# Problem: Consider the following reactions at 298 K:2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s) ΔH° = -1408.4 kJCalculate the following quantities. Find standard entropy values here.ΔSsys =ΔSsurr =ΔSuniv =

###### FREE Expert Solution

2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s) ΔH° = -1408.4 kJ

a) ΔSsys

$\overline{){\mathbf{∆}}{{\mathbf{S}}}_{{\mathbf{sys}}}{\mathbf{=}}\sum _{}{\mathbf{∆}}{\mathbf{S}}{{\mathbf{°}}}_{{\mathbf{p}}}{\mathbf{-}}\sum _{}{\mathbf{∆}}{\mathbf{S}}{{\mathbf{°}}}_{{\mathbf{r}}}}$

Note that we need to multiply each S˚ by the stoichiometric coefficient since S˚ is in J/mol • K.

Get ΔS° for each species from table:

• ΔS°Al(s) = 28.3 J/mol•K
• ΔS°Cl2(g) = 223.07 J/mol•K
• ΔS°AlCl3(g) = 110.67 J/mol•K

87% (128 ratings) ###### Problem Details

Consider the following reactions at 298 K:
2 Al (s) + 3 Cl2 (g) → 2 AlCl3 (s) ΔH° = -1408.4 kJ

Calculate the following quantities. Find standard entropy values here.
ΔSsys =
ΔSsurr =
ΔSuniv =

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