Consider the reaction X Y at 300 K. If Δ H^θ and K are 28.40 kJ mol ⁻¹ and 1.8×10⁻⁷ at the same temperature, then the magnitude of Δ S^θ for the reaction in J K ⁻¹ mol ⁻¹ is _ _ _ _. (Nearest integer) (Given: R = 8.3 J K ⁻¹ mol ⁻¹, ln 10 = 2.3, log 3 = 0.48, log 2 = 0.30)

Chemical Thermodynamics: JEE Main 2026 Chemistry question

JEE Main 2026 · 6 Apr, Morning shift · Q75

JEE Main 20266 Apr, Morning shiftChemistryMediumChemical Thermodynamics84× since 2002

Consider the reaction

\mathrm{X\rightleftharpoons Y}

at 300 K. If

\Delta H^\theta

and K are 28.40 kJ mol

^{-1}

and

1.8\times10^{-7}

at the same temperature, then the magnitude of

\Delta S^\theta

for the reaction in J K

^{-1}

mol

^{-1}

is________. (Nearest integer) (Given : R = 8.3 J K

^{-1}

mol

^{-1}

, ln 10 = 2.3, log 3 = 0.48, log 2 = 0.30)

Your answerType your answer. Integers and decimals are accepted.

JEE Main 2026 Chemical Thermodynamics Question with Solution (6 Apr Morning shift, Q75) | JEE Arc