In which of the following reactions will the | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) According to Le Chatelier's principle,for a gaseous reaction,increasing the pressure shifts the equilibrium towards the side with a smaller number

Vedclass · Accepted Answer

$N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$

Vedclass · Answer

(A) According to Le Chatelier's principle,for a gaseous reaction,increasing the pressure shifts the equilibrium towards the side with a smaller number of moles of gaseous species.If the number of moles of gaseous reactants equals the number of moles of gaseous products (i.e.,$\Delta n_g = 0$),then the pressure change has no effect on the equilibrium position.In reaction $(A)$: $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$,the number of moles of gaseous reactants is $1 + 1 = 2$ and the number of moles of gaseous products is $2$. Thus,$\Delta n_g = 2 - 2 = 0$.Therefore,increasing the pressure will not shift the equilibrium and the amount of products will not increase.

In which of the following reactions will the amount of products not increase upon increasing the pressure?

Similar Questions

What would happen to a reversible reaction at equilibrium when an inert gas is added while the pressure remains unchanged?

For a reaction,the value of $K_p$ increases with an increase in temperature. The $\Delta H$ for the reaction would be

State Le Chatelier's Principle.

For the reaction $N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)} + 21.9 \ kcal$,which conditions favor the production of ammonia?

Vedclass Test Series

Exam Paper Generator

Online Exam Module