If 1.10 g of steam at 100.0 °c condenses into 38.5 g of water, initially at 27.0 °c, in an insulated container, what is the final temperature of the entire water sample? assume no heat is lost to the surroundings.

Temperature = 44.02°C

Explanation:

Insulated container indicates no heat loss to the surroundings.

The specific heat capacity of a substance is a physical property of matter. It is defined as the amount of heat that is to be supplied to a unit mass of the material to produce a unit change in its temperature.

The SI unit of specific heat is joule per kelvin and kilogram, J/(K kg).

Now,

Specific heat for water is 4.1813 Jg⁻¹K⁻¹.

Latent heat of vaporization of water is 2257 Jg⁻¹.

Energy lost by steam in it's process of conversion to water, is the energy acquired by water resulting in an increase in it's temperature.

Q= Heat transferred

m= mass of the substance

T= temperature

Also,

L= Latent heat of fusion/ vaporization ( during phase change)

Now applying the above equations to the problem:

Temperature = 44.02°C

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.