At a particular temperature, the value of `K_(p)` is 100 for the reaction, `2NO(g)hArrN_(2)(g)+O_(2)(g)` occurring in a closed container. If the iniital pressure of `NO(g)` be 25 atm then calculate the partial pressures of NO, `N_(2) and O_(2)` at equilibrium.

At a given temperature, K_(p) is 0.36 for the reaction, 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) occurring in a closed vessel. If at equilibrium, the partial pressures of SO_(2)(g)&O_(2)(g) be 0.15 atm & 0.8 atm respectively, then calculate the partial pressure of SO_(3)(g) .

For the reaction 2NO_(2(g))hArrN_(2)O_(4(g)),K_(p)//K_(c) is equal to

For the reaction 2NO_(2(g))hArrN_(2)O_(4(g)),K_(p)//K_(c) is equal to

In the reaction 2NO(g) hArr N_(2)(g)+O_(2)(g) , the values of K_(c) and K_(p) are ……….. at a given temperature.

In the reaction 2NO(g) hArr N_(2)(g)+O_(2)(g) , the values of K_(c) and K_(p) are ……….. at a given temperature.

A sample of pure NO_2 gas heated to 1000 K decomposes : 2NO_2(g) hArr 2NO(g)+O_(2)(g) The equilibrium constant K_P is 100 atm. Analysis shows that the partial pressure of O_2 is 0.25 atm. At equilibrium.The partial pressure of NO_2 at equilibrium is:

For the reaction, N_(2)O_(4)(g)hArr 2NO_(2)(g) the degree of dissociation at equilibrium is 0.l4 at a pressure of 1 atm. The value of K_(p) is