Calculate the molar mass of sulphuric acid (H2SO4).

The atomic masses are given as H=1, S=32, O=16.

$$\text{Molar mass of H}_2\text{SO}_4 = (2 \times 1) + 32 + (4 \times 16) = 2 + 32 + 64 = 98 \text{ g/mol}$$

The target solution is 250 cm$^3$ (which is 0.250 dm$^3$) of 0.2 M $\text{H}_2\text{SO}_4$.

$$\text{Moles of H}_2\text{SO}_4 = \text{Molarity} \times \text{Volume (in dm}^3\text{)}$$ $$\text{Moles of H}_2\text{SO}_4 = 0.2 \text{ mol/dm}^3 \times 0.250 \text{ dm}^3 = 0.05 \text{ mol}$$

$$\text{Mass of H}_2\text{SO}_4 = \text{Moles} \times \text{Molar mass}$$ $$\text{Mass of H}_2\text{SO}_4 = 0.05 \text{ mol} \times 98 \text{ g/mol} = 4.9 \text{ g}$$

The density of pure sulphuric acid is 1.84 g/cm$^3$.

$$\text{Volume} = \frac{\text{Mass}}{\text{Density}}$$ $$\text{Volume of pure H}_2\text{SO}_4 = \frac{4.9 \text{ g}}{1.84 \text{ g/cm}^3} \approx 2.663 \text{ cm}^3$$

The calculated volume is approximately $2.66 \text{ cm}^3$, which matches option B.

The final answer is $\text{B. 2.66}$.