Textbook Question
A sealed flask contains 0.55 g of water at 28 °C. The vapor pressure of water at this temperature is 28.35 mmHg. What is the minimum volume of the flask in order that no liquid water be present in the flask?
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Ch.11 - Liquids, Solids & Intermolecular Forces
Chapter 11, Problem 96
Consider a planet where the atmospheric pressure at sea level is 2500 mmHg. Does water behave in a way that can sustain life on the planet?
Verified step by step guidance1
<Understand the problem: We need to determine if water can exist in a liquid state under the given atmospheric pressure of 2500 mmHg, which is crucial for sustaining life.>
<Recall the concept of boiling point: The boiling point of a liquid is the temperature at which its vapor pressure equals the external pressure.>
<Use the known data: On Earth, water boils at 100°C under 760 mmHg. We need to find the boiling point of water under 2500 mmHg.>
<Apply the Clausius-Clapeyron equation: This equation relates the change in vapor pressure with temperature, which can help estimate the boiling point under different pressures.>
<Consider the implications: If the boiling point is too low or too high, it might affect the ability of water to sustain life as we know it.>
Related Practice
Open Question
Based on the phase diagram of CO2 shown in Figure 11.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (b) 5.1 atm, (c) 10 atm, and (d) 100 atm.
Textbook Question
Based on the phase diagram of CO2 shown in Figure 11.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (a) 1 atm
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