Which of the following takes place as an ice cube cools a drink? (A) A calorie of heat energy is transferred from the ice to the water of the drink.(B) The specific heat of the water in the drink decreases.(C) Molecular collisions in the drink increase.(D) Evaporation of the water in the drink increases.(E) Kinetic energy in the drink decreases.

Heat energy always transfers from a body at a higher temperature to a body at a lower temperature.
Specific heat of a material is the amount of heat energy required to raise a unit temperature of the body which remains constant for a fixed substance.
The speed of evaporation varies with variation in temperature. As the temperature increase, the evaporation rate increases.
When heat is given to a substance, the temperature of the molecules increases due to which the randomness of the molecules increases causing an increased molecular collision.

Now, looking at point 1, option (A) is wrong. This is because ice is at a lower temperature while the cold drink is at a higher temperature. So, heat energy transfers from the water of cold drink to ice.

Looking at point 2, option (B) is wrong.

On addition of ice to the cold drink, the temperature of the cold drink decreases causing the decrease in the kinetic energy of the molecules of water in the cold drink and the molecular collisions. Also, the evaporation of water in drink decreases. So, from points 3 and 4, we can say that options (C) and (D) are wrong and option (E) is right.

Hence, the option (E) is correct.