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Standard XII

Physics

The Kelvin Scale

Boiling point...

Question

Boiling point of water at a place is found to be $110^{o} C$ . At this place:

external pressure is less than 1 atm

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external pressure is greater than 1 atm

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external pressure is equal to 1 atm

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cooking takes longer time

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Solution

The correct option is B external pressure is greater than 1 atm
Boiling point varies directly to the external pressure. Normal boiling point is $100 ° C .$ This is at $1$ atm. But here it is $110 ° C$ so pressure is above $1$ atm.

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Similar questions

The water boils when :

1.Saturated vapour pressure of water becomes equal to atmospheric pressure

2. Boiling point of water becomes more than atmospheric pressure

3. Saturated vapour pressure of water is less than atmospheric pressure

4. Vapour pressure of water becomes more than atmospheric pressure

Q. Assertion: At

1 a t m

, pure water can boil at a temperature less than

273 K

.
Reason: Water boils when the vapor pressure of the water is equal to the atmospheric pressure.

Comprehension # 2

Following passage explains the effect of temperature on the vapour pressure of the liquid.

Effect of temperature on vapour pressure

The quantity of heat required to evaporate a given liquid at constant temperature is defined as the heat of vaporisation. Variation of vapour pressure with temperature is given by,

Clausius-Clapeyron equation.

l o g_{e} P = - \frac{Δ H_{v a p}}{R T} + l o g_{e} A

A liquid is said to be at its boiling temperature if its vapour pressure is equal to external pressure. Therefore, the boiling point of water in particular and of liquids in general decreases as an altitude of a place increases where the external pressure is less than

1 a t m o s p h e r e

(normal b.p. of water is

373.15 K

1 a t m o s p h e r e

)

On top of mount everest, for example, where the atmospheric pressure is only about

260 m m H g

, water boils at approximately

71^{\circ} C

. Conversely, if the external pressure on a liquid is greater than

1 a t m

, the vapour pressure necessary for boiling than normal boiling is reached later, and the liquid boils at a temperature greater than the normal boiling point.

Clausius-Clapeyron equation can be written in the following form:

The temperature at which water boil depend on the pressure the water is under . At sea level the pressure is 100kPa,water boil at hundred degree Celsius the pressure in the pressure cooker is greater than 100kPa and boiling point of water is greater than hundred degree Celsius .

on the mountain top at the altitude of 7700 m the climber found that his fuel store couldn't raise the temperature of boiling water above 75 degrees celsius best explanation explanation of this

first the stop didn't have the sufficient oxygen 21 the few completely .

second the also called it absorb the heat from the water .

third the pressure was less than it was at sea level .

Fourth the air fresher was better than it was at sea level

Q. A substance does not have a normal boiling point when the pressure at the solid-liquid-gas triple point is greater than

1

atm.

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Boiling point of water at a place is found to be 110oC . At this place:

The correct option is B external pressure is greater than 1 atmBoiling point varies directly to the external pressure. Normal boiling point is 100°C. This is at 1 atm. But here it is 110°C so pressure is above 1 atm.

Boiling point of water at a place is found to be $110^{o} C$ . At this place:

The correct option is B external pressure is greater than 1 atm
Boiling point varies directly to the external pressure. Normal boiling point is $100 ° C .$ This is at $1$ atm. But here it is $110 ° C$ so pressure is above $1$ atm.