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

the answer is either b or c

i would say b

explanation:

but i think i would need more information than that