Question

Describe IN POINT FORM what happens when you raise the temperature of a sample of water from - 100 to +300 at a constant pressure of 0.5 atm. You'll type in your answer below. MAKE REASONABLE ESTIMATES OF TEMPERATURE AS NEEDED. (Assume that 0.5 atm is about where the little double dashes are on the Pressure axis, below the 1 atm mark and remember, while you do need to be reasonable, you are just taking ESTIMATES.) HO Platin) 218 + 200+ 40+ 0.006 o.oo loo 200 375 T(°C) AXES ARE NOT LINEAR

Answer 1

In the phase diagram of water,

"1" represent the freezing point curve showing equilibrium between ice and water at different temperatures.

where, "2" represent the vapour pressure curve for liquid water.The vapour pressure increases with rise in temperature.The point on this line denotes the pressure at which water and it's vapour exist in equilibrium at different temperatures.

Where "3" represent the vapour pressure(cvurve) for ice.It shows the vapour pressure at which ice is in equilibrium with it's vapour at different temperatures.

Therefore"A" represent the solid phase of water(ice).

"B" represent the vapour state of water, and "C" represent the liquid state of water.

So at constant pressure that is at 0.5 atm, if we increase temperature from -100 degree centrigrade, innitially it will be in solid state (ice) at -1000c, then upon increasing it will start liquify. At 500c, it will be in "C" state, that is it will be in liquid state. On more increasing e.g at 1000c, it will start vapourise as it will reach the liquid-vapour equilibrium curve which contains point "2".

Then at 2000c, it will be in complete vapour phase. And at 3000c, water will be completely vapourise.