Imagine a substance with the following points on the phase diagram: a triple point at .5 atm and -5°C; a normal melting point at 20°C; a normal boiling point at 150°C; and a critical point at 5 atm and 1000°C. The solid- liquid line is "normal" (meaning positive sloping). For this, complete the following: 1. Roughly sketch the phase diagram, using units of atmosphere and Kelvin. 1-solid, 2-liquid, 3-gas, 4-supercritical fluid, point O-triple point, C-critical point -78.5 °C (The phase of dry ice changes from solid to gas at -78.5 °C) 2. Rank the states with respect to increasing density and increasing energy. 3. Describe what one would see at pressures and temperatures above 5 atm and 1000°C.

Imagine a substance with the following points on the phase diagram: a triple point at .5 atm and -5°C; a normal melting point at 20°C; a normal boiling point at 150°C; and a critical point at 5 atm and 1000°C. The solid- liquid line is "normal" (meaning positive sloping). For this, complete the following: 1. Roughly sketch the phase diagram, using units of atmosphere and Kelvin. 1-solid, 2-liquid, 3-gas, 4-supercritical fluid, point O-triple point, C-critical point -78.5 °C (The phase of dry ice changes from solid to gas at -78.5 °C) 2. Rank the states with respect to increasing density and increasing energy. 3. Describe what one would see at pressures and temperatures above 5 atm and 1000°C.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter9: Liquids, Solids, And Materials

Section: Chapter Questions

Problem 116QRT

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