Change in Entropy:

$\overline{){\mathbf{\u2206}}{\mathbf{S}}{\mathbf{=}}\frac{\mathbf{\u2206}\mathbf{Q}}{\mathbf{T}}}$

a. An object at 20°C absorbs 25.0 kJ of heat. What is the change in entropy ΔS of the object? Express your answer numerically in joules per kelvin.

b. An object at 500 K dissipates 25.0 kJ of heat into the surroundings. What is the change in entropy Δ*S* of the object? Assume that the temperature of the object does not change appreciably in the process. Express your answer numerically in joules per kelvin.

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