Question

A fifty gram block of ice with an initial temperature of –25°C is warmed continually in a sealed container until it becomes fifty grams of water vapor at 125°C. Which of the following transitions requires absorption of the greatest amount of heat energy?

Group of answer choices

warming up the water vapor from 100°C to 125°C

warming up the water from 0°C to 100°C

boiling the water at its boiling point

warming up the ice from –25°C to 0°C

melting the ice at its melting point

Answer 1

The transition that requires the absorption of the greatest amount of heat energy is boiling the water at its boiling point.

Boiling water at its boiling point requires a significant amount of energy because it involves the phase transition from a liquid to a gas. During this transition, the water absorbs heat energy to break the intermolecular bonds and convert from a liquid state to a gaseous state. This process requires a large amount of energy compared to other transitions such as warming up the water or ice, where the temperature changes within a specific phase.

Therefore, out of the given options, boiling the water at its boiling point requires the absorption of the greatest amount of heat energy.

Step-by-step explanation: