Question

5) Consider the phase diagram for carbon dioxide(10). Supercritical fluid Solid Liquid Pressure (atm) -78.5 -56.4 Temperature (°C)— a) What is the critical temperature for carbon dioxide? b) What is the critical pressure for carbon dioxide? c) What phase(s) is/are present at -10°C and 30 atm. d) What phase(s) is/are present at -60°C and 10 atm. - e) What phase(s) is/are present at-78.5°C and 1 atm. f) What phase(s) is/are present at-56.4°C and 5.11 atm. g) What is the normal sublimation point of carbon dioxide, 6) True or False a. Instantaneous dipoles exist is all molecules and atoms. b. Viscosity decreases with increasing temperature. c. For molecules with similar size and molar mass, those with higher polarity would have lower boiling points d. Van der Waals forces are weaker than ionic bonds but stronger than covalent bonds. e. Liquids with weaker intermolecular interactions have lower viscosity. f. Ice has a higher density than water because ice has a ordered cagelike structure due to hydrogen bonding. g. The strength of dispersion forces depends on the molar mass and has little to due with the shape of the molecules involved. -

Answer 1

5.

A) 31.1 degree C Here in the graph the critical temperature at which the gas become supercritical

B) 73.0 atm the pressure corresponds to critical temperature

C) Liquid phase, because this temperature and pressure falls in liquid region

D) Solid phase at this temperature and pressure the aolid phase will be there.

E) solid and gas, this point will lie of sublimation curve.

F) solid, liquid and gas. This is the triple point where all phases exist.

G) -56.5 degree C and 1 atm pressure because these are normal pressure.