Final answer:
The entropy change of a 208 K hot reservoir after removing 229 J of heat is -1.101 J/K. The negative sign indicates that the entropy of the hot reservoir decreases.
Step-by-step explanation:
To calculate the entropy change in a system when a certain amount of heat is removed, you can use the formula ΔS = Q/T, where ΔS is the entropy change in joules per kelvin (J/K), Q is the heat transferred in joules (J), and T is the temperature of the system in kelvin (K). If 229 J of heat is removed from a 208 K hot reservoir, the entropy change (ΔS) would be calculated as follows:
ΔS = Q/T
ΔS = -229 J / 208 K
ΔS = -1.101 J/K
The negative sign indicates that the entropy of the hot reservoir has decreased. This is consistent with the second law of thermodynamics, which states that the entropy of an isolated system can either increase or remain constant; a decrease in entropy is associated with a transfer of entropy to the surroundings.