Question

Consider the reaction: \[ 4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{Cl}_{2}(g) \] Using standard absolute entropies at \( 298 \mathrm{~K} \), calculate the entropy change for the system when 2.17 moles of \( \mathrm{HCl}(g) \) react at standard conditions. \begin{tabular}{|c|c|} \hline Substance & \( S^{\circ}(\mathrm{J} / \mathrm{K} \) mol \( ) \) \\ \hline \( \mathrm{HCl}(g) \) & 186.9 \\ \hline \( \mathrm{O}_{2}(g) \) & 205.1 \\ \hline \( \mathrm{H}_{2} \mathrm{O}(g) \) & 188.8 \\ \hline \( \mathrm{Cl}_{2}(g) \) & 223.1 \\ \hline \end{tabular} \( \Delta S_{\text {system }}^{\circ}= \) \( \square \) \( \mathrm{J} / \mathrm{K} \)

          Consider the reaction:
\[
4 \mathrm{HCl}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{Cl}_{2}(g)
\]

Using standard absolute entropies at \( 298 \mathrm{~K} \), calculate the entropy change for the system when 2.17 moles of \( \mathrm{HCl}(g) \) react at standard conditions.
\begin{tabular}{|c|c|}
\hline Substance & \( S^{\circ}(\mathrm{J} / \mathrm{K} \) mol \( ) \) \\
\hline \( \mathrm{HCl}(g) \) & 186.9 \\
\hline \( \mathrm{O}_{2}(g) \) & 205.1 \\
\hline \( \mathrm{H}_{2} \mathrm{O}(g) \) & 188.8 \\
\hline \( \mathrm{Cl}_{2}(g) \) & 223.1 \\
\hline
\end{tabular}
\( \Delta S_{\text {system }}^{\circ}= \) \( \square \) \( \mathrm{J} / \mathrm{K} \)

Consider the reaction:

4 HCl(g)+O2(g) → 2 H2O(g)+2 Cl2(g)

Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.17 moles of HCl(g) react at standard conditions.

Substance S^∘(J / K mol )

HCl(g) 186.9

O2(g) 205.1

H2O(g) 188.8

Cl2(g) 223.1

Δ Ssystem ^∘= □ J / K

Added by Andrew C.

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