Assertion: At normal pressure (1 atm ) boiling point of water is 100 degree C or 373.15 K. Reason : As the pressure increases, boiling point of water also increases. a) If both assertion and reason are true then the reason is correct explanation of assertion. b) If both assertion and reason are true, but reason is not the correct explanation of assertion. c) If assertion is true, but reason is false d) If assertion is false, but reason is true e) Both assertion and reason are false Choose the correct option given in the question.
Answers
Answer:
c. Assertion is true but the reason is false.
Explanation:
The boiling point remains constant it can't be changed.
To change it we need to apply enough pressure to convert it into solid state.
If the pressure is enough that it can be converted into solid state then Option a can be correct
Answer:
The assertion and reason both are true, but the reason is not the correct explanation of the assertion (OPTION-B).
Explanation:
Definition of boiling point
The boiling point is defined as the temperature at which the vapour pressure of the liquid becomes equal to the atmospheric pressure of the surrounding environment.
This is the sole reason that water boils faster in hilly areas whereas it does not tend to boil at sea levels at lower temperatures.
At lower pressure, the vapour pressure equivalence is reached quicker at lower temperatures, so the liquid starts boiling at lower temperatures and vice-versa.
Apart from pressure, the quantity of solutes present in the solvent is also a determining factor for the boiling point.
The boiling point of pure water at 1 atm. pressure is 100°C or 373K.
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