 g/mol) to find the mass:
- Mass (g) = Moles × Molar Mass = 31.25 mol × 64 g/mol = 2000 g
Finally, converting grams to kilograms:
- Mass (kg) = ( \frac{2000}{1000} = 2 , ext{kg} )