Chemical EquilibriumHard
Question
At constant temperature, the equilibrium constant (Kp) for the decomposition reaction N2O4 $\rightleftharpoons$ 2NO2 is expressed by $K_{p} = \frac{4x^{2}P}{1 - x^{2}}$, where P = total pressure at equilibrium, x = extent of decomposition. Which one of the following statements is true?
Options
A.Kp increases with increase of P.
B.Kp increases with increase of x.
C.Kp increases with decrease of x.
D.Kp remains constant with change in P and x.
Solution
Equilibrium constant is a function of temperature only.
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
One mole of pure PCl5 is placed in an evacuated container and maintained at 250°C. The equilibrium is established at tot...Indicate the correct answer out of the following for the below reaction. NH4Cl + H2O$\rightleftharpoons$NH4OH + HCl...XY2 dissociates XY2(g) ⇋ XY(g) + Y(g). When the initial pressure of XY2 is 600 mm Hg, the total equilibrium pressu...The equilibrium constant for the reaction 3C2H2 $\rightleftharpoons$C6H6 is 4.0 at T K. If the equilibrium concentration...The Haber’s process for the manufacture of ammonia is usually carried out at about 500oC. If a temperature of about 250o...