Question

At what temperature and pressure can all three phases of water exist simultaneously? 1.20°C, 760 mmHg 0.01°C, 4.58 mmHg 4.58°C, 0.08 mmHg 0.01°C, 760 mmHg

Answer 1

0,01°C and 4,58 mmHg (≈611,7 Pa)

Answer 2

Answer:

0.01°C, 4.58 mmHg

Explanation:

Water exists in 3 phases; solid, liquid and gas. The three phases can be interconverted at different temperatures.

1) Fusion involves melting of solid to liquid. This occurs at the melting point of the solid. The equilibrium can be represented as:

H2O(s) ↔ H2O(l)

2) Vaporization involves evaporation of the liquid to gas. This occurs at the boiling point of the liquid.

H2O(l) ↔ H2O(g)

3) Sublimation involves the direct conversion of solid to gas.

H2O(s) ↔ H2O(g)

Triple point of water is the temperature and pressure at which all three phases coexist. This is the point in the water phase diagram, where the melting, vaporization and sublimation curves meet.  This occurs at a temperature of 0.01 C and pressure of 4.58 mmHg.