(Solved): Consider the reaction: \[ 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \longrightarrow 2 \mathrm{H}_{2}( ...

Consider the reaction: \[ 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \longrightarrow 2 \mathrm{H}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \] Using standard thermodynamic data at \( 298 \mathrm{~K} \), calculate the entropy change for the surroundings when \( \mathbf{2 . 4 6} \) moles of \( \mathrm{H}_{2} \mathrm{O}(\mathrm{I}) \) react at standard conditions. \[ \Delta \mathrm{S}^{\circ} \text { surroundings }= \] Consider the reaction: \[ \mathrm{Fe}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{FeCl}_{2}(s)+\mathrm{H}_{2}(g) \] Using standard thermodynamic data at \( 298 \mathrm{~K} \), calculate the entropy change for the surroundings when \( 2.00 \) moles of \( \mathrm{Fe}(s) \) react at standard conditions. \[ \Delta S_{\text {surroundings }}^{\circ}= \]