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
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.
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Transcribed Image Text:Problems
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.
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