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[tex]\Delta H_{f}\circ[/tex]=-1670kJ/mol for [tex]Al_{2}O_{3}[/tex]
What is [tex]\Delta H_{rxn}\circ[/tex] for
[tex]2Al_{2}O_{3}(s)\rightarrow4Al+3O_{2}(g)[/tex]
So clearly we simply multiply -1670*2=-3340kJ/mol.
The answer is actually POSITIVE 3340kJ/mol!
Can someone please explain to me how this reasoning works?
Thank you!
What is [tex]\Delta H_{rxn}\circ[/tex] for
[tex]2Al_{2}O_{3}(s)\rightarrow4Al+3O_{2}(g)[/tex]
So clearly we simply multiply -1670*2=-3340kJ/mol.
The answer is actually POSITIVE 3340kJ/mol!
Can someone please explain to me how this reasoning works?
Thank you!