C\(_2\)H\(_4\)(g) + H\(_2\)(g) → C\(_2\)H\(_6\)(g) ΔH = -137kJ mol-1
The reaction represented above is
exothermic
spontaneous
endothermic
in equilibrium
Explanation
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The given reaction is exothermic.
An exothermic reaction releases heat energy to the surroundings, resulting in a negative value for the enthalpy change (ΔH < 0). In this case, the enthalpy change for the reaction is -137 kJ mol-1, which indicates that the reaction releases 137 kJ of heat energy per mole of reactants.
In the given reaction, ethene (C2H4) reacts with hydrogen gas (H2) to form ethane (C2H6), and the reaction releases heat in the process. This means that the products have a lower energy content than the reactants, and the excess energy is released in the form of heat.
Therefore, the answer is (A) exothermic.
