Thermodynamics Homework Question.?

Question

For the gaseous reaction of xenon and fluorine to form xenon hexaflouride:

Calculate ΔS° at 298 K (ΔH = -402.0 kJ/mol and ΔG° = -280.0 kJ/mol).
-and-
Assuming ΔS° and ΔH change little with temperature, calculate ΔG° at 783.0 K.

Thanks so much for the help... allnighters are killing me for finals! ><

if someone could just help me setup the balanced equation... that's where I'm first getting stuck. I can probably figure it out from there because right now I can't determine number of moles.

Answer 1

Balanced reaction:
Xe + 3*F2--------XeF6

You donot need to consider the moles since the data given is of the whole reaction.

Writing delta as 'd'

dG=dH-T*dS
dS=(dH-dG)/T

dS=(-402+280)/298 = -0.4094 kJ/mol

---------------------------------------------------
dG=-402+783*0.4094
= -81.443kJ/mol

Answer 2

there is no need for balanced equation

formula is:
ΔG= ΔH - T ΔS
so
-280=-402-298[ΔS°]
calculate[ΔS°]

equation is:
Xe +3F2=XeF6

Answer 3

Balanced reaction:
Xe + 3*F2--------XeF6

writing delta as d

dG=dH-T*dS
dS=(dH-dG)/T

dH=