For which equation is the equilibrium constant equal to `K_a` for the ammonium ion, `NH_4^+`?

For a system in equilibrium, the rate constant for the forward reaction is represented by K_f and the rate constant for the reverse reaction is represented by K_r .Which equation represents the equilibrium constant for this reaction in the forward direction ?

In an equilibrium reaction for which DeltaG^(ɵ)=0 , the equilibrium constant K should be equal to :

In an equilibrium reaction for which DeltaG^(ɵ)=0 , the equilibrium constant K should be equal to :

Write the correctly balanced net ionic equations for the reations whose equilibrium constant at 298 K are K_b ( CH_3NH_2)= 4.4 xx 10^(-5)

Passage: When all the coefficients in a balanced chemical equation are multiplied by a constant factor X the equilibrium constant (originally K) becomes K^J . Similarly, when balanced equations are added together, the equilibrium constant for the combined process is equal to the product of the equilibrium constants for each step. Equilibrium constant of the reversed reaction is numerically equal to the reciprocal of the equilibrium constant of the original equation. Unit of K_p = ("atm")^(Deltan) , Unit of K_c =("mol" L^(-1))^(Deltan) Consider the two reactions: XeF_(6(g))+H_(2)O_((g)) harr XeOF_(4(g))+2HF_((g)), K_(1)" "XeO_(4(g))+XeF_(6(g)) harr XeOF_(4(g))+XeO_(3)F_(2(g)), K_(2) Then the equilibrium constant for the following reaction will be XeO_(4(g))+2HF_((g)) harr XeO_(3)F_(2(g))+H_(2)O_((g))

Ammonium hydrogen sulphide dissociates according to the equation : NH_4 HS(s) hArr NH_3(g)+H_2S(g) The total pressure at equilibrium at 400 K is found to be 1 atm.The equilibrium constant K_p of the reaction is :

Which is the constant equation for hydrolysis constant of NH_(4)CN ?

Which is the constant equation for hydrolysis constant of NH_(4)CN ?