`K_(p)` for the reaction `A hArr B` is 4. If initially only A is present then what will be the partial pressure of B after equilibrium ?

K_p for the reaction AtoB is 4. If initially only A is present then what will be the partial pressure of B after equilibrium-

The K_(p) value for the reaction. H_(2) +I_(2) hArr 2Hi at 460^(@)C is 49. If the initial pressure of H_(2) " and " I_(2) is 0.5 atm respectively , what will be the partial pressure of H_(2) at equilibrium ?

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

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

The equilibrium constant, K_(p) for the reaction 2SO_(2)(g)+O_(2)(g)hArr 2SO_(3)(g) is 4.0 atm^(-1) at 1000 K. What would be the partial pressure of SO_(2) if at equilibrium the amount of SO_(2) and SO_(3) is the same ?

For a reaction A(g) hArr B(g) at equilibrium . The partial pressure of B is found to be one fourth of the partial pressure of A . The value of DeltaG^(@) of the reaction A rarrB is

The equilibrium constant K_(p_(2)) and K_(p_(2)) for the reactions A hArr 2B and P hArr Q+R , respectively, are in the ratio of 2:3 . If the degree of dissociation of A and P are equal, the ratio of the total pressure at equilibrium is,