[" 57.Equilibrium is established in the reactior "],[A+B rightleftharpoons C+D" with "K_(c)=10.0" at this point."]

A(G)+B(g)hArrC(g)+D(g) Above equilibrium is established by taking A& B in a closed container. Initial concentration of A is twice of the initial concentration of B. At equilibrium concentraons of B and C are equal. Then find the equilibrium constant for the reaction, C(g)+D(g)hArrA(g)+B(g) .

The unit of equilibrium constant K_(c) for the reaction A+B hArr C would be

The unit of equilibrium constant K_(c) for the reaction A+B hArr C would be

In a system. A(s)+B(g)+ Heat rarr 2C(s)+2D(g) equilibrium is established. The pressure of B vapour is doubled to re - stablish the equilibrium. The factor by which D is changed is :

For a reaction, aA+bBhArrcC+dD , the reaction quotient Q=([C]_(0)^(c)[D]_(0)^(d))/([A]_(0)^(a)[B]_(0)^(b)) , where [A]_(0) , [B]_(0) , [C]_(0) , [D]_(0) are initial concentrations. Also K_(c)=([C]^(c)[D]^(d))/([A]^(a)[B]^(b)) where [A] , [B] , [C] , [D] are equilibrium concentrations. The reaction proceeds in forward direction if Q lt K_(c) and in backward direction if Q gt K_(c) . The variation of K_(c) with temperature is given by: 2303log(K_(C_(2)))/(K_(C_(1)))=(DeltaH)/(R)[(T_(2)-T_(1))/(T_(1)T_(2))] . For gaseous phase reactions K_(p)=K_(c)(RT)^(Deltan) where Deltan= moles of gaseous products - moles of gaseous reactants. Also -DeltaG^(@)=2.303RT log_(10)K_(c) . Which relation is correct?

What is equilibrium constant? Establish the relation between K_p and K_c for a reversible reaction in equilibrium.