Question

Why do liquids have a vapor pressure? Do all liquids have vapor pressures? Explain. Do solids exhibit vapor pressure? Explain. How does vapor pressure change with changing temperature? Explain.

Short answer

Vapor pressure is the pressure exerted by the vapor of a substance above its liquid or solid phase when it reaches equilibrium. All liquids have vapor pressures due to the distribution of kinetic energies that enable some molecules to escape the liquid's surface and become gaseous. Solids can also exhibit vapor pressure, but it is generally lower than in liquids as molecules in a solid are less mobile. The vapor pressure of a substance is dependent on temperature and is described by the Clausius-Clapeyron equation: \[ ln(P) = -\frac{\Delta H_{vap}}{R}(\frac{1}{T} - \frac{1}{T_0}) + ln(P_0) \] where P is the vapor pressure, ΔH_vap is the enthalpy of vaporization, T is the temperature, T_0 is the reference temperature, P_0 is the vapor pressure at the reference temperature, and R is the gas constant.

Step-by-step solution

Definition of Vapor Pressure

Vapor pressure is the pressure exerted by the vapor of a substance above its liquid or solid phase when it reaches a state of equilibrium. In other words, it's the pressure generated by the molecules in the gaseous phase of a substance when they are in equilibrium with the molecules in the condensed phase (liquid or solid).

Vapor Pressure of Liquids

All liquids have some degree of vapor pressure. This is because the molecules in a liquid have a distribution of kinetic energies, and some of these molecules have enough energy to escape the liquid's surface and become gas particles. These gas particles exert pressure on the container they are in, which is referred to as the liquid's vapor pressure.

Vapor Pressure of Solids

Solids can also exhibit vapor pressure, although it is generally lower than that of liquids. This occurs because the molecules in a solid are not as mobile as those in a liquid. Molecules within a solid are usually held in a rigid lattice structure. However, some molecules at the surface possess enough kinetic energy to break free from the structure and enter the gaseous phase, creating the solid's vapor pressure.

Vapor Pressure and Temperature

The vapor pressure of a substance is dependent on temperature. As the temperature increases, the kinetic energy of the molecules in the liquid or solid increases. With more kinetic energy, a greater number of molecules will have enough energy to escape the surface and enter the gaseous phase, and the vapor pressure increases. Conversely, as the temperature decreases, the vapor pressure will also decrease. This relationship between vapor pressure and temperature can be described using the Clausius-Clapeyron equation: \[ ln(P) = -\frac{\Delta H_{vap}}{R}(\frac{1}{T} - \frac{1}{T_0}) + ln(P_0) \] where P is the vapor pressure, ΔH_vap is the enthalpy of vaporization, T is the temperature, T_0 is the reference temperature, P_0 is the vapor pressure at the reference temperature, and R is the gas constant.