Calculate the standard entropy change of the system in the given below reaction using the standard molar entropy values given here. (Values for  

${\mathrm{S}}^{⊝}\mathrm{in} \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1})$.

Given:

$$\begin{gathered} \mathrm{Fe}\left(\mathrm{s}\right)=27.30 \\ \mathrm{MgO}\left(\mathrm{s}\right)=26.90 \\ \mathrm{Mg}\left(\mathrm{s}\right)=32.70 \\ {\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)=87.40 \\ 3\mathrm{Mg}\left(\mathrm{s}\right)+{\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)\to 3\mathrm{MgO}\left(\mathrm{s}\right)+2\mathrm{Fe}\left(\mathrm{s}\right) \end{gathered}$$

Calculate the entropy change of the surrounding in the following reaction. Assume that the value of $∆\mathrm{H}$ does not change with temperature.

$\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{CO}}_2\left(\mathrm{g}\right) ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=-393.5 \mathrm{kJ} {\mathrm{mol}}^{-1}, \mathrm{carried} \mathrm{out} \mathrm{at} 0^{°}\mathrm{C}$.

Calculate the entropy change of the surrounding in the following reaction. Assume that the value of $∆\mathrm{H}$ does not change with temperature.

$2\mathrm{C}\left(\mathrm{s}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\to {\mathrm{C}}_2{\mathrm{N}}_2\left(\mathrm{g}\right) ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=+307.9 \mathrm{kJ} {\mathrm{mol}}^{-1}, \mathrm{carried} \mathrm{out} \mathrm{at} {300}^{°}\mathrm{C}$.

Calculate the entropy change of the surrounding in the following reaction. Assume that the value of $∆\mathrm{H}$ does not change with temperature.

${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{F}}_2\left(\mathrm{g}\right)\to 2\mathrm{HF}\left(\mathrm{g}\right) ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=-271.1 \mathrm{kJ} {\mathrm{mol}}^{-1}, \mathrm{carried} \mathrm{out} \mathrm{at} \mathrm{standard} \mathrm{temperature}.$

Calculate the entropy change of the surrounding in the following reaction. Assume that the value of $∆\mathrm{H}$ does not change with temperature.

$\mathrm{Si}\left(\mathrm{s}\right)+2{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{SiH}}_4\left(\mathrm{g}\right) ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=+34.30 \mathrm{kJ} {\mathrm{mol}}^{-1}, \mathrm{carried} \mathrm{out} \mathrm{at} -3^{°}\mathrm{C}.$

Calculate the total entropy change in each of the following reactions using the standard molar entropy values given here.

Values for:

 $$\begin{gathered} {\mathrm{S}}^{⊝} \mathrm{in} \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}. \\ \mathrm{Given}: \\ \mathrm{S}\left(\mathrm{s}\right)=31.80 \\ {\mathrm{H}}_2\left(\mathrm{g}\right)=130.6 \\ {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right)=205.7 \\ \mathrm{S}\left(\mathrm{s}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\to {\mathrm{H}}_2\mathrm{S}\left(\mathrm{g}\right); ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=-20.6 \mathrm{kJ} {\mathrm{mol}}^{-1}. \end{gathered}$$

Calculate the total entropy change in each of the following reactions using the standard molar entropy values given here.

Values for

 $$\begin{gathered} {\mathrm{S}}^{⊝} \mathrm{in} \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}. \\ \mathrm{Given}: \\ \mathrm{C}\left(\mathrm{graphite}\right)=5.700 \\ {\mathrm{N}}_2\left(\mathrm{g}\right)=191.6 \\ {\mathrm{C}}_2{\mathrm{N}}_2\left(\mathrm{g}\right)=242.1 \\ 2\mathrm{C}\left(\mathrm{graphite}\right)+{\mathrm{N}}_2\left(\mathrm{g}\right)\to {\mathrm{C}}_2{\mathrm{N}}_2\left(\mathrm{g}\right); ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=+307.9 \mathrm{kJ} {\mathrm{mol}}^{-1}. \end{gathered}$$

Calculate the total entropy change in each of the following reactions using the standard molar entropy values given here.

Values for

$$\begin{gathered} {\mathrm{S}}^{⊝} \mathrm{in} \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}. \\ \mathrm{Given}: \\ \mathrm{P}\left(\mathrm{s}\right)=41.10 \\ {\mathrm{O}}_2\left(\mathrm{g}\right)=205.0 \\ {\mathrm{P}}_4{\mathrm{O}}_{10}\left(\mathrm{s}\right)=228.9 \\ 4\mathrm{P}\left(\mathrm{s}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\to {\mathrm{P}}_4{\mathrm{O}}_{10}\left(\mathrm{s}\right); ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=-2984.0 \mathrm{kJ} {\mathrm{mol}}^{-1}. \end{gathered}$$

Calculate the total entropy change in each of the following reactions using the standard molar entropy values given here.

Values for

$$\begin{gathered} {\mathrm{S}}^{⊝} \mathrm{in} \mathrm{J} {\mathrm{K}}^{-1} {\mathrm{mol}}^{-1}. \\ \mathrm{Given}: \\ {\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)=269.9 \\ {\mathrm{O}}_2\left(\mathrm{g}\right)=205.0 \\ {\mathrm{CO}}_2\left(\mathrm{g}\right)=213.6 \\ {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)=69.90 \\ {\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\to 3{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right); ∆{\mathrm{H}}_{\mathrm{reaction}}^{⊝}=-2219.2 \mathrm{kJ} {\mathrm{mol}}^{-1}. \end{gathered}$$