On a cold day, 24500 J of heat leaks out of a house. The...

On a cold day, 24500 $\mathrm{J}$ of heat leaks out of a house. The inside temperature is $21^{\circ} \mathrm{C},$ and the outside temperature is $-15^{\circ} \mathrm{C}$ . What is the increase in the entropy of the universe that this heat loss produces?

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Key Concepts

Temperature Conversion to Kelvin

Temperatures must be converted to an absolute scale, Kelvin, when used in thermodynamic formulas because these formulas require an absolute temperature scale where zero represents the absence of thermal energy. This ensures accurate calculation of entropy changes.

Heat Transfer

Heat transfer involves the flow of thermal energy from one system or body to another due to a temperature difference. In problems where heat is exchanged between two reservoirs at different temperatures, the individual changes in entropy must be calculated using the appropriate temperatures, reflecting the irreversible nature of real heat transfer.

Second Law of Thermodynamics

The second law states that in an isolated system, the total entropy can never decrease over time; it either remains constant in ideal reversible processes or increases in real, irreversible processes. This law underpins the concept that heat naturally flows from hotter to colder bodies, leading to an overall increase in entropy.

Entropy

Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the number of ways the energy in a system can be distributed, and changes in entropy are used to determine the direction of spontaneous processes.

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