`A(s) harr M(s) + 1/2O_2(g)`
`K_p` of the reaction is 4. Find the partial pressure of `O_2` at equilibrium

The value of K_p for the reaction, 2SO_2(g)+O_2(g) hArr 2SO_3(g) is 5 what will be the partial pressure of O_2 at equilibrium when equal moles of SO_2 and SO_3 are present at equilibrium ?

The equilibrium constant for the reaction A (s) hArr M (s) + (1)/(2) O _(2) (g) is K _(P) = 4. At equilibrium, the partial pressrue of O _(2) is __________ atm. (Round off to the nearest integer)

The equilibrium constant K_p for the reaction 2SO_(2)+O_(2) Leftrightarrow 2SO_(3) is 2.5 atm ""^(-1). What would be the partial pressure of O_2 at equilibrium. If the equilibrium pressures of SO_(2) and SO_(3) are equal

The equilibrium constant, K_(p) for the reaction 2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) is 44.0atm^(-1) "at" 1000 K . What would be the partial pressure of O_(2) if at equilibrium the amound of SO_(2) and SO_(3) is the same?

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:

Calculate the equilibrium constant K_(p) and K_(c ) for the reaction: CO(g)+1//2O_(2)(g) hArr CO_(2)(g) . Given that the partial pressure at equilibrium in a vessel at 3000 K are p_(CO)=0.4 atm, p_(CO_(2))=0.2 atm