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IF the bond energies of H – H , Br – Br and H – Br are 433 , 192 and 364 kJ mol⁻¹ respectively, the ΔH° for the reaction
H₂(g) + Br₂(g) → 2HBr(g) is
Options
(a) -261 kJ
(b) ⁺103 kJ
(c) ⁺261 kJ
(d) -103 kJ
Correct Answer:
-103 kJ
Explanation:
H – H + Br – Br → 2H – Br,
(433) + (192) (2 x 364)
=625 =728
(Energyabsorbed) (Energy released)
Net energy released = 728 – 625 = 103 KJ. i.e. ΔH = -103 KJ.
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Topics: Thermodynamics
(179)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Which is difference between melting and boiling point of zero group elements
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- The number of optical isomers formed by hydrogenation of the compound (CH₃)₂C=CHCH₃
- Which of the following compounds is the strongest base
Topics: Thermodynamics (179)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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