The temperature of 1.94 kg of water is 34 °c. to cool the water, ice at 0°c is added to it. the desired final temperature of the water is 11 °c. the latent heat of fusion for water is 33.5 × 10^4 j/kg, and the specific heat capacity of water is 4186 j/(kg·c°). ignoring the container and any heat lost or gained to or from the surroundings, determine how much mass m of ice should be added?

0.058 kg or 58 g

Explanation:

The amount of heat energy required to cool 1.94 kg of water from 34 Celcius to 11 Celcius degrees is:

where m = 1.94 kg is the water mass, c = 4186 J/kg.C is water specific heat and

Hence H = 1.94 * 4186 * 23 = 186779.32  J

The required mass of ice to absorb this amount of heat would be

freezing

deposition

condensation

explanation;

melting also called fusion is the process where solid becomes liquid, sublimation is the process where solid becomes gaseous without first changing to liquid, deposition involves change from gaseous to solid state, freezing involves change from liquid to solid, boiling or evaporation involves change of liquid to gaseous state, while condensation is the change from gaseous state to liquid state.

endothermic reactions involves absorption of heat from the surroundings or the environment while exothermic reactions involves loss of heat energy to the surroundings.

in this case, sublimation, evaporation and melting are endothermic reactions (gain energy from the environment) while, freezing, deposition and condensation are exothermic (loss of energy to the surroundings) reactions.

c. newton's third law of motion