For the reaction `A+3B hArr 2C+D` initial mole of A is twice that of B . If at equilibrium moles of B and C are equal , then percent of B reacted is

A+3B harr 2C+D For this hypothetical reaction, initial moles of A is twice that of B. If at equilibrium, moles of B and C are equal, the percent of B reacted is :

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 :

A+B rarr C+D Initially moles of A and B are equal. At equilibrium, moles of C are three times of A. The equilibrium constant of the reaction will be

For the reaction A + 2B to C, 5moles of A and 8moles of B will produce :-

In a gaseous reaction A+2B iff 2C+D the initial concentration of B was 1.5 times that of A. At equilibrium the concentration of A and D were equal. Calculate the equilibrium constant K_(C) .