Chemical Thermodynamics: JEE Main 2026 Chemistry question

JEE Main 2026 · 21 Jan, Morning shift · Q74

JEE Main 202621 Jan, Morning shiftChemistryHardChemical Thermodynamics84× since 2002

Use the following data :

\Delta_fH^\ominus

(500 K) / kJ mol

^{-1}

and

S^\ominus

(500 K) / J K

^{-1}

mol

^{-1}

: AB(g): 32, 222;

\mathrm{A_2}

(g): 6, 146;

\mathrm{B_2}

(g):

x

, 280. One mole each of

\mathrm{A_2}

(g) and

\mathrm{B_2}

(g) are taken in a 1 L closed flask and allowed to establish the equilibrium at 500K.

\mathrm{A_2(g)+B_2(g)\rightleftharpoons2AB(g)}

. The value of

x

(in kJ mol

^{-1}

) is ______. (Nearest integer) (Given :

\log K=2.2

R=8.3

J K

^{-1}

mol

^{-1}

)

Your answerType your answer. Integers and decimals are accepted.

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JEE Main 2026 Chemical Thermodynamics Question with Solution (21 Jan Morning shift, Q74) | JEE Arc