`(K_(p))/(K_(c))` for `N_(2)+3H_(2)iff``2NH_(3)` (gaseous phase) at `400K` is

K_(c) for the reaction N_(2)+3H_(2) hArr 2NH_(3) is 0.5 mol^(-2) L^(2) at 400 K . Find K_(p) . Given R=0.082 L-"atm deg"^(-1) mol^(-1)

The value of K_(c ) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 0.50 at 400^(@)C . Find the value of K_(p) at 400^(@)C when concentrations are expressed in mol L^(-1) and pressure in atm.

K_(p) for the reaction, N_(2)+3H_(2)hArr2NH_(3) is 1.6xx10^(-4)atm^(-2) at 400^(@)C . What will be K_(p) at 500^(@)C ? Heat of reaction in this temperature range is -25.14 kcal .

K_(p) for the reaction N_(2)+3H_(2) hArr 2NH_(3) at 400^(@)C is 1.64xx10^(-4) . Find K_(c) . Also find DeltaG^(ɵ) using K_(p) and K_(c) values and interprest the difference.

N_(2)+3H_(2)hArr 2NH_(3) . This is gaseous phase reaction taking place in 1L flask at 127^(@)C . Starting with 1 mole N_(2) and 3 moles H_(2) , equilibrium required 500mL of 1M HCl. Hence K_(c) is approximately

K_(p) for the reaction N_(2)+3H_(2) hArr 2NH_(3) is 1.6xx10^(-4) atm^(-2) at 400^(@)C . What will be K_(p) at 500^(@)C ? The heat of reaction on this temperature is -25.14 kcal?

At 450^(@)C the equilibrium constant K_(p) for the reaction N_(2)+3H_(2) hArr 2NH_(3) was found to be 1.6xx10^(-5) at a pressure of 200 atm. If N_(2) and H_(2) are taken in 1:3 ratio. What is % of NH_(3) formed at this temperature?

Write the relation between K_(p) " and " K_(c) for the reaction: N_(2)(g) +3H_(2) (g) hArr 2NH_(3)(g)