If a reaction is not spontaneous at any temperature, what is true of the reaction?

it has a positive enthalpy and positive entropy change.
it has a positive enthalpy and negative entropy change.
it has a negative enthalpy and positive entropy change.
it has a negative enthalpy and negative entropy change.

A reaction that is not spontaneous has a positive ΔG (positive Gibbs free energy) and since it said that it is non spontaneous at every temperature we know that at every temperature ΔG is positive.

Using that information we then use the equation ΔG=ΔH-TΔS where T represents temperature, ΔH represents change in enthalpy, and ΔS represents change in entropy and figure out which condition produces a positive ΔG at every temperature.  

ΔG is always positive when ΔH is positive and ΔS is negative which means that a reaction is non spontaneous at any temperature when the change in enthalpy is positive and change in entropy is negative.

This equation also shows the following:
a reaction is always spontaneous when ΔS is positive and ΔH is negative

a reaction is spontaneous at low temperatures when ΔS is negative and ΔH is negative

a reaction is spontaneous at high temperatures when ΔS is positive and ΔH is positive 

I hope this helps.  Let me know if anything is unclear.