Question

An insulated beaker with negligible mass contains liquid water with a mass of 0.310 kg and a temperature of 74.1 ?C .

How much ice at a temperature of -10.2 ?C must be dropped into the water so that the final temperature of the system will be 37.0 ?C ?

Take the specific heat of liquid water to be 4190 J/kg?K , the specific heat of ice to be 2100 J/kg?K , and the heat of fusion for water to be 3.34×10⁵ J/kg .

Answer 1

Let 'm' amount of ice was taken.

Heat gained by ice to come from -10.2 degrees to 0 degrees is

Now, this ice is converted into water at the same temperature of 0 degrees Celsius by latent heat process.

In the mean time, heat lost by water with mass 0.310 kg to come from 74.1 degrees to 37.0 degrees is

Now, using the principle of calorimetry, according to which,

Heat lost by water = Heat gained by ice