Calculate the equilibrium constant Kc for the reaction:2XY(g) ⇌2X (s) + Y2(g)When the number of moles of XY, X2, Y2 : 0.8 ,0.4 & 0.2 moles respectively, put in container of volume = 4L .

The equilibrium constant, KC, for the following reaction is 280 at 1,000 K.2SO2(g) + O2(g) ⇌ 2SO3(g)If [SO2]eq = 0.80 M and [O2]eq = 0.35 M, then [SO3]eq = 6.2 × 10-27.9262.72792 M.

For the reaction ⇌+2H2gS2g2H2Sg, determine the equilibrium constant at 700°C if at this temperature, the equilibrium concentrations are as follows: [H2] = 0.208 M, [S2] = 1.13 × 10-6 M, [H2S] = 0.725 M

The equilibrium constant, KC, for the following reaction is 2.5 × 10-3N2(g) + O2(g) ⇌ 2NO(g)If [N2]eq = 0.75 M and [NO]eq = 0.090, then [O2]eq

One mole each of 2NO (g) and 2 4N O (g)were mixed in a 1 3dm flask and allowed toequilibrate. The following equilibrium wasestablished : 32 2 42NO (g) N O (g)If at equilibrium the reaction mixturecontained 0.75 moles of 2 4N O (g) , calculatethe value of equilibrium constant ck for thereaction

Write the expression for equilibriumconstant, pk for the reaction :+ 2 22NO (g) O (g) 2NO (g)in terms of :(i) partial pressure and(ii) mole fraction of the gaseous species