Question

SO2 in the atmosphere contributes to acid rain. The equation for the formation of the acid is represented by: 2SO2 (g) + O2 (g) + 2H2O (l) ------> H2SO4 (aq)
What mass of sulphuric acid will form from 50.0L of sulphur dioxide at SLC (Standard Laboratory Conditions)?

Answer 1

Answer on Question #50516, Chemistry, Inorganic Chemistry

$\mathrm{SO}_2$ in the atmosphere contributes to acid rain. The equation for the formation of the acid is represented by: $2\mathrm{SO}_2(\mathrm{g}) + \mathrm{O}_2(\mathrm{g}) + 2\mathrm{H}_2\mathrm{O}(\mathrm{l}) \longrightarrow 2\mathrm{H}_2\mathrm{SO}_4$ (aq)

What mass of sulphuric acid will form from 50.0L of sulphur dioxide at SLC (Standard Laboratory Conditions)?

Solution:

Standard Laboratory Conditions is 1 atm (101.325 kPa) and $25^{\circ}\mathrm{C}$ (298.15 K). Using Mendeleev - Clapeyron equation:

$$p \times V = n \times R \times T$$ $$n = \frac {p \times V}{R \times T}$$

R is ideal gas constant, 8.31 J/(mol×K)

It is obvious that

$$n (S O _ {2}) = n (H _ {2} S O _ {4})$$ $$n = \frac {m}{M _ {r}}$$

$\mathrm{M_r(H_2SO_4)} = 98,079 \mathrm{~g/mol}$

$$\frac {m}{M _ {r}} = \frac {p \times V}{R \times T}$$ $$m = \frac {p \times V \times M _ {r}}{R \times T}$$ $$m = \frac {101325\ \mathrm{Pa} \times 0.05\ \mathrm{m}^3 \times 98.079\ \mathrm{g/mol}}{8.31\ \frac{\mathrm{J}}{\mathrm{K} \times \mathrm{mol}} \times 298.15\ \mathrm{K}} = \frac {496892.73375}{2477.6265} = 200.55\ \mathrm{g}$$

Answer:

200.55 g of sulphuric acid

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