For a gaseous reaction `2B rarr A`, the equilibrium constant `K_(p)` is ……… to`//`than `K_(c)`.

For a gaseous reaction aA(g)+bB(g)hArrcC(g)+dD(g) equilibrium constants K_(c),K_(p) and K_(x) are K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)),K_(p)=(Pc^(c).P_(D)^(d))/P_(A)^(a)//P_(b)^(b) and Kx=(x_(C)^(c).x_(D)^(d))/(x_(A)^(a).x_(B)^(b) where [A] rarr molar concentration of A,p_(A) rarr partial pressure of A and P rarr total pressure, x_(A) rarr mole fraction of A Select the write option

For a gaseous reaction aA(g)+bB(g)hArrcC(g)+dD(g) equilibrium constants K_(c),K_(p) and K_(x) are represented by the following reation K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)),K_(p)=(Pc^(c).P_(D)^(d))/P_(A)^(a) and Kx=(x_(C)^(c).x_(D)^(d))/(x_(A)^(a).x_(B)^(b) where [A] represents molar concentrationof A,p_(A) represents partial pressure of A and P represents total pressure, x_(A) represents mole fraction of A For the reaction SO_(2)Cl_(2)(g)hArrSO_(2)(g)+Cl_(2)(g),K_(p)gtK_(x) is obtained at :

For a given reversible reaction at a fixed temperature, equilibrium constants K_(p) and K_(c) are related by ………

For a gaseous reaction aA(g)+bB(g)hArrcC(g)+dD(g) equilibrium constants K_(c),K_(p) and K_(x) are represented by the following reation K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)),K_(p)=(Pc^(c).P_(D)^(d))/P_(A)^(a) and Kx=(x_(C)^(c).x_(D)^(d))/(x_(A)^(a).x_(B)^(b) where [A] represents molar concentrationof A,p_(A) represents partial pressure of A and P represents total pressure, x_(A) represents mole fraction of For the following equilibrium relation betwen K_(c) and K_(c) (in terms of mole fraction) is PCl_(3)(g)+Cl_(2)(g)hArrPCl_(5)(g)

Read the following paragraph and answer the questions given below, for a general reaction, aA+bB hArr cC+dD , equilibrium constant K_c is given by K_c=([C]^c[D]^d)/([A]^a[B]^b) However, when all reactants and products are gases the equilibrium constant is generally expressed in terms of partial pressure. K_p=(P_C^cxx P _D^d)/(P_A^axxP_B^b) For a reversible reaction , if concentration of the reactants are doubled, the equilibrium constant will be

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For a general reaction, aA+bB hArr cC+dD , equilibrium constant K_c is given by K_c=([C]^c[D]^d)/([A]^a[B]^b) . However, when all reactants and products are gases the equilibrium constant is generally expressed in terms of partial pressure. K_p=(P_C^cxx P _D^d)/(P_A^axxP_B^b) In which of the following equilibrium will shift forward on addition of inert gas at constant pressure ?

If equilibrium constant for the reaction A_(2)+B_(2) hArr 2AB is k, then for the backward reaction AB hArr 1//2 A_(2)+1//2B_(2) the equilibrium constant k' is 1//K .

For reaction 2A+B hArr 2C, K=x Equilibrium constant for C hArr A+1//2 B will be