Calculate $\Delta S^\circ_{rxn}$ for the hypothetical reaction below. The $S^\circ$ for each species is shown below: $A_2B_2(g) \rightarrow 2A(g) + 2B(g)$ $\begin{array}{|c|c|} \hline S^\circ (J\\/K\\\cdot mol) \\ \hline A_2B_2(g) & 219.17 \\ A(g) & 73.06 \\ B(g) & 78.19 \\ \hline \end{array}$ 83.32 -83.32 -67.93
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We can do this by summing up the individual entropy changes for each species involved in the reaction. ΔS = (2 * ΔS(A)) + (2 * ΔS(B)) - ΔS(AzBz) Show more…
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