C\(_2\)H\(_4\)(g) + H\(_2\)(g) → C\(_2\)H\(_6\)(g)  ΔH = -137kJ mol-1 The reaction represented above is

Chemistry JAMB 2007

C\(_2\)H\(_4\)(g) + H\(_2\)(g) → C\(_2\)H\(_6\)(g)  ΔH = -137kJ mol-1
The reaction represented above is

  • exothermic checkmark
  • spontaneous
  • endothermic
  • in equilibrium

The correct answer is: A

Explanation

Since ΔH has a negative value, it implies an exothermic reaction, which means a lot of heat is being liberated or evolved from the system to the environment.

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