## Related questions with answers

Use tabulated thermodynamic data to calculate the standard entropy change of each of the reactions listed below.

(a) $\mathrm{Fe}(\mathrm{s})+2 \mathrm{HCl}(\mathrm{g}) \rightarrow \mathrm{FeCl}_2$ (s) $+\mathrm{H}_2(\mathrm{~g})$

(b) $3 \mathrm{NO}_2(\mathrm{~g})+\mathrm{H}_2 \mathrm{O}(\ell) \rightarrow 2 \mathrm{HNO}_3(\ell)+\mathrm{NO}(\mathrm{g})$

(c) $2 \mathrm{~K}(\mathrm{~s})+\mathrm{Cl}_2(\mathrm{~g}) \rightarrow 2 \mathrm{KCl}(\mathrm{s})$

(d) $\mathrm{Cl}_2(\mathrm{~g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow 2 \mathrm{NOCl}(\mathrm{g})$

(e) $\mathrm{SiCl}_4(\mathrm{~g}) \rightarrow \mathrm{Si}(\mathrm{s})+2 \mathrm{Cl}_2(\mathrm{~g})$

Solution

VerifiedFirst we should look up values for standard molar entropy and use them in the equation below.

$\Delta S^{\circ} = \Sigma_{i} v_{i} S^{\circ} ( product)_{i} - \Sigma_{j} v_{j} S^{\circ} ( reactant)_{j}$

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