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Question

For the gas phase reaction, C2H4+H2C2H6 [ΔHo=136.8kJ mol1], is carried out in vessel, the equilibrium concentration of C2H4 can be increased by:

A
increasing the temperature
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B
decreasing the pressure
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C
removing some H2
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D
adding some C2H6
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Solution

The correct options are
A increasing the temperature
B removing some H2
C decreasing the pressure
D adding some C2H6
The given reaction is :-
C2H4+H2C2H6;H0=136.8KJ/mol
(I) This reaction is exothermic reaction, so increase of temperature favours backward reaction and formation of C2H6 is lowered.
(II) High pressure favours the reaction which takes place with decrease in no. of moles. So, an decreasing the pressure, the formation of C2H6 is decreased.
(III) Removing of H2 increases backward reaction rate as per Le Chatelier's principle.
(IV) Adding of C2H6 also decreases the forward reaction as predicted by Le Chatelier's principle.

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