At a given temperature equilibrium is attained when 50% of each reactant is converted into the products
`A(g)+B(g)hArrC(g)+D(g)`
If amount of B(g) is doubled, percentage of B converted into products will be :-

At a particular temp, the following equilibrium is attained when 50% of each reactant is converted into products. A(g)+B(g) iff C(g)+D(g) . If the amount of B in moles in doubled, the % of B converted into products is

At a certain temperature the equilibrium constant K_C is 0.25 for the reaction A(g)+B(g)hArrC(g)+D(g) If we take 1 mole of each of four gases in a 10 litre container , what woluld be the equilibrium concentration of A(g) ?

The K_(c) for given reaction will be A_(2(g))+2B_((g))hArrC_((g))+2D_((g))

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

At a certain temperature the equilibrium constant K_(c) is 0.25 for the reaction A_(2)(g)+B_(2)(g)hArrC_(2)(g)+D_(2)(g) If we take 1 mole of each of the four gases in a 10 litre container ,what would be equilibrium concentration of A_(2) (g)?

Show the rate of the following reaction in terms of partial pressure of the reactants and the products. 2A(g) rarr 2B(g) + C(g)

In the following reaction, 3A (g)+B(g) hArr 2C(g) +D(g) , Initial moles of B is double at A . At equilibrium, moles of A and C are equal. Hence % dissociation is :