A chemical reaction's spontaneity refers to the reaction's ability to proceed without energetic input. In simple words, if a reaction is spontaneous at a given temperature, then it will not require energy to proceed.
If it's not spontaneous at a given temperature, then it will require energy to proceed.
Your bread and butter when it comes to assessing a reaction's spontaneity is this equation
#color(blue)(DeltaG = DeltaH - T * DeltaS)" "#, where
In order for a reaction to be spontaneous, you need
In your case, a positive enthalpy change of reaction and a negative entropy change of reaction will always, irrespective of the temperature at which the reaction takes place, result in
Plug in your values to get the actual value for
#DeltaG = "147 kJ" - (273.15 + 149) color(red)(cancel(color(black)("K"))) * (-67.0)"J"/color(red)(cancel(color(black)("K")))#
#DeltaG = "147 kJ" + overbrace("28,284.05 J")^(color(purple)("convert to kJ"))#
#DeltaG = "147 kJ" + "28.284 kJ" = color(green)(+"175 kJ")#
The answer is rounded to three sig figs.