The industrial production of sulfuric acid involves several steps - Edexcel - GCSE Chemistry - Question 7 - 2018 - Paper 1

From the balanced equation, we have:

$2SO_2(g) + O_2(g) \rightarrow 2SO_3(g)$

This indicates that 2 volumes of sulfur dioxide react with 1 volume of oxygen. Therefore, for 750 dm³ of sulfur dioxide, the volume of oxygen required is computed as follows:

$\text{Volume of } O_2 = \frac{750 \, \text{dm}^3}{2} = 375 \, \text{dm}^3$

So, the volume of oxygen needed is 375 dm³.

To find the mass of sulfur dioxide (SO₂), we first use its molar volume at room temperature and pressure. One mole of any gas occupies 24 dm³.

First, we calculate the number of moles in 750 dm³ of sulfur dioxide:

$\text{Number of moles} = \frac{750 \, \text{dm}^3}{24 \, \text{dm}^3/mol} = 31.25 \, \text{moles}$

Next, we can calculate the mass using the relative formula mass of SO₂, which is 64 g/mol:

$\text{Mass} = \text{Number of moles} \times \text{Molar mass} = 31.25 \, \text{moles} \times 64 \, \text{g/mol} = 2000 \, g$

Finally, convert grams to kilograms:

$\text{Mass} = \frac{2000 \, g}{1000} = 2 \, kg$

Thus, the mass of 750 dm³ of sulfur dioxide is 2 kg.