For a particular reaction, δh = -144.6 kj and δs = -301.2 j/k. calculate δg for this reaction at 298 k.

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! :)

Is a logical series of steps