Question

For the gas phase reaction
$C_2{H}_4+H_2\rightleftharpoons C_2{H}_6(\Delta H=-32.7kcal)$
carried out in a vessel, the equilibrium concentration of $C_2{H}_4$ can be increased by :

• A. increasing the temperature
• B. decreasing the pressure
• C. removing some $H_2$
• D. adding some $C_2{H}_6$

Answer 1

Answer: (A), (B), (C), (D)

The correct options are
A increasing the temperature
B decreasing the pressure
C removing some $H_2$
D adding some $C_2{H}_6$

According to Le-Chatlier's principle- Any change in the equilibrium will move the reaction in the direction where the effect of the change will be finished.

(i) for an exothermic reaction when Temp. increases, equilibrium constant decreases, and the reaction will move backward.

(ii)Decreasing the pressure will move the direction where mols are more.

(iii)Removal of $H_2$ will move the reaction in a backward direction to increase the conc. of $H_2.$

(iv)Adding some $C_2{H}_6$ will move the reaction in backward to decrease the conc. of $C_2{H}_6$ and to remain the reaction in equilibrium.