The equilibrium constants of a reaction at `27^(@)C` and aet `127^(@)C` are `1.6xx10^(-3)` and `7.6xx10^(-2)` respectively. Is the reaction exothermic or endothermic?

The rate constants for a reaction at 400 K and 500 K are 2 . 60 xx 10^(-5) s^(-1) and 2.60 xx 10^(-3) s^(-1) respectively. The activation energy of the reaction in kJ mol^(-1) is

For the formation of NH_3 from H_2 at 500 K, The concentration of N_2, H_2 and NH_3 at equilibrium are 1.5xx10^(-2) M , 3.0 x 10^(-2) M and 1.2 xx 10^(-2) M , respectively. The equilibrium constant for the reverse reaction is

The dissociation constants of H_(2)O, H_(2)S, H_(2)Se are 1.8xx10^(-6),1.4xx10^(-16), 1.3xx10^(-7) and 2.2xx10^(-5) , respectively. What do these values denote?

For the formation of NH_(3) from N_(2) and H_(2) at 500 K, the concentration of N_(2), H_(2) and NH_(3) at equilibrium are 1. 5xx10^(-2) M and 1.2xx10^(-2)M, respectively. The equilibrium constant for the reverse reaction is

The equilibrium constant of the reaction, SO_(2)(g) + 1/2 O_(2)(g) hArr 2SO_(3)(g) is 5 xx 10^(-2)atm . The equilibrium constant of the reaction, 2SO_(3)(g) hArr 2SO_(2)(g) + O_(2)(g)

A mixture of 1.57 mol of N_(2) , 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20L reaction vessel at 500K . At this temperature, the equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium ? If not, what is the direction of the net reaction ?