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## Homework Statement

The reaction is [tex]NH_{4}Cl(s)\rightarrow NH_{3}(g)+HCl(g)[/tex]

[tex]\Delta H^{o}=+176 kJ and \Delta G^{o}=+91.2 kJ[/tex] at 298 K

What is the value of [tex]\Delta G[/tex] at 1000 K?

## Homework Equations

[tex]\Delta G=\Delta H-T\Delta S[/tex]

The same applies if all 'deltas' are standard

## The Attempt at a Solution

Well, I solved for standard change of entropy ([tex]\Delta S^{o}[/tex]) and came up with .284 kJ/K, which is the same when using a table of standard entropies. My problem is, I'm not sure where to go from this to find [tex]\Delta G[/tex], or even a way to link standard values to normal values for these. I tried plugging in the values for standard delta H and delta S with 1000K to find delta G, but something tells me that this is incorrect. Any help would be greatly appreciated!

-Swerting