This example shows that adding a given amount of energy to a system increases its entropy, but adding the same amount of energy to another system at higher temperature results in a smaller increase in entropy. This is because the change in entropy is inversely proportional to the temperature.

Question

If the same amount of energy were used as it takes to melt ice at $0C$ to water at $0C,$ compare the entropy changes for melting ice, silver, and lead, from smallest to largest. $($Select all that app

Melting the silver involves the largest entropy change.

Melting the ice involves the smallest entropy change.

Melting the ice involves the largest entropy change.

Melting the lead involves the smallest entropy change.

Melting the lead involves the largest entropy change.

Melting the silver involves the smallest entropy change.