Enthalpy and entropy

The table below shows standard entropies, $S⊖S^\ominus$ .

Substance	$N2O4(g)\text{N}_2\text{O}_4(\text{g})$	$NO2(g)\text{NO}_2(\text{g})$
$mol−1K−1S^\ominus\text{ / J mol}^{-1}\text{K}^{-1}$	304.3	240.1

What is the entropy change, $ΔS⊖\Delta S^\ominus$ , in $mol−1K−1\text{J mol}^{-1}\text{K}^{-1}$ , for the following reaction?

\text{N}_2\text{O}_4(\text{g}) \rightarrow 2\text{NO}_2(\text{g})

$- 175.9$

$- 64.2$

$+ 64.2$

$+ 175.9$

The table below shows standard entropies, $S⊖S^\ominus$ .

Substance	$N2O4(g)\text{N}_2\text{O}_4(\text{g})$	$NO2(g)\text{NO}_2(\text{g})$
$mol−1K−1S^\ominus\text{ / J mol}^{-1}\text{K}^{-1}$	304.3	240.1

What is the entropy change, $ΔS⊖\Delta S^\ominus$ , in $mol−1K−1\text{J mol}^{-1}\text{K}^{-1}$ , for the following reaction?

\text{N}_2\text{O}_4(\text{g}) \rightarrow 2\text{NO}_2(\text{g})

$- 175.9$

$- 64.2$

$+ 64.2$

$+ 175.9$

Enthalpy and entropy Questions