At point D ( $273.16 K, 0.006 a t m$ ) all there phases of water coexist. Observed phase change when the temperature is increased from $- 10^{0} C t o + 10^{0} C,$ at a constant pressure of 0.006 atm is.

Solid → Liquid

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Liquid → Gas

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Solid → Gas

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Gas → Liquid

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Solution

The correct option is C Solid → Gas
Along the constant pressure line of P=0.006, we have ice (solid H₂O) on the left of the triple point, and steam (gaseous H₂O) on the right.

Thus, as we increase the temperature from below Tp to above Tp, we observe a solid → gas phase transition, i.e., we see ice directly turning into gas without going through the water phase. Magical!

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Similar questions

At point D (

273.16 K, 0.006 a t m

) all there phases of water coexist. Observed phase change when the temperature is increased from

- 10^{0} C t o + 10^{0} C,

at a constant pressure of 0.006 atm is.

In a closed container of constant volume, the pressure of water exhibits an interesting dependence on temperature -

The point D (273.16 K,0.006 atm) is called the triple point, Tp, of water, where all there phases coexist. What is the observed phase change when the temperature is increased from -10⁰C to +10⁰C, while maintaining a constant pressure of 0.006 atm?

In a closed container of constant volume, the pressure of water exhibits an interesting dependence on temperature -