When 2 8 X 10 4 Kg Of A Certain Chemical Compound Is Dissolved In 0 579 L Of Water At 270c The Osmotic Pressure Of The 1 (21.07 KiB) Viewed 15 times
When 2.8 x 10-4 kg of a certain chemical compound is dissolved in 0.579 L of water at 270C, the osmotic pressure of the resultant solution is measured and found to have a value of 0.1625 atm. What is the molar mass of the chemical compound? (1 Point) O a. 107.5 g/mol O b. 6.602 g/mol O c. 73.3 g/mol O d. 57.9 g/mol
Normal boiling point = 68°C. Normal freezing point = -35°C Triple point: -35.2°C and 0.014 atm Critical point: 115°C and 122 atm A sample of the substance is placed in a container at a temperature of 68°C and a pressure of 0.95 atm. The substance is cooled to -40°C at constant pressure. What phase change(s) occur? (1 Point) none gas to liquid gas to solid gas to liquid to solid liquid to solid
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