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Chemical Thermodynamics Part 3

Section: Chemistry
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Question : 12 of 22
 
Marks: +1, -0
Use the following data :
Substance‌
∆fH⊖(500K)
kJmol−1
‌
S⊖(500K)
JK−1mol−1
AB(g)32222
A2(g)6146
B2(g)x280

One mole each of A2(g) and B2(g) are taken in a 1 L closed flask and allowed to establish the equilibrium at 500 K .
A2(g)+B2(g)⇌2AB(g) The value of x(inkJmol−1) is ____ . (Nearest integer)
‌ (Given : ‌log‌K=2.2‌‌R=8.3JK−1mol−1‌ ) ‌
[21 Jan 2026 Shift 1]
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