For the following reaction, suggest whether the entropy of the reactants or the products will be greater or whether it is difficult to decide.

Explain your answer.

$2\mathrm{K}\left(\mathrm{s}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)\to 2\mathrm{KOH}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

For the following reaction, suggest whether the entropy of the reactants or the products will be greater or whether it is difficult to decide.

Explain your answer.

${\mathrm{MgCO}}_3\left(\mathrm{s}\right)\to \mathrm{MgO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

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:

$$\begin{gathered} {\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{l}\right)=109.6 \\ {\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)=69.90 \\ {\mathrm{O}}_2\left(\mathrm{g}\right)=205.0 \end{gathered}$$

$2{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{l}\right)\to 2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$

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:

$$\begin{gathered} {\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)=151.1 \\ {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)=219.7 \\ {\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)=69.90 \\ {\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right) \end{gathered}$$

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:

$$\begin{gathered} \mathrm{MgO}\left(\mathrm{s}\right)=26.90 \\ {\mathrm{O}}_2\left(\mathrm{g}\right)=205.0 \\ \mathrm{Mg}\left(\mathrm{s}\right)=32.70 \\ 2\mathrm{Mg}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\to 2\mathrm{MgO}\left(\mathrm{s}\right) \end{gathered}$$

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:

$$\begin{gathered} \mathrm{NaCl}\left(\mathrm{s}\right)=72.10 \\ {\mathrm{Cl}}_2\left(\mathrm{g}\right)=165.0 \\ \mathrm{Na}\left(\mathrm{s}\right)=51.20 \\ 2\mathrm{Na}\left(\mathrm{s}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)\to 2\mathrm{NaCl}\left(\mathrm{s}\right) \end{gathered}$$

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.

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