2 Al (s) + 3 Cl_{2} (g) → 2 AlCl_{3} (s) ΔH° = -1408.4 kJ

a) **ΔS _{sys} **

$\overline{){\mathbf{\u2206}}{{\mathbf{S}}}_{{\mathbf{sys}}}{\mathbf{=}}{\sum _{}}{\mathbf{\u2206}}{\mathbf{S}}{{\mathbf{\xb0}}}_{{\mathbf{p}}}{\mathbf{-}}{\sum _{}}{\mathbf{\u2206}}{\mathbf{S}}{{\mathbf{\xb0}}}_{{\mathbf{r}}}}$

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

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.

ΔS_{sys} =

ΔS_{surr} =

ΔS_{univ} =

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Entropy concept. You can view video lessons to learn Entropy. Or if you need more Entropy practice, you can also practice Entropy practice problems.