Textbook Question
Explain the observed trend in the boiling points of these compounds.
H2Te -2 °C
H2Se -41.5 °C
H2S -60.7 °C
H2O 100 °C
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Ch.11 - Liquids, Solids & Intermolecular Forces
Chapter 11, Problem 87
Examine the phase diagram for iodine shown in Figure 11.39(a). What state transitions occur as we uniformly increase the pressure on a gaseous sample of iodine from 0.010 atm at 185 °C to 100 atm at 185 °C?
Verified step by step guidance1
Identify the initial state of iodine at 0.010 atm and 185 °C on the phase diagram. This is likely in the gaseous region.
Determine the path of pressure increase on the phase diagram from 0.010 atm to 100 atm while keeping the temperature constant at 185 °C.
Observe the phase boundaries that the path crosses as pressure increases. Note the transitions from gas to any other phases.
Identify the first phase transition as the pressure increases. This is likely from gas to solid, as iodine sublimates under certain conditions.
Continue to increase the pressure and note any further phase transitions, such as from solid to another phase, if applicable.
Related Practice
Textbook Question
The vapor pressure of water at 25 °C is 23.76 torr. If 1.25 g of water is enclosed in a 1.5-L container, will any liquid be present? If so, what mass of liquid?
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Textbook Question
The vapor pressure of CCl3F at 300 K is 856 torr. If 11.5 g of CCl3F is enclosed in a 1.0-L container, will any liquid be present? If so, what mass of liquid?
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Open Question
Carbon tetrachloride displays a triple point at 249.0 K and a melting point (at 1 atm) of 250.3 K. Which state of carbon tetrachloride is more dense, the solid or the liquid, and why?
Open Question
Four ice cubes at exactly 0 °C with a total mass of 53.5 g are combined with 115 g of water at 75 °C in an insulated container. If no heat is lost to the surroundings, what is the final temperature of the mixture?
Textbook Question
A sample of steam with a mass of 0.552 g and at a temperature of 100 °C condenses into an insulated container holding 4.25 g of water at 5.0 °C. Assuming that no heat is lost to the surroundings, what is the final temperature of the mixture?
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