Question

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion, 4Al(s) + 3O2(g) ? 2Al2O3(s). ?G° for this reaction is _ and this reaction is _. ?G°f (kJ/mol) Al(s) 0 O2(g) 0 Al2O3(s) -1576.4 Select one: a. -3152.8 kJ/mol, nonspontaneous b. 3152.8 kJ/mol, spontaneous c. 3152.8 kJ/mol, nonspontaneous d. 0 kJ/mol; at equilibrium e. -3152.8 kJ/mol, spontaneous

          Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further
corrosion, 4Al(s) + 3O2(g) ? 2Al2O3(s).
?G° for this reaction is _________ and this reaction is _________.
?G°f (kJ/mol)
Al(s) 0
O2(g) 0
Al2O3(s) -1576.4
Select one:
a. -3152.8 kJ/mol, nonspontaneous
b. 3152.8 kJ/mol, spontaneous
c. 3152.8 kJ/mol, nonspontaneous
d. 0 kJ/mol; at equilibrium
e. -3152.8 kJ/mol, spontaneous

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further
corrosion, 4Al(s) + 3O2(g) ? 2Al2O3(s).
?G° for this reaction is and this reaction is .
?G°f (kJ/mol)
Al(s) 0
O2(g) 0
Al2O3(s) -1576.4
Select one:
a. -3152.8 kJ/mol, nonspontaneous
b. 3152.8 kJ/mol, spontaneous
c. 3152.8 kJ/mol, nonspontaneous
d. 0 kJ/mol; at equilibrium
e. -3152.8 kJ/mol, spontaneous

Added by Luz H.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

09/01/2023

Step 1

4 \,\text{kJ/mol}$ Now, we can calculate the Gibbs free energy change for the reaction using the equation: $\Delta G^\circ = \sum \Delta G_f^\circ(\text{products}) - \sum \Delta G_f^\circ(\text{reactants})$ For the given reaction: Show more…

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Aluminum forms a layer of aluminum oxide when exposed to air, which protects the bulk metal from further corrosion. The balanced chemical equation for this reaction is 4Al(s) + 3O2(g) -> 2Al2O3(s). The ΔG for this reaction is -1576.4 kJ/mol.