An ice cube at 0.00 ∘C∘C with a mass of 21.5 gg is placed into 500.0 gg of water, initially at 31.0 ∘C∘C, in an insulated container. Part A Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all of the ice has melted?

The temperature of the entire water sample after all of the ice has melted is 31.4 °C

Explanation:

This question relates to the first law of thermodynamics which states that energy can not be created nor destroyed but changes from one form to another

The specific heat capacity of water is 4.2 J/(g °C)

The latent heat of fusion of ice = 333.55 J/g

Mass of the ice = 21.5 g

Mass of the water = 500 g

Initial temperature of water = 31 °C

Therefore

Heat gained by the ice = 21.5 g × 333.55 J/g = 7162.725 J

= 500×4.2×(T-31)

Or T = 31.4 °C

Therefore the temperature of the entire water sample after all of the ice has melted is 31.4 °C

you gotta add the following molecules so we can give u an answer

explanation:

explanation:

0.07 g/cm³

1.37 g/cm³