The highest boiling point is expected for:
a.) Isooctane
b.) n-Octane
c.) 2,2,3,3-Tetramethyl butane
d.) n-Butane

Hint: n-Octane is a straight-chain exacerbate that has a very large surface area. Along these lines, there are more van der Waals forces of attraction, bringing about high boiling points.

Complete step by step solution:
Boiling point is characterized as the specific temperature at which the vapor pressure of the fluid is equivalent to the environmental pressure. Take, for example, the instance of water.
The vapor-pressure of the water at room temperature is 0.0313 atm. (vapor pressure - is the pressure applied by the vapor delivered by a fluid or strong substance in a shut compartment or space) .

To expand the vapor pressure of the water, we have to build the temperature (since vapor pressure is straightforwardly corresponding to temperature). Thus, we heat the water and increment the vapor pressure. After some time, the temperature of water increases too . At that occasion, the vapor pressure of water likewise increments to 1 atm which is equivalent to the barometric pressure at a drift level. Along these lines, we give \[100{}^\circ C\] the title of 'boiling point of a drift water level'.

This additionally implies the boiling point of water above the ocean level isn't \[100{}^\circ C\].

The correct answer is B.

Note: Along these lines, less measure of increment in vapor pressure is required to arrive at the barometric pressure. In this way, the measure of heat required to build the vapour pressure of water to arrive at the climatic pressure is not as much as that required at lower elevations. Consequently, the boiling point is lesser at higher heights. This clarifies the way that the boiling point of adrift water level is \[100{}^\circ C\] yet on the head of Mt. Everest it is \[71{}^\circ C\].