For the gaseous reaction, C 2 H 4 + H 2 ⇌ C 2 H 6 , ∆ H = - 130 k J m o l - 1 carried in a closed vessel, the equilibrium concentration of the C 2 H 6 can definitely be increased by

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According to Le-Chatelier's principle exothermic reactions are favourable at low pressure. The reaction in which number of moles decreases are favourable at high pressure or low volume.

$C_{2} H_{4} + H_{2} ⇌ C_{2} H_{6}, ∆ H = - 130 k J m o l^{- 1}$

$∵$ The reaction is exothermic and number of moles of reactants are decreasing.

$∵$ The reaction rate is increased by decreasing temperature and increasing pressure.

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