What would be the effect of increasing the volume of each of the following system on its equilibrium. 1. 2CO(.g.)+O2(.g.)leftharpoons2CO2(.g.) 2. N2O4(.g.)leftharpoons2NO2(.g.)

Question

What would be the effect of increasing the volume of each of the following system on its equilibrium. 1. 2CO(.g.)+O2(.g.)leftharpoons2CO2(.g.) 2. N2O4(.g.)leftharpoons2NO2(.g.) (A) 1 in forward and 2 in backward (B) both forward (C) both backward (D) 1 is backward and 2 in forward direction

Tardigrade Admin · Accepted Answer

Increasing volume will result in the decreases of concentration of all gases as per Le-Chatelier principle, the reaction should move in a direction of increases in total number of gaseous moles. Thus shift is in a direction of Δ ng>0 .

Q. What would be the effect of increasing the volume of each of the following system on its equilibrium.

$1.$ $2 CO (g) + O_{2} (g) ⇌ 2 C O_{2} (g)$

$2.$ $N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)$

1 in forward and 2 in backward

both forward

both backward

1 is backward and 2 in forward direction

Increasing volume will result in the decreases of concentration of all gases as per Le-Chatelier principle, the reaction should move in a direction of increases in total number of gaseous moles. Thus shift is in a direction of $Δ n_{g} > 0$ .

Q. What would be the effect of increasing the volume of each of the following system on its equilibrium. 1. 2CO(g)+O2​(g)⇌2CO2​(g) 2. N2​O4​(g)⇌2NO2​(g)