In a reversible reaction,K_c K_p and Delta | vedclass

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

Question

(A) For a reversible reaction,the relationship between $K_p$ and $K_c$ is $K_p = K_c(RT)^{\Delta n}$.Given $K_c > K_p$,it implies that $(RT)^{\Delta n

Vedclass · Accepted Answer

Decrease in pressure and temperature

Vedclass · Answer

(A) For a reversible reaction,the relationship between $K_p$ and $K_c$ is $K_p = K_c(RT)^{\Delta n}$.Given $K_c > K_p$,it implies that $(RT)^{\Delta n} $A$ negative $\Delta n$ indicates that the number of moles of gaseous products is less than the number of moles of gaseous reactants.According to Le Chatelier's principle,an increase in pressure shifts the equilibrium towards the side with fewer moles,favoring the product.Conversely,a decrease in pressure will shift the equilibrium towards the reactant side,resulting in less product formation.Given $\Delta H = +40 \, kcal$,the reaction is endothermic.According to Le Chatelier's principle,an increase in temperature favors the endothermic direction (product side).Conversely,a decrease in temperature will shift the equilibrium towards the reactant side,resulting in less product formation.Therefore,a decrease in both pressure and temperature will result in less product formation.

In a reversible reaction,$K_c > K_p$ and $\Delta H = +40 \, kcal$. The formation of product will be less at:

Similar Questions

The equilibrium $SO_2Cl_{2(g)} \rightleftharpoons SO_{2(g)} + Cl_{2(g)}$ is attained in a closed vessel at $25 \, ^\circ C$. If an inert gas,$He$,is added at constant volume,which of the following statement$(s)$ is/are correct?

For the reaction: $A + B + Q \rightleftharpoons C + D$,if the temperature is increased,then the concentration of the products will

What happens when pressure is increased on the equilibrium system $Ice \rightleftharpoons Water$?

In which of the following systems will doubling the volume of the container cause a shift to the right?

Consider the heterogeneous equilibrium in a closed container:
$NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$
If more $NH_4HS_{(s)}$ is added to the equilibrium,what will be the effect on the system?

Vedclass Test Series

Exam Paper Generator

Online Exam Module