For the gas phase reaction, C2H4(g)+H2(g)⇌C2H6(g);△Ho=−136.8kJmol−1 carried out in a vessel, the equilibrium concentration of C2H4 can be increased by:
Increasing the temperature
Decreasing the pressure
Removing some H2
Adding some C2H6
The correct options are A Increasing the temperature B Decreasing the pressure C Removing some H2 D Adding some C2H6 a. As the reaction is exothermic, the temperature reaction will shift in a backward direction, i.e., concentration of C2H4 will increase.
b. The reaction is carried out in the gas phase, hence on decreasing the pressure the reaction will shift in the direction where there are more number of moles. Hence, reaction will shift on the reactant's side.
c. Removing the reactant, H2 will shift the equilibrium to the backward direction and hence concentration of C2H4 will increase.
d. Adding the product C2H6 will shift the equilibrium to the backward direction and hence concentration of C2H4 will increase.