Chapter 12, Problem 52E

Interpretation Introduction

(a)

Interpretation:

The result of heating a sample of water from -20 to 200 ⁰C at a constant pressure of 600 Torr should be described.

Concept introduction:

When a phase change occurs, temperature remains constant. Temperature at which a solid starts to melt is called melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point liquid and vapor phases become indistinguishable.

Interpretation Introduction

(b)

Interpretation:

The result of increase in the pressure on a sample of iodine from $\text{90 mmHg to 100 atm}$ at a constant temperature of $114{}^0\text{C}$ should be described.

Concept introduction:

Temperature at which a solid starts to melt is called the melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point, the liquid and vapor phases become indistinguishable. A gas can be liquefied under the temperatures below critical temperature.

Interpretation Introduction

(c)

Interpretation:

The result of cooling the sample of carbon dioxide at ${\text{35 }}^{0}C$ to ${\text{-100 }}^{0}C$ at a constant pressure of $\text{50 atm}$ should be described.

Concept introduction:

Temperature at which a solid starts to melt is called melting point and temperature at which the vapor pressure of a liquid equals to atmospheric pressure is called boiling point. All three phases are in equilibrium at triple point and beyond the critical point liquid and vapor phases become indistinguishable. A gas can be liquefied under the temperatures below critical temperature.