A 1.0-kg chunk of ice at 0 $\degree$C melts,absorbing 80 000 cal of heat in the process.Which of the following best describes what happens to this system?

Question

Quizplus · Accepted Answer

During the process of melting, the ice absorbs heat from the surroundings which leads to an increase in the entropy of the system (ice and surroundings). The transformation from solid to liquid represents an increase in disorder and randomness, resulting in higher entropy. Therefore, choice A is the best option as it describes the system's increased entropy.

A 10-Kg Chunk of Ice at 0 °\degree° C Melts,absorbing 80 000 Cal of Heat in the Process

A 10-Kg Chunk of Ice at 0 $\degree$ C Melts,absorbing 80 000 Cal of Heat in the Process