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

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

A. exothermic
B. spontaneous
C. endothermic
D. in equilibrium

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

Correct Answer: Option A

Explanation

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