For the equilibrium, 2NO2(g)leftharpoons N2O4(g)+14.6 textkcal, increase in temperature

Question

For the equilibrium, 2NO2(g)leftharpoons N2O4(g)+14.6 textkcal, increase in temperature (A) favours the formation of N2O4  (B) favours the decomposition of N2O4  (C) does not affect equilibrium (D) stop the reaction

Tardigrade Admin · Accepted Answer

The given reaction is exothermic and according to Le-Chatelier principle high temperature shifts the equilibrium in backward direction. In other words, high temperature favours the decomposition of N2O4

Q. For the equilibrium, $2 N O_{2} (g) ⇌ N_{2} O_{4} (g) + 14.6 kcal,$ increase in temperature

favours the formation of $N_{2} O_{4}$

favours the decomposition of $N_{2} O_{4}$

does not affect equilibrium

stop the reaction

The given reaction is exothermic and according to Le-Chatelier principle high temperature shifts the equilibrium in backward direction. In other words, high temperature favours the decomposition of $N_{2} O_{4}$

Q. For the equilibrium, 2NO2​(g)⇌N2​O4​(g)+14.6kcal, increase in temperature

favours the formation of N2​O4​

favours the decomposition of N2​O4​