One mole of helium (He) gas is added to the equilibrium `N_2O_4(g) hArr 2NO_2(g)` set up in cylinder fitted with piston in such a way that the piston is moved outwards to keep the total equilibrium pressure constant:

Consider the following equilibrium system: SO_2(g)+1/2O_2(g)hArr SO_3(g) set up in a cylinder fitted with a piston. Some inert gas is added and the piston is moved outwards to keep the total gaseous pressure constant. Predict which of the following is true?

If Ar is added to the equilibrium N_2(g) +3H_2(g) hArr 2NH_3 at constant volume , the equilibrium will

If Ar is added to the equilibrium N_2(g) +3H_2(g) hArr 2NH_3 at constant volume , the equilibrium will

18.4 g of N_(2)O_(4) is taken in a 1 L closed vessel and heated till the equilibrium is reached. N_(2)O_(4(g))hArr2NO_(2(g)) At equilibrium it is found that 50% of N_(2)O_(4) is dissociated . What will be the value of equilibrium constant?

For the equilibrium reaction 2NO_2(g) hArr N_2O_4(g) + 60.0 kJ the increase in temperature

For the following equilibrium reaction , N_2O_4(g) hArr 2NO_2(g) NO_2 is 50% of total volume at given temperature . Hence vapour density of the equilibrium mixture is

Pressure has no influence in the following equilibrium: N_2(g)+O_2(g)harr2NO_(g) . What is the reason for this?