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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Ch.11 - Liquids, Solids & Intermolecular Forces
Chapter 11, Problem 88
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?
Verified step by step guidance1
Identify the given data: the triple point temperature is 249.0 K, and the melting point at 1 atm is 250.3 K.
Understand that the triple point is the condition under which all three phases (solid, liquid, and gas) coexist in equilibrium.
Recognize that the melting point at 1 atm is higher than the triple point temperature, indicating that the solid is more stable at lower temperatures and pressures.
Recall that if the melting point at 1 atm is higher than the triple point temperature, it suggests that the solid is denser than the liquid. This is because, at the triple point, the solid can exist at a lower pressure than the liquid, implying higher density.
Conclude that the solid state of carbon tetrachloride is more dense than the liquid state, as indicated by the relationship between the triple point and the melting point.
Related Practice
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
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?
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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Open Question
Draw a heating curve (such as the one in Figure 11.36) for 1 mole of methanol beginning at 170 K and ending at 350 K. Assume that the values given here are constant over the relevant temperature ranges. Melting point: 176 K, Boiling point: 338 K, ΔH_fus: 2.2 kJ/mol, ΔH_vap: 35.2 kJ/mol, C_s,solid: 105 J/mol·K, C_s,liquid: 81.3 J/mol·K, C_s,gas: 48 J/mol·K.