Derve the relation `K_(p)=K_(c)(RT)^(Deltan_(g))` for a general chemical equilibrium reaction.

For the reaction : N_(2)O_(4)(g)hArr 2NO_(2)(g) the concentration of the equilibrium mixture at 300 K are [N_(2)O_(4)]=4.8xx10^(-2)mol L^(-1) and [NO_(2)]=1.2xx10^(-2)mol L^(-1). K_(c ) for the reaction is :

Write the relation between standard free energy change and equilibrium constant K_(p) for a reversible reaction.

The relationship between K_(p) and K_(c ) is K_(p) = K_(c ) (RT) Delta n . What would be the value of Deltan for the reaction NH_(4) Cl (s) hArr NH_(3) (g) + HCl(g) ?

At a certain temperature and a total pressure of 10^(5) Pa, iodine vapours contain 40% by volume of iodine atoms. I_(2)(g) hArr 2I(g) K_(p) for the equilibrium reaction is :

For the equilibrium 2NOCl_((g))hArr2NO_((g))+Cl_(2(g)) the value of the equilibrium constant K_(c) is 3.75xx10^(-6) at 790^(@)C . Calculate K_(p) for this equilibrium at the same temperature.

For the reaction : NH_(2)COONH_(4)(g) hArr 2NH_(3)(g)+CO_(2)(g) equilibrium pressure was found to be 3 atm at 1000 K. K_(p) is :

Give an example of reaction where K_p=K_c