A) 8 kJ
B) 88 kJ
C) - 16 kJ
D) 196 kJ
Correct Answer: D
Solution :
\[2{{N}_{2}}{{O}_{(g)}}+{{O}_{2(g)}}\to 4N{{O}_{(g)}}\] \[\Delta {{H}_{1}}(kJ):\] \[2\times 82\] 0\[4\times 90\] \[\Delta {{H}_{\operatorname{Re}action}}=\Sigma \Delta {{H}_{f(Product)}}-\Sigma \Delta {{H}_{f(Reactant)}}\] \[=4\times 90-2\times 92=360-164=196kJ\]You need to login to perform this action.
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