AP Chemistry
9.2 Absolute Entropy and Entropy Change
9.1 Introduction to Entropy
A student heats a sample of pure calcium carbonate, \(\text{CaCO}_3(s)\), in an open crucible, causing it to decompose according to the balanced equation below.
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
Which of the following correctly predicts and explains the sign of the standard entropy change, \(\Delta S^\circ\), for this reaction?
\[ \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \]
Which of the following correctly predicts and explains the sign of the standard entropy change, \(\Delta S^\circ\), for this reaction?
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