JEE Main 20236 Apr, Morning shiftChemistryMediumChemical Thermodynamics84× since 2002The value of logK\log \mathrm{K}logK for the reaction A⇌B\mathrm{A} \rightleftharpoons \mathrm{B}A⇌B at 298 K298 \mathrm{~K}298 K is ___________. (Nearest integer) Given: ΔH∘=−54.07 kJ mol−1\Delta \mathrm{H}^{\circ}=-54.07 \mathrm{~kJ} \mathrm{~mol}^{-1}ΔH∘=−54.07 kJ mol−1 ΔS∘=10 J K−1 mol−1\Delta \mathrm{S}^{\circ}=10 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}ΔS∘=10 J K−1 mol−1 (Take 2.303×8.314×298=57052.303 \times 8.314 \times 298=57052.303×8.314×298=5705 )Your answerType your answer. Integers and decimals are accepted.CheckSkip · show solution
