For a reaction ΔH:(+3kJ)⋅ΔS=(+10J/K) beyond whichtemperature this reaction will be spontaneous

ΔG=ΔH−TΔS For the spontaneous reaction the ∆ G must be negative.  ΔH=3KJ=+3000JΔS=+10J/K If T=300K⇒ΔG=3000−300×10=0 If T=200K⇒ΔG=3000−200×10=1000J If T=273K⇒ΔG=3000−273×10=270J If T=373KΔG=3000−373×10=−730JHence, beyond 373 temperature the reaction will be spontaneous.