At high altitudes such as hill stations, water boils at a temperature lower than 100°C, whereas in a pressure cooker it boils above 100°C. Which of the following statements correctly explains this phenomenon?
- AOption (a)
Water molecules at high altitude have lower kinetic energy than at sea level, so they boil at a lower temperature.
- BOption (b)
Boiling point of a liquid is independent of external pressure and depends only on temperature.
- COption (c)
Boiling point of a liquid increases with an increase in atmospheric pressure and decreases with a decrease in atmospheric pressure.
- DOption (d)
Boiling point of a liquid decreases with an increase in atmospheric pressure and increases with a decrease in atmospheric pressure.
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Correct answer
Boiling point of a liquid increases with an increase in atmospheric pressure and decreases with a decrease in atmospheric pressure.
Why this answer is correct
The correct answer is Boiling point of a liquid increases with an increase in atmospheric pressure and decreases with a decrease in atmospheric pressure..
Key Points
- The boiling point of a liquid is defined as the temperature at which its vapor pressure equals the external atmospheric pressure surrounding the liquid.
- At high altitudes, such as hill stations, the atmospheric pressure is significantly lower than at sea level due to the thinner air column above. Because the external pressure is lower, water requires less heat to match its vapor pressure with the environment, causing it to boil at temperatures below 100°C.
- In a pressure cooker, the steam produced is trapped inside a sealed container, which rapidly increases the internal pressure. This elevated pressure prevents water molecules from escaping into the gas phase until a much higher temperature is reached, typically around 120°C.
- The physical principle involved is that the boiling point is directly proportional to the external pressure; as pressure increases, more thermal energy is needed to facilitate the phase change from liquid to gas.
Additional Information
- Vapor Pressure:
- It is the pressure exerted by a vapor in thermodynamic equilibrium with its condensed phases at a given temperature in a closed system.
- As temperature increases, the kinetic energy of molecules increases, thereby increasing the vapor pressure.
- Clausius-Clapeyron Equation:
- This equation characterizes the phase transition between two states of matter and mathematically relates the dependence of boiling point on pressure.
- Practical Implications:
- In mountainous regions, food takes longer to cook in open vessels because the water cannot exceed its low boiling point (e.g., 92°C), providing less heat to the food.
- Autoclaves used in hospitals for sterilization operate on the same principle as a pressure cooker to reach temperatures high enough to kill resistant bacteria and spores.