Plot a vapor pressure curve for GaCl3 from the following vapor pressures. Determine the boiling

step 1 So firstly what you'd be expected to do here is to just plot the data. And so as a rough sketch

Plot a vapor pressure curve for GaCl3 from the following...

Plot a vapor pressure curve for $\mathrm{GaCl}_{3}$ from the following vapor pressures. Determine the boiling point of $\mathrm{GaCl}_{3}$ under a pressure of 250 torr from the plot: $$ \begin{array}{llrrllll} t\left({ }^{\circ} \mathrm{C}\right) & 91 & 108 & 118 & 132 & 153 & 176 & 200 \\ \operatorname{vp} \text { (torr) } & 20 . & 40 . & 60 . & 100 . & 200 . & 400 . & 760 . \end{array} $$

Plot a vapor pressure curve for $\mathrm{GaCl}_{3}$ from the following vapor pressures. Determine the boiling point of $\mathrm{GaCl}_{3}$ under a pressure of 250 torr from the plot:
$$
\begin{array}{llrrllll}
t\left({ }^{\circ} \mathrm{C}\right) & 91 & 108 & 118 & 132 & 153 & 176 & 200 \\
\operatorname{vp} \text { (torr) } & 20 . & 40 . & 60 . & 100 . & 200 . & 400 . & 760 .
\end{array}
$$

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Key Concepts

Vapor Pressure Curve

A vapor pressure curve represents the relationship between the temperature of a substance and its vapor pressure. As temperature increases, more molecules gain enough energy to overcome intermolecular forces, leading to higher vapor pressure. This curve is used to visualize how the vapor pressure changes with temperature, and it provides important insights into the thermodynamic behavior of a substance during phase transitions.

Boiling Point Determination

The boiling point of a substance is the temperature at which its vapor pressure equals the surrounding or external pressure. In the context of a vapor pressure curve, identifying the boiling point involves finding the temperature corresponding to a given ambient pressure, such as 250 torr in this example. This principle is central to understanding phase equilibrium and the conditions under which a liquid turns into vapor.

Phase Equilibrium

Phase equilibrium refers to the balance between different phases of a substance, such as liquid and vapor, where the rate of evaporation equals the rate of condensation. This equilibrium condition is achieved at the boiling point when the vapor pressure of the liquid equals the external pressure. The concept is pivotal in studying thermal properties and the stability of phases under varying pressure and temperature conditions.

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