9. Example 11.10 How much energy is required to vaporize 305.4g of mercury (Hg). [Hg = 200.59g/mol] Hg(l) → Hg(g) ∆H

[answerhappygod]

9. Example 11.10
How much energy is required to vaporize 305.4g of mercury
(Hg). [Hg = 200.59g/mol]
Hg(l) →
Hg(g)
∆Hvap
= +59.10kJ/mol
10. The triple point of a substance is where 3
phases coexist for a particular substance. For example, according
to the following diagram, water
(H2O)
at a pressure of 0.06atm and a temperature of
0.01°C, water coexists as a gas (steam),
liquid (water), and solid (ice).

9 Example 11 10 How Much Energy Is Required To Vaporize 305 4g Of Mercury Hg Hg 200 59g Mol Hg L Hg G H 1 (173.89 KiB) Viewed 19 times

11.a Problem-6
What phase is water in at a pressure of 15,000kPa and temperature
of 100°C.

9 Example 11 10 How Much Energy Is Required To Vaporize 305 4g Of Mercury Hg Hg 200 59g Mol Hg L Hg G H 2 (272.42 KiB) Viewed 19 times

11.b Vapor Pressure vs Temperature
Which of the following substances has the highest and lowest
vapor pressures.

9 Example 11 10 How Much Energy Is Required To Vaporize 305 4g Of Mercury Hg Hg 200 59g Mol Hg L Hg G H 3 (162.62 KiB) Viewed 19 times

17. Example 12.7
If a solution is 6.55% by mass of
glucose(C6H12O6)
of solution. What is the molarity of the solution. Assume the
density of the solution is d=1.03g/mL.
[C6H12O6=180.16g/mol]
Water phase diagram Supercritical Fluid Critical Point 218 Water Ice Pressure (atm) Triple Point 0.06 Steam 374 00.01 100 Temperature (°C)
D 22,089 Critical point С 1 Ice (solid) Water (liquid) Pressure (kPa) 101 1 1 1 Triple point 1 1 0.6 B Water vapor (gas) 0 0.0 100 374 Temperature (°C)
11.b Vapor Pressure vs Temperature Which of the following substances has the highest and lowest vapor pressures. 1000 900 800 700 Normal boiling point (1 atm) 600 Vapor pressure (mmHg) 500 Diethyl ether (CH3CH2OCH2CH3) Bromine (Br) Ethanol (CH3CH2OH) - Water (H20) n-Octane [CH3(CH2).CH3] Ethylene glycol (HOCH2CH2OH) Mercury (Hg) 400 300 200 100 0 – 100 - 50 o 50 100 150 200 250 300 350 400