Question

What is the normal boiling point of methane? In what state will it be $ - {170^0}C $ at atmospheric pressure?

Answer 1

Hint: Methane is a saturated hydrocarbon with the molecular formula of $ C{H_3}OH $ in which the intermolecular forces present are Vander Waal interaction. These very weak forces lead to the low boiling and melting point. The normal boiling point of methane is $ - {162^0}C $ . below this temperature methane exists as liquid.

Complete Step By Step Answer:
Boiling point is defined as the point or temperature at which the liquid can convert into gas or vapour.
Alkanes are saturated hydrocarbons in which the bonding between the carbon and hydrogen atoms are single covalent bonds. These compounds are inert due to the less polarity of the carbon-carbon and carbon-hydrogen bonds. The intermolecular forces in alkanes are weak. Vander Waal forces lead to the low boiling points and low melting points.
The boiling point of methane is $ - {162^0}C $ which means at this temperature the methane which is in liquid state can start to convert into gaseous or vapour state.
Given temperature is $ - {170^0}C $ which is below the normal boiling point of methane. It reveals that at this temperature methane will be in a liquid state.
Thus, the normal boiling point of methane is $ - {162^0}C $ it will be in liquid state at $ - {170^0}C $ at atmospheric pressure.

Note:
Methane has so many applications due to its low boiling point. It can be used to perform some atmosphere sensitive reactions that should be done in low temperature conditions. At this time in a low temperature bath methane can be filled as at low temperature so many solvents like water will freeze but methane will exist as liquid.