A) \[{{N}_{2}}(g)+{{O}_{2}}(g)+180.8kJ\to 2NO(g)\]
B) \[C(\text{graphite})+2S(s)\to C{{S}_{2}}(l)-91.9kJ\]
C) \[{{N}_{2}}(g)+3{{H}_{2}}(g)-92kJ\to 2N{{H}_{3}}(g)\]
D) \[\text{C(g)+}{{\text{H}}_{\text{2}}}\text{O(g)}\to \text{CO(g)+}{{\text{H}}_{\text{2}}}\text{(g)-131}\text{.1kJ}\]
Correct Answer: C
Solution :
The reactions in which products has lesser energy than reactants, the energy is released in the reaction and such reactions are known as exothermic reactions, e.g. \[{{N}_{2}}+3{{H}_{2}}\to 2N{{H}_{3}}+\text{92 kJ}\] In this equation energy is released. So, it is an example of exothermic reaction.
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