The laboratory production of sulphuric acid involves the catalysed oxidation of sulphur in oxygen, followed by the separation of the resulting sulphur trioxide (SO₃) from sulphur dioxide (SO₂) as shown below: sulphur trioxide is collected as solid crystals in trap A, and sulphur dioxide is collected as a liquid in trap B, which consists of a sealable ampoule.

(a) The vapour pressure of SO₂ is 0.0167 x 10⁵ Pa at its triple point temperature of 197.7 K, and its enthalpy of vaporisation is reported as 26000 J mol^-1.  Upon collection, the SO₂ is to be stored in the ampoule B sealed by taps t, which has a maximum pressure tolerance of 8 atmospheres.  

Use the Clausius-Clapeyron equation to estimate the boiling temperature of SO₂ at atmospheric pressure (1 atm = 1.013 x 10⁵ Pa), and estimate whether the ampoule can safely be stored at a room temperature of 22 °C.

(b) In order to ensure that the SO₂ is retained, the experimenter considers increasing the pressure inside the apparatus to 2 atm, but then wonders if the increased pressure might encourage the SO₃ in trap A to melt.  Comment on this.