The heat required to raise the temperature of a substance by 
is represented by
where m stands for the mass of the substance and
indicates the specific heat of the substance. In this situation, we possess 
and 
, the specific heat of water.
Consequently, we can ascertain the temperature rise:
Initially, the water's temperature was
, so the end temperature should be
Thus, the water is expected to be vapor by now.
However, to give a more accurate statement, during the liquid to vapor transition, the heat added to the system is used to break molecular bonds instead of raising the system's temperature. The heat necessary for the phase change from liquid to vapor is expressed as
where
denotes the latent heat of vaporization for water.
Nevertheless, the initial heat input of 50 KJ is less than this requirement, indicating there isn't sufficient heat to finish the liquid-vapor transition. Therefore, the water will remain in the liquid-vapor change phase at a temperature of
(the temperature at which the phase change begins)
where m stands for the mass of the substance and
Consequently, we can ascertain the temperature rise
Initially, the water's temperature was
Thus, the water is expected to be vapor by now.
However, to give a more accurate statement, during the liquid to vapor transition, the heat added to the system is used to break molecular bonds instead of raising the system's temperature. The heat necessary for the phase change from liquid to vapor is expressed as
where
Nevertheless, the initial heat input of 50 KJ is less than this requirement, indicating there isn't sufficient heat to finish the liquid-vapor transition. Therefore, the water will remain in the liquid-vapor change phase at a temperature of