AP Chemistry
9.2 Absolute Entropy and Entropy Change
The Haber process for the industrial synthesis of ammonia is represented by the following balanced chemical equation:
\[ \text{N}_2\text{(g)} + 3\,\text{H}_2\text{(g)} \rightarrow 2\,\text{NH}_3\text{(g)} \]
The absolute standard molar entropy values, \(S^\circ\), for the substances involved at \(298\text{ K}\) are given in the table below.
Based on the data in the table, what is the value of \(\Delta S^\circ_{\text{rxn}}\) for the reaction at \(298\text{ K}\)?
\[ \text{N}_2\text{(g)} + 3\,\text{H}_2\text{(g)} \rightarrow 2\,\text{NH}_3\text{(g)} \]
The absolute standard molar entropy values, \(S^\circ\), for the substances involved at \(298\text{ K}\) are given in the table below.
| Substance | \(S^\circ\ (\text{J}/(\text{mol}\cdot\text{K}))\) |
|---|---|
| \(\text{N}_2\text{(g)}\) | \(192\) |
| \(\text{H}_2\text{(g)}\) | \(131\) |
| \(\text{NH}_3\text{(g)}\) | \(193\) |
Based on the data in the table, what is the value of \(\Delta S^\circ_{\text{rxn}}\) for the reaction at \(298\text{ K}\)?
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