The equilibrium constant for the following reaction is `1.6xx10^(5)` at `1024k`
`H_(2)(g)+Br_(2)(g)hArr2HBr(g)`
Find the equilibrium pressure of all gases if `10.0` bar of `HBr` is introdued into a sealed container at `1024K`.

If the equilibrium constant for the reaction, H_(2)(g) +I_(2)(g) hArr 2HI(g) is K What is the equilibrium constant of HI(g) rarr 1/2 H_(2)(g) + 1/2I_(2)(g) ?

The equilibrium constant for the given reaction is 100. N_(2)(g) + 2O_(2)(g) hArr 2NO_(2)(g) What is the equilibrium constant for the reaction given below? NO_(2)(g) hArr 1/2 N_(2)(g) + O_(2)

For the following reaction NH_(4)HS_((s)) harr NH_(3(g))+H_(2)S_((g)) the total pressure at equilibrium is 30 atm. The value of K_(P) 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)

Define equilibrium constant. Write the equilibrium constant expression for the reaction of H_(2)(g)+I_(2)(g)hArr2HI(g) and its reverse reaction. How are the two equilibrium constants related?

In the reaction C_((s)) + CO_(2(g)) hArr CO_(2(g)) , the equilibrium pressure is 6.75 atm. If 50% of CO_(2) reacts then the find value of K_(p) .

The equilibrium constant for the reaction , H_(2) (g) + CO_(2) (g) hArr H_(2) O (g) + CO (g) is 16 at 1000^(@) C . If 1.0 mole of H_(2) and 1.0 mole of CO_(2) are placed in one litre flask , the final equilibrium concentration of CO at 1000^(@) C is

For the reaction, 0.5 C(s)+0.5CO_(2)(g) hArr CO(g) the equilibrium pressure is 12 atm. If CO_(2) conversion is 50%, the value of K_(p) , in atom is

The equilibrium constant for the reaction: N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) at 725K is 6.0xx10^(-2) . At equilibrium [H_(2)]=0.25 "mol" L^(-1) and [NO_(3)]=0.06 "mol" L^(-1) Calculate the equilirbium concentration of N_(2) .