To calculate, I would need to know if the final answer is supposed to be in kJ or in J/K.
Either way, use the Gibb's Formula:
ΔG= ΔH-TΔS
If the final answer is supposed to be in J/K then plug-in your values to the formula and simply solve.
However, if your final answer is supposed to be in kJ, your first step would be to convert ΔS from J/K into kJ.
This is simply done by dividing the given ΔS by 1000 ----> (-301.2/1000).
(we divide by 1000 because by definition that's what a "kilo" is )
New ΔS value= -0.3012 kJ
Now all you have to do is plug-in all the values into the formula.
ΔG= ΔH-TΔS
ΔG= (-144.6 kJ) - 298K(-0.3012kJ)
= -54.84 kJ
Since the ΔG is negative, this means that the reaction is spontaneous.
Hope this helps! :)
