A) \[-78\,kJ\]
B) \[-156\,kJ\]
C) \[-1478\,kJ\]
D) \[+1478\,kJ\]
Correct Answer: A
Solution :
\[{{N}_{2}}+3{{H}_{2}}\xrightarrow{{}}2N{{H}_{3}}\]For this reaction, Heat evolved \[=6\times \](\[N-H\]bond energy) \[-\] [3 (\[H-H\]bond energy) + (\[N\equiv N\]) bond energy] = 6 (389) \[-\] [3 (437) + (945)] = 2334 \[-\] (1311 + 945) = 2334 \[-\] 2256 = 78 kJ \[\therefore \] \[\Delta H=-78\,kJ\]You need to login to perform this action.
You will be redirected in
3 sec