JEE Main 20246 Apr, Evening shiftChemistryMediumChemical Thermodynamics84× since 2002For the reaction at 298 K,2 A+B→C,ΔH=400 kJ mol−1298 \mathrm{~K}, 2 \mathrm{~A}+\mathrm{B} \rightarrow \mathrm{C}, \Delta \mathrm{H}=400 \mathrm{~kJ} \mathrm{~mol}^{-1}298 K,2 A+B→C,ΔH=400 kJ mol−1 and ΔS=0.2 kJ mol−1 K−1\Delta S=0.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}ΔS=0.2 kJ mol−1 K−1. The reaction will become spontaneous above __________ K\mathrm{K}K.Your answerType your answer. Integers and decimals are accepted.CheckSkip · show solution
