Question

Consider the reaction: \[ \mathrm{H}_{2}(g)+\mathrm{C}_{2} \mathrm{H}_{4}(g) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g) \] Using standard absolute entropies at \( 298 \mathrm{~K} \), calculate the entropy change for the system when 2.44 moles of \( \mathrm{H}_{2}(\mathrm{~g}) \) react at standard conditions. \begin{tabular}{|c|c|} \hline Substance & \( S^{\circ}\left(\frac{\mathrm{J}}{\mathrm{K} \cdot \mathrm{mol}}\right) \) \\ \hline \( \mathrm{C}_{2} \mathrm{H}_{6}(g) \) & 229.6 \\ \hline \( \mathrm{H}_{2}(g) \) & 130.7 \\ \hline \( \mathrm{C}_{2} \mathrm{H}_{4}(g) \) & 219.6 \\ \hline \end{tabular} \( \Delta S_{\text {system }}^{\curvearrowleft}= \) \( \square \) \( \mathrm{J} / \mathrm{K} \)

          Consider the reaction:
\[
\mathrm{H}_{2}(g)+\mathrm{C}_{2} \mathrm{H}_{4}(g) \rightarrow \mathrm{C}_{2} \mathrm{H}_{6}(g)
\]

Using standard absolute entropies at \( 298 \mathrm{~K} \), calculate the entropy change for the system when 2.44 moles of \( \mathrm{H}_{2}(\mathrm{~g}) \) react at standard conditions.
\begin{tabular}{|c|c|}
\hline Substance & \( S^{\circ}\left(\frac{\mathrm{J}}{\mathrm{K} \cdot \mathrm{mol}}\right) \) \\
\hline \( \mathrm{C}_{2} \mathrm{H}_{6}(g) \) & 229.6 \\
\hline \( \mathrm{H}_{2}(g) \) & 130.7 \\
\hline \( \mathrm{C}_{2} \mathrm{H}_{4}(g) \) & 219.6 \\
\hline
\end{tabular}
\( \Delta S_{\text {system }}^{\curvearrowleft}= \) \( \square \) \( \mathrm{J} / \mathrm{K} \)

Consider the reaction:

H2(g)+C2H4(g) →C2H6(g)

Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.44 moles of H2( g) react at standard conditions.

Substance S^∘((J)/(K·mol))

C2H6(g) 229.6

H2(g) 130.7

C2H4(g) 219.6

Δ Ssystem ^↶= □ J / K

Added by Andrew C.

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